Titration Curves - MCAT Chemical and Physical Foundations of Biological Systems
Card 1 of 63
A titration reaches its equivalence point. You measure the pH and find it to be 6.4. You were most likely working with which of the following sets of compounds:
A titration reaches its equivalence point. You measure the pH and find it to be 6.4. You were most likely working with which of the following sets of compounds:
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For a strong acids and strong base, the equivalence pH will be 7.0. We can see that our equivalence pH is less than 7.0, meaning that the acidic component is prevailing. Hence, we must be working with an acid that is stronger than our base. HNO3 is a strong acid, and NH3 is a weak base, meaning that the acid will prevail, and the pH will be acidic (<7.0).
The other answer choices show a strong acid and strong base (HCl and NaOH), a weak acid and strong base (HF and KOH, HCN and LiOH), and a weak acid and weak base (H2S and C5H8O2). Though the equivalence pH of a weak acid and weak base may not be 7.0, we do not have enough information to choose this answer. The best answer choice is HNO3 and NH3
For a strong acids and strong base, the equivalence pH will be 7.0. We can see that our equivalence pH is less than 7.0, meaning that the acidic component is prevailing. Hence, we must be working with an acid that is stronger than our base. HNO3 is a strong acid, and NH3 is a weak base, meaning that the acid will prevail, and the pH will be acidic (<7.0).
The other answer choices show a strong acid and strong base (HCl and NaOH), a weak acid and strong base (HF and KOH, HCN and LiOH), and a weak acid and weak base (H2S and C5H8O2). Though the equivalence pH of a weak acid and weak base may not be 7.0, we do not have enough information to choose this answer. The best answer choice is HNO3 and NH3
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A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
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At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
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Which of the following pH values is an acceptable equivalence point for a weak base being titrated by a strong acid?
Which of the following pH values is an acceptable equivalence point for a weak base being titrated by a strong acid?
Tap to reveal answer
The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.
The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.
The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.
The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.
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is a diprotic acid. Which of the following statements is true about its second half equivalence point?
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H2CO3 will have two equivalence points and two half equivalence points, one set corresponding to each of its two protons.
After the first equivalence point, all of the acid is in the form HCO3-. When an acid is at a half equivalence point, the acid's concentration will be equal to the concentration of the conjugate base. For the second half equivalence point, the acid is in the HCO3- form, and the conjugate base is CO32-. As a result, at the second half equivalence point, the concentrations of HCO3- and CO32- will be equal.
H2CO3 will have two equivalence points and two half equivalence points, one set corresponding to each of its two protons.
After the first equivalence point, all of the acid is in the form HCO3-. When an acid is at a half equivalence point, the acid's concentration will be equal to the concentration of the conjugate base. For the second half equivalence point, the acid is in the HCO3- form, and the conjugate base is CO32-. As a result, at the second half equivalence point, the concentrations of HCO3- and CO32- will be equal.
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Which of the following curves represents the titration of a strong base by a strong acid?
Which of the following curves represents the titration of a strong base by a strong acid?
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Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.
Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.
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Acids and bases can be described in three principal ways. The Arrhenius definition is the most restrictive. It limits acids and bases to species that donate protons and hydroxide ions in solution, respectively. Examples of such acids include HCl and HBr, while KOH and NaOH are examples of bases. When in aqueous solution, these acids proceed to an equilibrium state through a dissociation reaction.
All of the bases proceed in a similar fashion.
The Brønsted-Lowry definition of an acid is a more inclusive approach. All Arrhenius acids and bases are also Brønsted-Lowry acids and bases, but the converse is not true. Brønsted-Lowry acids still reach equilibrium through the same dissociation reaction as Arrhenius acids, but the acid character is defined by different parameters. The Brønsted-Lowry definition considers bases to be hydroxide donors, like the Arrhenius definition, but also includes conjugate bases such as the A- in the above reaction. In the reverse reaction, A- accepts the proton to regenerate HA. The Brønsted-Lowry definition thus defines bases as proton acceptors, and acids as proton donors.
A scientist decides to study an acid, 
, by carefully adding a base to the solution through a titration. At the equivalence point of an acid-base titration .
Acids and bases can be described in three principal ways. The Arrhenius definition is the most restrictive. It limits acids and bases to species that donate protons and hydroxide ions in solution, respectively. Examples of such acids include HCl and HBr, while KOH and NaOH are examples of bases. When in aqueous solution, these acids proceed to an equilibrium state through a dissociation reaction.
All of the bases proceed in a similar fashion.
The Brønsted-Lowry definition of an acid is a more inclusive approach. All Arrhenius acids and bases are also Brønsted-Lowry acids and bases, but the converse is not true. Brønsted-Lowry acids still reach equilibrium through the same dissociation reaction as Arrhenius acids, but the acid character is defined by different parameters. The Brønsted-Lowry definition considers bases to be hydroxide donors, like the Arrhenius definition, but also includes conjugate bases such as the A- in the above reaction. In the reverse reaction, A- accepts the proton to regenerate HA. The Brønsted-Lowry definition thus defines bases as proton acceptors, and acids as proton donors.
A scientist decides to study an acid,
Tap to reveal answer
A titrant is added to a solution being studied. In this scenario, the base is the titrant and the equivalence point is reached when all of the acid has been neutralized by the base. The equivalence point is defined as the point at which moles of added titrant equal the moles of initial solute in solution.
The equimolar concentration of acid and conjugate base happens at a point known as the half-equivalence point, which can be confusing.
A titrant is added to a solution being studied. In this scenario, the base is the titrant and the equivalence point is reached when all of the acid has been neutralized by the base. The equivalence point is defined as the point at which moles of added titrant equal the moles of initial solute in solution.
The equimolar concentration of acid and conjugate base happens at a point known as the half-equivalence point, which can be confusing.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Tap to reveal answer
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
What is the approximate pKa of the starting acid?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
What is the approximate pKa of the starting acid?
Tap to reveal answer
The pKa corresponds to the pH when half of the acid has been neutralized. In this case, that would correspond to when half of the 0.5M NaOH has been added. We can see in the curve that the equivalence point is at around 22mL of NaOH, as this is the steepest change in pH. The half equivalence point will be found at approximately 11mL of NaOH addition. On the graph, 11mL of NaOH results in a pH of approximately 5.0, giving us our pKa value.
The pKa corresponds to the pH when half of the acid has been neutralized. In this case, that would correspond to when half of the 0.5M NaOH has been added. We can see in the curve that the equivalence point is at around 22mL of NaOH, as this is the steepest change in pH. The half equivalence point will be found at approximately 11mL of NaOH addition. On the graph, 11mL of NaOH results in a pH of approximately 5.0, giving us our pKa value.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
Which of the following compounds could be the acid that is being titrated in this experiment?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
Which of the following compounds could be the acid that is being titrated in this experiment?
Tap to reveal answer
NaOH is a strong base, so if the acid were a strong acid, the pH at equivalence would be 7. The graph, however, shows that the pH at equivalence is greater than 7, which means the acid being titrated is a weak acid.
We can also find the approximate pKa value from the half equivalence point. In the graph, the equivalence point occurs at a pH around 8.9, corresponding to the addition of about 22mL of NaOH. The half equivalence point will thus be after the addition of approximately 11mL of NaOH, giving a pH of 5.0. The pH at the half equivalence is equal to the pKa, meaning that the Ka value must be around 10-5.
This leads to our answer, 
.
NaOH is a strong base, so if the acid were a strong acid, the pH at equivalence would be 7. The graph, however, shows that the pH at equivalence is greater than 7, which means the acid being titrated is a weak acid.
We can also find the approximate pKa value from the half equivalence point. In the graph, the equivalence point occurs at a pH around 8.9, corresponding to the addition of about 22mL of NaOH. The half equivalence point will thus be after the addition of approximately 11mL of NaOH, giving a pH of 5.0. The pH at the half equivalence is equal to the pKa, meaning that the Ka value must be around 10-5.
This leads to our answer,
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A titration reaches its equivalence point. You measure the pH and find it to be 6.4. You were most likely working with which of the following sets of compounds:
A titration reaches its equivalence point. You measure the pH and find it to be 6.4. You were most likely working with which of the following sets of compounds:
Tap to reveal answer
For a strong acids and strong base, the equivalence pH will be 7.0. We can see that our equivalence pH is less than 7.0, meaning that the acidic component is prevailing. Hence, we must be working with an acid that is stronger than our base. HNO3 is a strong acid, and NH3 is a weak base, meaning that the acid will prevail, and the pH will be acidic (<7.0).
The other answer choices show a strong acid and strong base (HCl and NaOH), a weak acid and strong base (HF and KOH, HCN and LiOH), and a weak acid and weak base (H2S and C5H8O2). Though the equivalence pH of a weak acid and weak base may not be 7.0, we do not have enough information to choose this answer. The best answer choice is HNO3 and NH3
For a strong acids and strong base, the equivalence pH will be 7.0. We can see that our equivalence pH is less than 7.0, meaning that the acidic component is prevailing. Hence, we must be working with an acid that is stronger than our base. HNO3 is a strong acid, and NH3 is a weak base, meaning that the acid will prevail, and the pH will be acidic (<7.0).
The other answer choices show a strong acid and strong base (HCl and NaOH), a weak acid and strong base (HF and KOH, HCN and LiOH), and a weak acid and weak base (H2S and C5H8O2). Though the equivalence pH of a weak acid and weak base may not be 7.0, we do not have enough information to choose this answer. The best answer choice is HNO3 and NH3
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A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
Tap to reveal answer
At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
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Which of the following pH values is an acceptable equivalence point for a weak base being titrated by a strong acid?
Which of the following pH values is an acceptable equivalence point for a weak base being titrated by a strong acid?
Tap to reveal answer
The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.
The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.
The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.
The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.
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is a diprotic acid. Which of the following statements is true about its second half equivalence point?
Tap to reveal answer
H2CO3 will have two equivalence points and two half equivalence points, one set corresponding to each of its two protons.
After the first equivalence point, all of the acid is in the form HCO3-. When an acid is at a half equivalence point, the acid's concentration will be equal to the concentration of the conjugate base. For the second half equivalence point, the acid is in the HCO3- form, and the conjugate base is CO32-. As a result, at the second half equivalence point, the concentrations of HCO3- and CO32- will be equal.
H2CO3 will have two equivalence points and two half equivalence points, one set corresponding to each of its two protons.
After the first equivalence point, all of the acid is in the form HCO3-. When an acid is at a half equivalence point, the acid's concentration will be equal to the concentration of the conjugate base. For the second half equivalence point, the acid is in the HCO3- form, and the conjugate base is CO32-. As a result, at the second half equivalence point, the concentrations of HCO3- and CO32- will be equal.
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Which of the following curves represents the titration of a strong base by a strong acid?
Which of the following curves represents the titration of a strong base by a strong acid?
Tap to reveal answer
Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.
Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.
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Acids and bases can be described in three principal ways. The Arrhenius definition is the most restrictive. It limits acids and bases to species that donate protons and hydroxide ions in solution, respectively. Examples of such acids include HCl and HBr, while KOH and NaOH are examples of bases. When in aqueous solution, these acids proceed to an equilibrium state through a dissociation reaction.
All of the bases proceed in a similar fashion.
The Brønsted-Lowry definition of an acid is a more inclusive approach. All Arrhenius acids and bases are also Brønsted-Lowry acids and bases, but the converse is not true. Brønsted-Lowry acids still reach equilibrium through the same dissociation reaction as Arrhenius acids, but the acid character is defined by different parameters. The Brønsted-Lowry definition considers bases to be hydroxide donors, like the Arrhenius definition, but also includes conjugate bases such as the A- in the above reaction. In the reverse reaction, A- accepts the proton to regenerate HA. The Brønsted-Lowry definition thus defines bases as proton acceptors, and acids as proton donors.
A scientist decides to study an acid, , by carefully adding a base to the solution through a titration. At the equivalence point of an acid-base titration .
Acids and bases can be described in three principal ways. The Arrhenius definition is the most restrictive. It limits acids and bases to species that donate protons and hydroxide ions in solution, respectively. Examples of such acids include HCl and HBr, while KOH and NaOH are examples of bases. When in aqueous solution, these acids proceed to an equilibrium state through a dissociation reaction.
All of the bases proceed in a similar fashion.
The Brønsted-Lowry definition of an acid is a more inclusive approach. All Arrhenius acids and bases are also Brønsted-Lowry acids and bases, but the converse is not true. Brønsted-Lowry acids still reach equilibrium through the same dissociation reaction as Arrhenius acids, but the acid character is defined by different parameters. The Brønsted-Lowry definition considers bases to be hydroxide donors, like the Arrhenius definition, but also includes conjugate bases such as the A- in the above reaction. In the reverse reaction, A- accepts the proton to regenerate HA. The Brønsted-Lowry definition thus defines bases as proton acceptors, and acids as proton donors.
A scientist decides to study an acid,
Tap to reveal answer
A titrant is added to a solution being studied. In this scenario, the base is the titrant and the equivalence point is reached when all of the acid has been neutralized by the base. The equivalence point is defined as the point at which moles of added titrant equal the moles of initial solute in solution.
The equimolar concentration of acid and conjugate base happens at a point known as the half-equivalence point, which can be confusing.
A titrant is added to a solution being studied. In this scenario, the base is the titrant and the equivalence point is reached when all of the acid has been neutralized by the base. The equivalence point is defined as the point at which moles of added titrant equal the moles of initial solute in solution.
The equimolar concentration of acid and conjugate base happens at a point known as the half-equivalence point, which can be confusing.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Tap to reveal answer
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
What is the approximate pKa of the starting acid?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
What is the approximate pKa of the starting acid?
Tap to reveal answer
The pKa corresponds to the pH when half of the acid has been neutralized. In this case, that would correspond to when half of the 0.5M NaOH has been added. We can see in the curve that the equivalence point is at around 22mL of NaOH, as this is the steepest change in pH. The half equivalence point will be found at approximately 11mL of NaOH addition. On the graph, 11mL of NaOH results in a pH of approximately 5.0, giving us our pKa value.
The pKa corresponds to the pH when half of the acid has been neutralized. In this case, that would correspond to when half of the 0.5M NaOH has been added. We can see in the curve that the equivalence point is at around 22mL of NaOH, as this is the steepest change in pH. The half equivalence point will be found at approximately 11mL of NaOH addition. On the graph, 11mL of NaOH results in a pH of approximately 5.0, giving us our pKa value.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
Which of the following compounds could be the acid that is being titrated in this experiment?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
Which of the following compounds could be the acid that is being titrated in this experiment?
Tap to reveal answer
NaOH is a strong base, so if the acid were a strong acid, the pH at equivalence would be 7. The graph, however, shows that the pH at equivalence is greater than 7, which means the acid being titrated is a weak acid.
We can also find the approximate pKa value from the half equivalence point. In the graph, the equivalence point occurs at a pH around 8.9, corresponding to the addition of about 22mL of NaOH. The half equivalence point will thus be after the addition of approximately 11mL of NaOH, giving a pH of 5.0. The pH at the half equivalence is equal to the pKa, meaning that the Ka value must be around 10-5.
This leads to our answer, .
NaOH is a strong base, so if the acid were a strong acid, the pH at equivalence would be 7. The graph, however, shows that the pH at equivalence is greater than 7, which means the acid being titrated is a weak acid.
We can also find the approximate pKa value from the half equivalence point. In the graph, the equivalence point occurs at a pH around 8.9, corresponding to the addition of about 22mL of NaOH. The half equivalence point will thus be after the addition of approximately 11mL of NaOH, giving a pH of 5.0. The pH at the half equivalence is equal to the pKa, meaning that the Ka value must be around 10-5.
This leads to our answer,
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A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
A weak acid is slowly titrated with a strong base. Where on the titration curve would the solution be the most well-buffered?
Tap to reveal answer
At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.
Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pKa.
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Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.
The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?
Tap to reveal answer
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
For any titration curve the equivalence point corresponds to the steepest part of the curve. In this case, the question indicates that the pH at equivalence was 8.9, which would correspond to a volume between 20.0 and 24.0 on the x-axis of the graph. This leads to our approximate answer of 21.8mL.
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