Title: Chapter 14: Acid-Base Equilibria
Course: Test

Q: Which of the following is an electronic device used to measure the hydrogen ion activity in aqueous solutions?
- pH meter
- potentiometer
- ammeter
A: pH meter

Q: Which of the following is a typical type of electrode found on a pH meter?
- gold electrode
- glass electrode
- silver electrode
A: glass electrode

Q: When titrating a weak acid with a strong base, approximately where would the pH be observed when reaching the equivalence point?
- at the equivalence point, the pH is greater than 7
- at the equivalence point, the pH is equal to 7
- at the equivalence point, the pH is less than 7
A: at the equivalence point, the pH is greater than 7

Q: When titrating a weak base with a strong acid, approximately where would the pH be observed when reaching the equivalence point?
- at the equivalence point, the pH is greater than 7
- at the equivalence point, the pH is equal to 7
- at the equivalence point, the pH is less than 7
A: at the equivalence point, the pH is less than 7

Q: When titrating a strong acid with a strong base, approximately where would the pH be observed when reaching the equivalence point?
- at the equivalence point, the pH is greater than 7
- at the equivalence point, the pH is equal to 7
- at the equivalence point, the pH is less than 7
A: at the equivalence point, the pH is equal to 7

Q: What are the products formed at the equivalence point when titrating a strong acid with a strong base?
- salt and water
- the solution is neutral, so water only
- no products are formed
A: salt and water

Q: Phenolphthalein can be used as an _____ in acid-base titrations.
- equivalence point
- end-point
- indicator
A: indicator

Q: Phenolphthalein can be used as an indicator in acid-base titrations. When a few drops are added to an acidic solution which is then titrated with a strong base, the color of the solution changes from _____ to _____.
- colorless; pink
- pink; colorless
- colorless; red
A: colorless; pink

Q: When blue litmus paper is in contact with an acid, the litmus paper will turn _____.
- orange
- red
- green
A: red

Q: When red litmus paper is in contact with a base, the litmus paper will turn _____.
- orange
- green
- blue
A: blue

Q: Which of the following is a diprotic acid?
- H_3PO_4
- H_2PO_4^-
- HPO_4^2-
A: H_2PO_4^-

Q: Which of the following is an amphiprotic substance?
- H_3PO_4
- PO_4^3-
- HPO_4^2-
A: HPO_4^2-

Q: What is the conjugate base that is formed when carbonic acid is dissolved in water?
- H_3O^+
- HCO_3^-
- CO_3^2-
A: HCO_3^-

Q: When phosphoric acid is dissolved in water, what is the conjugate acid that is formed?
- H_2PO_4^-
- H_3O^+
- HPO_4^2-
A: H_3O^+

Q: What is the conjugate base that is formed upon the addition of carbonic acid to water?
- HCO_3^-
- H_3O^+
- CO_3^2-
A: HCO_3^-

Q: Rank the following oxyanions in order of increasing basicity: ClO_4^-, ClO_2^-, ClO^-, ClO_3^-.
- ClO_4^-, ClO^-, ClO_2^-, ClO_3^-
- ClO^-, ClO_2^-, ClO_3^-, ClO_4^-
- ClO_4^-, ClO_3^-, ClO_2^-, ClO^-
A: ClO_4^-, ClO_3^-, ClO_2^-, ClO^-

Q: Rank the following oxoacids in order of increasing acidity: HClO_2, HClO_4, HClO, HClO_3.
- HClO, HClO_2, HClO_3, HClO_4
- HClO_4, HClO_2, HClO, HClO_3
- HClO_4, HClO_3, HClO_2, HClO
A: HClO, HClO_2, HClO_3, HClO_4

Q: What is the pH of a solution if 10 mL of a 1 M HCl solution is added to 10 mL of a 1 M NaOH solution?
- 14
- 7
- 0
A: 7

Q: If 10 mL of a 1 M HI solution is added to 5 mL of a 1 M KOH solution, the resulting solution would be _____.
- acidic
- basic
- neutral
A: acidic

Q: If 3 mL of a 0.5 M HBr solution is added to 20 mL of a 0.5 M NaOH solution, the resulting solution would be _____.
- acidic
- basic
- neutral
A: basic

Q: What is the hydronium concentration of a solution at pH 7?
- 1 x 10^+7 M
- 1 x 10^-14 M
- 1 x 10^-7 M
A: 1 x 10^-7 M

Q: A student titrates 50.0 mL of an unknown concentration of HI with 85 mL of a 1.0 M solution of NaOH to reach the equivalence point. What is the pH of the HI solution?
- -0.23
- 0.23
- 1.7
A: -0.23

Q: A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution?
- -0.10
- 0.10
- 1.2
A: -0.10

Q: A student discovers a bottle of a highly corrosive monoprotic acid with the label partially destroyed. How can the concentration of the unknown acid be determined without using a pH meter?
- The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH^- added would be equal to moles of H^+ in the unknown at the half-way point, therefore, the concentration of the unknown can be calculated.
- The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH^- added would be equal to moles of H^+ in the unknown at the equivalence point, therefore, the concentration of the unknown can be calculated.
- The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of the unknown acid is 1 x 10^-7 M.
A: The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH^- added would be equal to moles of H^+ in the unknown at the equivalence point, therefore, the concentration of the unknown can be calculated.

Q: A student discovers a bottle of NaOH with a partially destroyed label. How can the concentration be determined without using a pH meter?
- The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The moles of H^+ and OH^- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.
- The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of NaOH is 1 x 10^-7 M.
- The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate HCl. The moles of H^+ and OH^- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.
A: The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The moles of H^+ and OH^- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.

Q: What is the pH of 0.048 M solution of hydrochloric acid?
- 0.32
- 4.8
- 1.3
A: 1.3

Q: What is the pH of 0.014 M solution of hydroiodic acid?
- 1.4
- 1.9
- 0.85
A: 1.9

Q: What is the pH of deionized water?
- pH = 7
- pH < 7
- pH > 7
A: pH = 7

Q: What is the pH of 0.48 M HCl solution?
- 0.32
- -0.32
- 13.68
A: 0.32

Q: What is the pH of 8.1 x 10^-5 M HClO_4 solution?
- 9.91
- 4.09
- -4.09
A: 4.09

Q: What is the hydroxide ion concentration for a 23% (m/v) HNO_3 solution?
- 10.35 M
- 3.65 M
- 2.74 x 10^-15 M
A: 2.74 x 10^-15 M

Q: Blood is considered a buffered solution. What is the pH range of blood?
- 7.35 to 7.45
- 6.35 to 6.45
- 8.35 to 8.45
A: 7.35 to 7.45

Q: What instrument can be used to measure the hydrogen ion concentration in solutions?
- ammeter
- pH meter
- potentiometer
A: pH meter

Q: Which acid has a lower pH?
- 1.0 M acetic acid
- 0.50 M acetic acid
- 0.25 M acetic acid
A: 1.0 M acetic acid

Q: Which acid has a higher hydrogen ion concentration?
- 1.0 M HCl
- 0.050 M HNO_3
- 1.25 M HBr
A: 1.25 M HBr

Q: What is the base in the following reaction: HCl (aq) + H_2O (l) →Cl^- (aq) + H_3O^+ (aq)?
- Cl^-
- H_3O^+
- H_2O
A: H_2O

Q: What is the conjugate acid in the following reaction: HCl (aq) + H_2O (l) →Cl^- (aq) + H_3O^+ (aq)?
- Cl^-
- H_3O^+
- H_2O
A: H_3O^+

Q: What is the conjugate base in the following reaction: HCl (aq) + H_2O (l) →Cl^- (aq) + H_3O^+ (aq)?(Paired item 1)
- Cl^-
- H_3O^+
- H_2O
A: Cl^-

Q: What is the conjugate base of HSO_4^-?
- H_2SO_4
- SO_4^2-
- SO_4^-
A: SO_4^2-

Q: What is the conjugate acid of HSO_4^-?
- H_2SO_4
- SO_4^2-
- H_2SO_4^-
A: H_2SO_4

Q: Write the equilibrium expression for the autoionization of water.
- K_w = [H_3O^+] [OH^-] / [H_2O]^2
- K_w = [H_3O^+] [OH^-]
- K_w = [H_2O]^2 / [H_3O^+] [OH^-]
A: K_w = [H_3O^+] [OH^-]

Q: What is the pOH of a solution that has a pH of 7?
- 7
- 14
- 0
A: 7

Q: What is the pOH of a solution that has a pH of 2?
- 12
- 7
- 14
A: 12

Q: Which acid has the lowest hydroxide ion concentration?
- 0.010 M HCl
- 0.050 M HNO_3
- 0.015 M HBr
A: 0.010 M HCl

Q: What is the conjugate base in the following reaction: HI (aq) + H_2O (l) →I^- (aq) + H_3O^+ (aq)?
- I^-
- H_3O^+
- H_2O
A: I^-

Q: What is the acid in the following reaction: NH_3 (aq) + H_2O (l) →NH_4^+ (aq) + OH^- (aq)?
- NH_3
- NH_4^+
- H_2O
A: H_2O