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Describe an acidic buffer solution.

An acidic buffer solution is made from a weak acid and a salt of that weak acid.

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"Describe an acidic buffer solution."	"An acidic buffer solution is made from a weak acid and a salt of that weak acid."
"How do buffer solutions work?"	"In a buffer solution, there is a higher concentration of the salt ion than in the pure acid or base. This allows the ratio of the conjugate acid/base to stay constant, keeping the pH fairly constant."
"What happens when small amounts of acid are added to a buffer solution?"	"The equilibrium will shift to the left, removing nearly all the H+ ions added, due to the high concentration of the salt ion in the buffer."
"What happens when small amounts of alkali are added to a buffer solution?"	"The OH- ions will react with H+ ions to form water, causing the equilibrium to shift to the right and produce more H+ ions."
"Describe the process of calculating the pH of buffer solutions."	"The pH of buffer solutions can be calculated using the weak acid dissociation expression and considering the initial concentration of the acid and salt. The salt content can be added through a salt solution or by partially neutralizing a weak acid with alkali."
"What is the purpose of assuming the [A-] concentration in buffer solutions?"	"Assuming the [A-] concentration allows us to rearrange the weak acid dissociation expression and calculate the pH of the buffer solution."
"Define a buffer solution."	"A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. It is made by combining a weak acid and its conjugate base or a weak base and its conjugate acid."
"How can a buffer solution be made by adding a solid salt?"	"A buffer solution can be made by adding a solid salt, such as sodium ethanoate, to a solution of a weak acid, such as ethanoic acid. The salt dissociates to provide the conjugate base, which helps maintain the pH of the solution."
"Describe the process of making a buffer solution by adding sodium hydroxide to partially neutralize a weak acid."	"To make a buffer solution by adding sodium hydroxide, the weak acid is partially neutralized by reacting it with sodium hydroxide. The moles of the weak acid in excess and the moles of the conjugate base formed are used to calculate the pH of the resulting buffer solution."
"Describe the process of calculating change in pH of a buffer on addition of a small amount of acid or alkali."	"When a small amount of alkali is added to a buffer, the moles of the buffer acid decrease by the number of moles of alkali added, while the moles of salt increase by the same amount. The pH can then be recalculated with the new values. The same principle applies when a small amount of acid is added, but in this case, the moles of the buffer salt decrease and the moles of buffer acid increase."
"How can the pH of a buffer solution be calculated after the addition of a small amount of NaOH?"	"The moles of acid and salt in the buffer solution before and after the addition of NaOH are determined. The moles of acid decrease by the amount of NaOH added, while the moles of salt increase. The pH can then be calculated using the new values."
"What happens to the pH a buffer solution when it is diluted with water?"	"Diluting a buffer solution with water does not change its pH. This is because the ratio of [HA]/[A-] in the buffer equation remains constant as both the concentrations of salt and acid are diluted by the same proportion."
"Describe the process of constructing a pH curve."	"Transfer 25cm³ of acid to a conical flask with a volumetric pipette. Measure the initial pH of the acid with a pH meter. Add alkali in small amounts, stirring the mixture to equalize the pH. Measure and record the pH. Repeat the process with smaller volumes of alkali when approaching the endpoint."
"What is the purpose of calibrating a pH meter?"	"Calibrating a pH meter is necessary because pH meters can lose accuracy on storage."
"Define the equivalence point in a titration curve."	"The equivalence point in a titration curve is the point at which the stoichiometrically equivalent amounts of acid and base have reacted."
"Describe the general shape of a titration curve for a weak acid and a strong base."	"At the start, the pH rises quickly and then levels off. The flattened part is called the buffer region and is formed because a buffer solution is made."
"How can the accuracy of pH probes be improved?"	"The accuracy of pH probes can be improved by maintaining a constant temperature."
"Describe the difference between a weak acid and a weak base."	"A weak acid is an acid that does not completely dissociate in water, while a weak base is a base that does not completely ionize in water."
"Define pH."	"pH is a measure of the acidity or alkalinity of a solution. It is a logarithmic scale that ranges from 0 to 14, with 7 being neutral, values below 7 indicating acidity, and values above 7 indicating alkalinity."
"What is the purpose of choosing an indicator in a titration?"	"The purpose of choosing an indicator in a titration is to visually determine the endpoint of the reaction, which is when the color of the indicator changes and indicates that the reaction is complete."
"How do indicators work in a titration?"	"Indicators can be considered as weak acids. They have a different color in their acidic form (Hln) compared to their conjugate base form (In). The color change of the indicator corresponds to a specific pH range, allowing for the determination of the endpoint of the titration."
"Describe the relationship between pH and the equilibrium of an indicator in an acid solution."	"In an acid solution, the presence of H+ ions pushes the equilibrium of the indicator towards the reactants. This results in the indicator having a specific color, known as the acidic color."
"Describe how to calculate the concentration of a weak acid given its pH."	"To calculate the concentration of a weak acid with a given pH, we can use the K2 expression and the known Ka value. First, we take the negative logarithm of the given pH to find [H+]. Then, we substitute [H+] into the K2 expression and solve for [HA]."
"Define a Bronsted-Lowry base."	"A Bronsted-Lowry base is a substance that can accept a proton."
"What is the equation for calculating pH?"	"pH = - log [H+]"
"How do you calculate the pH of strong acids?"	"The concentration of hydrogen ions in a monoprotic strong acid will be the same as the concentration of the acid."
"Describe the ionic product for water."	"In all aqueous solutions and pure water, the equilibrium H2O (I) H+ (aq) + OH- (aq) occurs."
"What is the value of Kw for all aqueous solutions at 25°C?"	"Kw = 1x10-14 mol2dm-6"
"What is the pH of pure water at 25°C?"	"pH = 7"
"Describe how to calculate the pH of a strong base."	"To calculate the pH of a strong base, we need to work out the concentration of the hydroxide ion and assume complete dissociation. Then, we can use the Kw expression to find [H+(aq)]. Finally, we take the negative logarithm of [H+(aq)] to obtain the pH value."
"Define complete dissociation for strong bases."	"Complete dissociation refers to the process in which strong bases completely break apart into their ions when dissolved in water."
"Describe the dissociation expression for weak acids."	"The dissociation expression for weak acids can be represented as HA (aq) -> H+ (aq) + A- (aq), where HA is the undissociated acid and H+ and A- are the dissociated ions."
"What is the pKa value and how is it related to Ka?"	"The pKa value is the negative logarithm of the Ka value. It is used to express the acidity of a weak acid. The larger the pKa value, the weaker the acid."
"How can the pH of a weak acid be calculated?"	"To calculate the pH of a weak acid, we can make two assumptions: 1) [H+] is equal to the concentration of the dissociated ions [H+(aa)] and 2) the initial concentration of the undissociated acid [HA] remains constant. Then, we can use the K2 expression and take the negative logarithm of [H+] to find the pH value."
"Describe the Bronsted-Lowry definition of acid."	"A Bronsted-Lowry acid is a substance that can donate a proton."
"Describe pH calculations involving neutralisation reactions."	"pH calculations involving neutralisation reactions can be complex, especially when determining the pH of a partially neutralised acid or a solution with excess alkali. The method used depends on whether the acid is strong or weak in the partially neutralised case."
"Define strong acid and strong base neutralisations."	"Strong acid and strong base neutralisations involve the reaction between a strong acid and a strong base to form water and a salt. The pH of the resulting mixture can be calculated by determining the concentration of excess H+ or OH- ions."
"How do you calculate the new concentration of excess H+ ions in a strong acid and strong base neutralisation?"	"To calculate the new concentration of excess H+ ions in a strong acid and strong base neutralisation, divide the moles of excess H+ ions by the total volume of the solution (in dm³)."
"Describe the process of determining which ion is in excess in a strong acid and strong base neutralisation."	"To determine which ion is in excess in a strong acid and strong base neutralisation, calculate the concentration of excess H+ and OH- ions separately. The ion with the higher concentration is the one in excess."
"Do strong diprotic acids and bases affect pH calculations differently?"	"Yes, strong diprotic acids and bases, such as H2SO4 and Ba(OH)2, can affect pH calculations differently. The number of moles of H+ or OH- ions produced will be twice the number of moles of the diprotic acid or base used."
"Describe the process of calculating the new concentration of excess HA in a weak acid and strong base neutralization."	"The new concentration of excess HA can be calculated by subtracting the moles of OH- from the initial moles of HA and dividing by the total volume."
"What is the formula to calculate the concentration of salt formed [A-] in a weak acid and strong base neutralization?"	"The concentration of salt formed [A-] can be calculated by dividing the moles of OH- added by the total volume."
"Define pH and how it is calculated in a weak acid and strong base neutralization."	"pH is a measure of the acidity or alkalinity of a solution. In a weak acid and strong base neutralization, pH can be calculated using the formula pH = -log[H+]."
"Describe the process of calculating the pH of a resulting mixture in a specific example of weak acid and strong base neutralization."	"In the given example, the pH of the resulting mixture can be calculated by rearranging the equation Ka=[H+][A-] to get [H+], and then substituting the values to find the pH."
"How can the pH of a weak acid at half equivalence be simplified?"	"At half equivalence, the assumption can be made that [HA] = [A-]. Therefore, [H+(aq)] = K2 and pH = pKa."

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Describe an acidic buffer solution.

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An acidic buffer solution is made from a weak acid and a salt of that weak acid.

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[{"id":977854,"front":"Describe an acidic buffer solution.","back":"An acidic buffer solution is made from a weak acid and a salt of that weak acid.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"An acidic buffer solution is created by combining a weak acid with a salt of that weak acid. The weak acid provides the acidic component, while the salt acts as a source of the conjugate base. This combination allows the solution to resist changes in pH when small amounts of acid or base are added. The weak acid can donate protons to neutralize any added base, while the conjugate base can accept protons to neutralize any added acid. This maintains the overall acidity of the solution and keeps the pH relatively stable.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977856,"front":"How do buffer solutions work?","back":"In a buffer solution, there is a higher concentration of the salt ion than in the pure acid or base. This allows the ratio of the conjugate acid/base to stay constant, keeping the pH fairly constant.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":1,"explanation":"Buffer solutions work by maintaining a relatively constant pH. They achieve this by having a higher concentration of the salt ion compared to the pure acid or base. This higher concentration allows the ratio of the conjugate acid/base to remain constant, which helps to resist changes in pH when small amounts of acid or base are added. In other words, buffer solutions act as a reservoir of both the acid and base components, allowing them to neutralize any added acid or base and maintain the pH within a desired range.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977864,"front":"What happens when small amounts of acid are added to a buffer solution?","back":"The equilibrium will shift to the left, removing nearly all the H+ ions added, due to the high concentration of the salt ion in the buffer.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":2,"explanation":"When small amounts of acid are added to a buffer solution, the equilibrium of the system will shift to the left. This occurs because the buffer solution contains a high concentration of the salt ion, which will react with the added H+ ions. As a result, the H+ ions will be removed from the solution, maintaining the pH of the buffer solution and preventing significant changes in acidity.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977867,"front":"What happens when small amounts of alkali are added to a buffer solution?","back":"The OH- ions will react with H+ ions to form water, causing the equilibrium to shift to the right and produce more H+ ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":3,"explanation":"When small amounts of alkali are added to a buffer solution, the OH- ions from the alkali will react with the H+ ions in the buffer solution. This reaction forms water and causes the equilibrium to shift to the right, resulting in the production of more H+ ions. This process helps maintain the pH of the buffer solution and prevents drastic changes in acidity or alkalinity.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977870,"front":"Describe the process of calculating the pH of buffer solutions.","back":"The pH of buffer solutions can be calculated using the weak acid dissociation expression and considering the initial concentration of the acid and salt. The salt content can be added through a salt solution or by partially neutralizing a weak acid with alkali.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":4,"explanation":"Buffer solutions are made up of a weak acid and its conjugate base. The pH of a buffer solution can be calculated by using the dissociation expression of the weak acid and considering the initial concentrations of the acid and its conjugate base. The addition of a salt solution or partially neutralizing a weak acid with an alkali can also contribute to the salt content of the buffer solution.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977872,"front":"What is the purpose of assuming the [A-] concentration in buffer solutions?","back":"Assuming the [A-] concentration allows us to rearrange the weak acid dissociation expression and calculate the pH of the buffer solution.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":5,"explanation":"Assuming the concentration of [A-] in buffer solutions is essential for calculating the pH. This assumption enables the rearrangement of the weak acid dissociation expression, facilitating the determination of the buffer solution's pH.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977875,"front":"Define a buffer solution.","back":"A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. It is made by combining a weak acid and its conjugate base or a weak base and its conjugate acid.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":6,"explanation":"Buffer solutions are crucial in various fields like biology and chemistry. They help maintain a stable pH, essential for enzyme function and chemical reactions. The key components are a weak acid and its conjugate base or a weak base and its conjugate acid, ensuring the solution can neutralize added acids or bases.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977877,"front":"How can a buffer solution be made by adding a solid salt?","back":"A buffer solution can be made by adding a solid salt, such as sodium ethanoate, to a solution of a weak acid, such as ethanoic acid. The salt dissociates to provide the conjugate base, which helps maintain the pH of the solution.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":7,"explanation":"Adding a solid salt like sodium ethanoate introduces its conjugate base into the solution, which can react with any added acid to maintain the pH. This process helps stabilize the solution's pH, making it a buffer solution.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977881,"front":"Describe the process of making a buffer solution by adding sodium hydroxide to partially neutralize a weak acid.","back":"To make a buffer solution by adding sodium hydroxide, the weak acid is partially neutralized by reacting it with sodium hydroxide. The moles of the weak acid in excess and the moles of the conjugate base formed are used to calculate the pH of the resulting buffer solution.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":8,"explanation":"Creating a buffer solution involves a delicate balance between a weak acid and its conjugate base. By partially neutralizing the weak acid with sodium hydroxide, you establish a system that can resist changes in pH. This equilibrium is crucial for maintaining stability in various chemical and biological processes.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977884,"front":"Describe the process of calculating change in pH of a buffer on addition of a small amount of acid or alkali.","back":"When a small amount of alkali is added to a buffer, the moles of the buffer acid decrease by the number of moles of alkali added, while the moles of salt increase by the same amount. The pH can then be recalculated with the new values. The same principle applies when a small amount of acid is added, but in this case, the moles of the buffer salt decrease and the moles of buffer acid increase.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":9,"explanation":"When a small amount of acid or alkali is added to a buffer, the moles of the buffer acid or salt change accordingly. This change in moles affects the pH of the buffer. Adding alkali decreases the moles of the buffer acid and increases the moles of the buffer salt, leading to a change in pH. Adding acid has the opposite effect, decreasing the moles of the buffer salt and increasing the moles of the buffer acid, resulting in a different pH. The pH can be recalculated using the new mole values to determine the change in pH of the buffer.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977891,"front":"How can the pH of a buffer solution be calculated after the addition of a small amount of NaOH?","back":"The moles of acid and salt in the buffer solution before and after the addition of NaOH are determined. The moles of acid decrease by the amount of NaOH added, while the moles of salt increase. The pH can then be calculated using the new values.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":10,"explanation":"Buffer solutions resist changes in pH due to their composition of weak acids and their conjugate bases. When NaOH is added, it reacts with the weak acid, reducing its concentration while increasing the concentration of the conjugate base. This shift can be quantified using the Henderson-Hasselbalch equation for precise pH calculation.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977892,"front":"What happens to the pH a buffer solution when it is diluted with water?","back":"Diluting a buffer solution with water does not change its pH. This is because the ratio of [HA]/[A-] in the buffer equation remains constant as both the concentrations of salt and acid are diluted by the same proportion.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":11,"explanation":"When a buffer solution is diluted with water, the pH remains constant due to the equilibrium between the weak acid and its conjugate base. The ratio of their concentrations, which determines pH, remains unchanged as both are diluted proportionally. This maintains the buffer's ability to resist pH changes.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977894,"front":"Describe the process of constructing a pH curve.","back":"Transfer 25cm³ of acid to a conical flask with a volumetric pipette. Measure the initial pH of the acid with a pH meter. Add alkali in small amounts, stirring the mixture to equalize the pH. Measure and record the pH. Repeat the process with smaller volumes of alkali when approaching the endpoint.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":12,"explanation":"The process described involves carefully adding alkali to the acid while measuring the pH at each step. This allows for the construction of a pH curve, showing the relationship between the amount of alkali added and the resulting pH. The gradual addition of alkali ensures that the endpoint can be accurately determined.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977896,"front":"What is the purpose of calibrating a pH meter?","back":"Calibrating a pH meter is necessary because pH meters can lose accuracy on storage.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":13,"explanation":"Calibrating a pH meter is important because over time, pH meters can become less accurate due to factors such as aging, exposure to contaminants, or changes in the electrode. Calibration ensures that the pH meter is measuring pH values correctly and provides reliable and accurate results. Without calibration, there is a risk of obtaining incorrect pH readings, which can lead to inaccurate conclusions or decisions based on the data.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977897,"front":"Define the equivalence point in a titration curve.","back":"The equivalence point in a titration curve is the point at which the stoichiometrically equivalent amounts of acid and base have reacted.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":14,"explanation":"The equivalence point is crucial in titrations as it indicates complete neutralization. At this stage, the pH can change rapidly, often leading to a sharp inflection on the curve. Understanding this point helps in determining the concentration of unknown solutions accurately, making it essential for quantitative analysis in chemistry.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977899,"front":"Describe the general shape of a titration curve for a weak acid and a strong base.","back":"At the start, the pH rises quickly and then levels off. The flattened part is called the buffer region and is formed because a buffer solution is made.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":15,"explanation":"The titration curve for a weak acid and a strong base generally starts with a rapid increase in pH as the strong base is added. This is due to the neutralization of the weak acid by the strong base. As the titration progresses, the pH levels off and remains relatively constant. This region is known as the buffer region, where a buffer solution is formed. In this region, the weak acid and its conjugate base act as a buffer, resisting changes in pH. This occurs because the weak acid can donate or accept protons, maintaining a relatively stable pH.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977900,"front":"How can the accuracy of pH probes be improved?","back":"The accuracy of pH probes can be improved by maintaining a constant temperature.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":16,"explanation":"Temperature fluctuations can affect the ionization of the pH-sensitive glass membrane, leading to inaccurate readings. By stabilizing the temperature, the response of the probe becomes more consistent, ensuring that the measurements reflect the true pH of the solution. This is crucial in sensitive applications like biochemical assays.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977902,"front":"Describe the difference between a weak acid and a weak base.","back":"A weak acid is an acid that does not completely dissociate in water, while a weak base is a base that does not completely ionize in water.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":17,"explanation":"A weak acid only partially dissociates in water, releasing fewer hydrogen ions. In contrast, a weak base only partially ionizes in water, producing fewer hydroxide ions. This results in different pH levels and varying effects on solutions they are added to.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977903,"front":"Define pH.","back":"pH is a measure of the acidity or alkalinity of a solution. It is a logarithmic scale that ranges from 0 to 14, with 7 being neutral, values below 7 indicating acidity, and values above 7 indicating alkalinity.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":18,"explanation":"pH plays a crucial role in various chemical processes, biological functions, and environmental systems. For instance, in agriculture, soil pH affects nutrient availability for plants. In aquatic ecosystems, pH influences species diversity and health, highlighting its importance in both natural and human-made environments.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977904,"front":"What is the purpose of choosing an indicator in a titration?","back":"The purpose of choosing an indicator in a titration is to visually determine the endpoint of the reaction, which is when the color of the indicator changes and indicates that the reaction is complete.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":19,"explanation":"Choosing an indicator in a titration is crucial as it allows for the visual detection of the endpoint of the reaction. This is important because it provides a clear signal that the reaction is complete, helping to ensure accurate and precise measurements in the titration process.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977905,"front":"How do indicators work in a titration?","back":"Indicators can be considered as weak acids. They have a different color in their acidic form (Hln) compared to their conjugate base form (In). The color change of the indicator corresponds to a specific pH range, allowing for the determination of the endpoint of the titration.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":20,"explanation":"Indicators play a crucial role in titrations by signaling the completion of a reaction. Their color change occurs at a specific pH, which is linked to the acidity or basicity of the solution. This visual cue helps chemists accurately identify when the reactants have fully reacted, ensuring precise measurements.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977906,"front":"Describe the relationship between pH and the equilibrium of an indicator in an acid solution.","back":"In an acid solution, the presence of H+ ions pushes the equilibrium of the indicator towards the reactants. This results in the indicator having a specific color, known as the acidic color.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":21,"explanation":"In an acid solution, the increase in H+ ions shifts the equilibrium of the indicator towards the reactants, causing it to exhibit a specific color characteristic of acidity. This is due to the impact of pH on the indicator's equilibrium position and its resulting color change.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977824,"front":"Describe how to calculate the concentration of a weak acid given its pH.","back":"To calculate the concentration of a weak acid with a given pH, we can use the K2 expression and the known Ka value. First, we take the negative logarithm of the given pH to find [H+]. Then, we substitute [H+] into the K2 expression and solve for [HA].","front_language":"English","back_language":"English","front_image":"","back_image":"","order":22,"explanation":"Calculating the concentration of a weak acid from its pH involves using the dissociation constant (Ka) and the relationship between the concentration of the acid, its conjugate base, and the hydrogen ion. By manipulating the Ka expression and the pH, the concentration of the weak acid can be determined.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977798,"front":"Define a Bronsted-Lowry base.","back":"A Bronsted-Lowry base is a substance that can accept a proton.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":23,"explanation":"A Bronsted-Lowry base is characterized by its ability to receive a proton, which is a positively charged hydrogen ion (H+). This definition distinguishes it from a Bronsted-Lowry acid, which donates a proton. Understanding these concepts is fundamental in acid-base chemistry.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977800,"front":"What is the equation for calculating pH?","back":"pH = - log [H+]","front_language":"English","back_language":"English","front_image":"","back_image":"","order":24,"explanation":"The pH scale measures the acidity or basicity of a solution, with lower values indicating higher acidity. The logarithmic nature of the equation reflects how small changes in hydrogen ion concentration can lead to significant shifts in pH, highlighting the sensitivity of chemical systems to ion concentration.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977804,"front":"How do you calculate the pH of strong acids?","back":"The concentration of hydrogen ions in a monoprotic strong acid will be the same as the concentration of the acid.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":25,"explanation":"The pH of a strong acid can be calculated by determining the concentration of hydrogen ions in the acid. In a monoprotic strong acid, all of the acid molecules dissociate completely in water, resulting in an equal concentration of hydrogen ions. This concentration of hydrogen ions directly determines the pH of the strong acid solution.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977806,"front":"Describe the ionic product for water.","back":"In all aqueous solutions and pure water, the equilibrium H2O (I) <=> H+ (aq) + OH- (aq) occurs.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":26,"explanation":"The ionic product for water is a measure of the concentration of hydrogen ions (H+) and hydroxide ions (OH-) in water. It is a constant value at a given temperature and is equal to the product of the concentrations of H+ and OH-. In pure water, the concentration of H+ and OH- ions is equal, resulting in a neutral solution. In aqueous solutions, the concentration of H+ and OH- ions can vary, leading to acidic or basic solutions. The equilibrium between water molecules and its ions is essential for many chemical reactions and plays a crucial role in maintaining the pH of a solution.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977808,"front":"What is the value of Kw for all aqueous solutions at 25°C?","back":"Kw = 1x10-14 mol2dm-6","front_language":"English","back_language":"English","front_image":"","back_image":"","order":27,"explanation":"At 25°C, the ion product of water, Kw, reflects the balance between the concentrations of hydrogen ions (H⁺) and hydroxide ions (OH⁻) in pure water. This equilibrium constant is crucial for understanding acid-base chemistry, as it helps determine pH and the behavior of acids and bases in solution.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977811,"front":"What is the pH of pure water at 25°C?","back":"pH = 7","front_language":"English","back_language":"English","front_image":"","back_image":"","order":28,"explanation":"Pure water at 25°C has a pH of 7 because at this temperature, the concentration of hydrogen ions (H+) and hydroxide ions (OH-) in water is equal, resulting in a neutral pH. This is due to the autoionization of water molecules.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977814,"front":"Describe how to calculate the pH of a strong base.","back":"To calculate the pH of a strong base, we need to work out the concentration of the hydroxide ion and assume complete dissociation. Then, we can use the Kw expression to find [H+(aq)]. Finally, we take the negative logarithm of [H+(aq)] to obtain the pH value.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":29,"explanation":"The process involves determining the concentration of hydroxide ions in the strong base and assuming complete dissociation. Using the Kw expression, we find the concentration of hydrogen ions. Taking the negative logarithm of this concentration gives the pH value.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977816,"front":"Define complete dissociation for strong bases.","back":"Complete dissociation refers to the process in which strong bases completely break apart into their ions when dissolved in water.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":30,"explanation":"Complete dissociation is a key characteristic of strong bases, indicating their ability to fully ionize in aqueous solutions. This results in a high concentration of hydroxide ions, leading to significant increases in pH. Such properties make strong bases effective in neutralizing acids and facilitating various chemical reactions.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977818,"front":"Describe the dissociation expression for weak acids.","back":"The dissociation expression for weak acids can be represented as HA (aq) -> H+ (aq) + A- (aq), where HA is the undissociated acid and H+ and A- are the dissociated ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":31,"explanation":"The dissociation expression for weak acids shows the equilibrium between the undissociated acid (HA) and its dissociated ions (H+ and A-). This equilibrium expression is crucial in understanding the extent of ionization of weak acids in solution and calculating their dissociation constants.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977820,"front":"What is the pKa value and how is it related to Ka?","back":"The pKa value is the negative logarithm of the Ka value. It is used to express the acidity of a weak acid. The larger the pKa value, the weaker the acid.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":32,"explanation":"The pKa value is a measure of the strength of an acid, with lower values indicating stronger acids. It is the negative logarithm of the acid dissociation constant (Ka), which represents the extent of acid dissociation. A higher pKa value signifies a weaker acid, as it indicates a lower tendency to donate protons.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977822,"front":"How can the pH of a weak acid be calculated?","back":"To calculate the pH of a weak acid, we can make two assumptions: 1) [H+] is equal to the concentration of the dissociated ions [H+(aa)] and 2) the initial concentration of the undissociated acid [HA] remains constant. Then, we can use the K2 expression and take the negative logarithm of [H+] to find the pH value.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":33,"explanation":"The pH of a weak acid can be calculated by assuming that the concentration of dissociated ions is equal to the concentration of [H+], and the initial concentration of the undissociated acid remains constant. By using the K2 expression and taking the negative logarithm of [H+], the pH value can be determined.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977795,"front":"Describe the Bronsted-Lowry definition of acid.","back":"A Bronsted-Lowry acid is a substance that can donate a proton.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":34,"explanation":"The Bronsted-Lowry definition focuses on the transfer of protons in acid-base reactions. Acids donate protons, while bases accept them. This definition is broader than the Arrhenius definition, which is limited to substances that release H+ ions in water.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977826,"front":"Describe pH calculations involving neutralisation reactions.","back":"pH calculations involving neutralisation reactions can be complex, especially when determining the pH of a partially neutralised acid or a solution with excess alkali. The method used depends on whether the acid is strong or weak in the partially neutralised case.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":35,"explanation":"Neutralization reactions involve the combination of an acid and a base to form a salt and water. Calculating the pH of such reactions can be complex due to the presence of excess reactants and partially neutralized acids. The method for determining pH depends on the strength of the acid involved in the reaction.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977828,"front":"Define strong acid and strong base neutralisations.","back":"Strong acid and strong base neutralisations involve the reaction between a strong acid and a strong base to form water and a salt. The pH of the resulting mixture can be calculated by determining the concentration of excess H+ or OH- ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":36,"explanation":"Strong acid and strong base neutralizations are fundamental chemical reactions that exemplify the concept of acid-base chemistry. The complete dissociation of both reactants leads to a predictable outcome, typically resulting in a neutral pH of 7, assuming equal concentrations. This principle is crucial in various applications, including titrations and buffer solutions.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977830,"front":"How do you calculate the new concentration of excess H+ ions in a strong acid and strong base neutralisation?","back":"To calculate the new concentration of excess H+ ions in a strong acid and strong base neutralisation, divide the moles of excess H+ ions by the total volume of the solution (in dm³).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":37,"explanation":"In a neutralization reaction, strong acids fully dissociate, providing H+ ions, while strong bases provide OH- ions. The reaction results in water and can leave excess H+ or OH- depending on the initial concentrations. Understanding the stoichiometry and total volume is crucial for accurate concentration calculations.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977831,"front":"Describe the process of determining which ion is in excess in a strong acid and strong base neutralisation.","back":"To determine which ion is in excess in a strong acid and strong base neutralisation, calculate the concentration of excess H+ and OH- ions separately. The ion with the higher concentration is the one in excess.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":38,"explanation":"In a strong acid and strong base neutralization, the excess ion can be determined by calculating the concentration of H+ and OH- ions separately. The ion with the higher concentration is the one in excess. This method helps identify the dominant ion in the neutralization process.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977833,"front":"Do strong diprotic acids and bases affect pH calculations differently?","back":"Yes, strong diprotic acids and bases, such as H2SO4 and Ba(OH)2, can affect pH calculations differently. The number of moles of H+ or OH- ions produced will be twice the number of moles of the diprotic acid or base used.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":39,"explanation":"Strong diprotic acids and bases release more ions per mole compared to monoprotic ones, leading to greater changes in pH. This characteristic is crucial in titration and buffer calculations, as it influences the stoichiometry and the resulting equilibrium concentrations in solution. Understanding this helps in accurate pH predictions.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977836,"front":"Describe the process of calculating the new concentration of excess HA in a weak acid and strong base neutralization.","back":"The new concentration of excess HA can be calculated by subtracting the moles of OH- from the initial moles of HA and dividing by the total volume.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":40,"explanation":"In weak acid and strong base neutralization, the reaction typically results in the formation of water and a salt. The initial moles of the weak acid (HA) are crucial, as they determine how much remains after reacting with the strong base (OH-). The total volume accounts for dilution effects, ensuring accurate concentration calculations.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977838,"front":"What is the formula to calculate the concentration of salt formed [A-] in a weak acid and strong base neutralization?","back":"The concentration of salt formed [A-] can be calculated by dividing the moles of OH- added by the total volume.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":41,"explanation":"In a neutralization reaction, the strong base reacts with the weak acid, leading to the formation of a salt and water. The concentration of the salt is influenced by the moles of hydroxide ions, which directly correlate to the amount of acid neutralized, and the total volume of the solution, which dilutes the resulting salt.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977840,"front":"Define pH and how it is calculated in a weak acid and strong base neutralization.","back":"pH is a measure of the acidity or alkalinity of a solution. In a weak acid and strong base neutralization, pH can be calculated using the formula pH = -log[H+].","front_language":"English","back_language":"English","front_image":"","back_image":"","order":42,"explanation":"pH measures the concentration of hydrogen ions in a solution. In a weak acid and strong base neutralization, the excess hydroxide ions from the base react with the weak acid, resulting in a higher pH. The pH is calculated using the negative logarithm of the hydrogen ion concentration.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977843,"front":"Describe the process of calculating the pH of a resulting mixture in a specific example of weak acid and strong base neutralization.","back":"In the given example, the pH of the resulting mixture can be calculated by rearranging the equation Ka=[H+][A-] to get [H+], and then substituting the values to find the pH.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":43,"explanation":null,"deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977846,"front":"How can the pH of a weak acid at half equivalence be simplified?","back":"At half equivalence, the assumption can be made that [HA] = [A-]. Therefore, [H+(aq)] = K2 and pH = pKa.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":44,"explanation":"At half equivalence, the assumption is that the concentrations of the weak acid and its conjugate base are equal. This simplifies the expression for the concentration of H+ ions to be equal to the second dissociation constant (K2) and allows for the pH to be calculated directly from the pKa of the weak acid. This simplification is based on the specific conditions at half equivalence in the titration of a weak acid with a strong base.","deleted_at":null,"flashcard_deck_id":"ViDxh","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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