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| 1 |
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Q:
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A solution of unknown acid is titrated with NaOH and the following titration curve is seen.
What is the most likely identity of the acid? |
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A
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HCl |
B
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H2O |
C
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H2SO4 |
D
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H3PO4 |
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Tags:
Titrations | |
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| 2 |
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Q:
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A titration was performed on a weak acid of pKa 5 with an extremely strong base. On the titration curve, at which pH will the equivalence point be seen?
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A
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Less than 7 |
B
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7 |
C
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Greater than 7 |
D
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Not enough information given |
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Tags:
Titrations | |
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| 3 |
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Q:
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The pKa of the amino acid tyrosine is between 10.0 and 10.3. Tyrosine molecule R groups are phenolics, with the hydroxyl hydrogen titrating in the pH range given. If a given solution of tyrosine molecules is brought from pH 9 to pH 11, what do you expect to occur to the hydroxyl group? |
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A
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The hydroxyl will go from being protonated at pH 9 to being deprotonated at pH 11 |
B
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The hydroxyl will go from being deprotonated at pH 9 to being protonated at pH 11 |
C
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The hydroxyl will remain deprotonated during the pH shift |
D
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The hydroxyl will remain protonated during the pH shift |
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Tags:
Titrations | |
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| 4 |
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Q:
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A weak acid is titrated with NaOH. The equivalence point will occur at a pH |
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A
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Less than 7 |
B
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of 7 |
C
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Greater than 7 |
D
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dependent on the pKa of the weak acid |
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Tags:
Titrations | |
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| 5 |
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Q:
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A buffer is made for an experiment to a pH of 7.5. The scientist realizes that the volume of the buffer is 5 mL too low, and adds 5 mL of water. What will be the pH of the subsequent solution? |
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A
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pH < 7 |
B
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7 < pH < 7.5 |
C
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pH = 7.5 |
D
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pH > 7.5 |
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Tags:
Titrations | |
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| 6 |
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Q:
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At which pH could the equivalence point of a weak base titrated with hydrochloric acid be reached? |
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A
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5.6 |
B
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7 |
C
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7.5 |
D
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None of the above |
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Tags:
Titrations | |
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| 7 |
Go |
Q:
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0.045 moles of NaOH are used to titrate 500 mL of a 0.030 M solution of an acid. What is the most likely identity of the acid? |
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A
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HCl |
B
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H2SO4 |
C
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H3PO4 |
D
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Cannot be determined based on the given information. |
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Tags:
Titrations | |
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| 8 |
Go |
Q:
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A titration was performed on a weak acid of pKa 6 with an extremely strong base. On the titration curve, at which pH will the equivalence point be seen? |
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A
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Less than 7 |
B
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7 |
C
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Greater than 7 |
D
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Not enough information given |
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Tags:
Titrations | |
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| 9 |
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Q:
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Oxalic acid, H2C2O4, is a diprotic acid with a pKa value of 1.19. If 0.10 M oxalic acid is titrated 0.10 M NaOH, what would be the pH halfway to the first equivalence point? Relevant equilibria are given below:
H2C2O4 + H2O ↔ H3O+ + HC2O4- (pKa1 = 1.19)
HC2O4- + H2O ↔ H3O+ + C2O4-2 (pKa2 = 4.21) |
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A
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1.19 |
B
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4.21 |
C
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2.70 |
D
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2.11 |
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Tags:
Acid/Base Equilibria | Titrations | |
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| 10 |
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Q:
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What volume of a 0.4 M solution of NaOH is necessary to take the pH of a 36 ml solution of 0.8 M HCl to 7.0? |
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A
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18 mL |
B
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32 mL |
C
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36 mL |
D
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72 mL |
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Tags:
Acid/Base Equilibria | Titrations | |
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| 11 |
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Q:
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The graph above is a titration curve of three different solutions. Solution I is titrated with a base of a lower pH. Rank the solutions in terms of the strength of the acid in the solution. |
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A
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I < II < III |
B
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III < I < II |
C
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II < III < I |
D
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There is no difference among the strength of the acids. |
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Tags:
Titrations | |
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| 12 |
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Q:
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Arginine has a pKa of 12.48. At which pH will >50% of the R-groups in a solution of arginine be positively charged? |
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A
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13.58 |
B
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12.48 |
C
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11.09 |
D
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Cannot be determined from the information given |
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Tags:
Titrations | |
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| 13 |
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Q:
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Solid NaOH is hygroscopic, meaning it absorbs moisture from the air. A student places solid NaOH into a weighing dish and leaves the sample out for too long before weighing it. The student then dissolves the NaOH and uses the solution in a titration of an acid. The measured amount of the acid will therefore be |
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A
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less than the actual amount of acid |
B
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greater than the actual amount of acid |
C
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equal to the actual amount of acid |
D
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the answer cannot be determined with the given information |
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Tags:
Titrations | |
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| 14 |
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Q:
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A weak base is titrated with H2SO4. The equivalence point will occur at a pH that is: |
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A
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Less than 7 |
B
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Exactly 7 |
C
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Greater than 7 |
D
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Dependent on the pKb of the base |
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Tags:
Acid/Base Equilibria | Titrations | |
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| 15 |
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Q:
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An acid, HX, has an acid dissociation constant of 7*10-3. Which of the following is the expected pH of a solution that contains equal concentrations of HX and X- (the conjugate base of HX)? |
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Tags:
Titrations | |
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| 16 |
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Q:
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An acid is titrated with a sodium hydroxide and a titration curve is developed. The half-equivalence point is found to be at a pH of approximately 4 and the equivalence point is found to be at a pH of approximately 8. What is the Ka of this acid? |
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A
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10-3 |
B
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9 x 10-5 |
C
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1.2 x 10-8 |
D
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9 x 10-10 |
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Tags:
Titrations | |
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| 17 |
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Q:
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If 0.025 L of a 4M solution of sodium hydroxide is titrated with hydrochloric acid, how many millimoles of hydrochloric acid would be expected to be used in the reaction? |
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Tags:
Titrations | |
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| 18 |
Go |
Q:
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A titration curve is developed from an unknown acid and it is found that there are two equivalence points. Which of the following acids would be a possible identity of the unknown acid? |
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A
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HSO4- |
B
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H2SO4 |
C
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H3PO4 |
D
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H4P2O7 |
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Tags:
Titrations | |
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| 19 |
Go |
Q:
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65 mL of 9 M sodium hydroxide is added in a titration reaction with hydrochloric acid. Approximately how many mmol of HCl would be utilized in this reaction? |
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A
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0.6 mmol |
B
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6 mmol |
C
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60 mmol |
D
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600 mmol |
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Tags:
Titrations | |
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