When an acid and base neutralize each other, the products are generally water and...

1. an ion.
2. a gel.
3. a colloid.
4. a salt.

How many moles of Ca(OH)₂ are needed to neutralize three moles of HCl?

1. 1
2. 1.5
3. 3
4. 2

An aqueous solution is prepared with 2 moles of HCl and 1 mole of Ca(OH)₂. The resulting solution contains mainly...

1. water, Cl^- ions, OH^- ions, and Ca²⁺ ions.
2. water, Cl^- ions, H⁺ ions, and Ca²⁺ ions.
3. water, Cl^- ions, and Ca²⁺ ions.
4. water, Cl^- ions, H⁺ ions, OH^- ions, and Ca²⁺ ions.

Identify the products of the following chemical reaction:

3LiOH + H₃PO₄ ⟶

1. Li₃PO₄ + 3H₂O
2. Li₃P + 2H₂O + H₃O₅
3. 3H⁺ + 3O₂ + H₃Li₃
4. 3LiH + (OH)₃PO₄

Identify the products of the following chemical reaction:

Sr(OH)₂ + 2HNO₃ ⟶

1. Sr(NO₂)₂ + 2H₂O₂
2. SrNO₃ + H₂O
3. SrH₂ + HNO₅
4. Sr(NO₃)₂ + 2H₂O

Aqueous ammonia can be used to neutralize sulfuric acid and nitric acid to produce two salts extensively used as fertilizers. They are...

1. NH₄SO₄ and NH₄NO₃, respectively
2. (NH₄)₂SO₄ and NH₄NO₃, respectively
3. NH₄SO₃ and NH₄OH, respetively
4. cyanamide and cellulose nitrate, respectively

Identify the salt that is produced from the acid-base neutralization reaction between potassium hydroxide and acetic acid.

1. potassium amide
2. potassium cyanide
3. potassium acetate
4. potassium formate

What is the pH of an aqueous solution that is 0.018 M C6H₅NH₂ (K_b = 4.3 × 10^-10) and 0.12 M C6H₅NH₃Cl?

1. 2.87
2. 4.02
3. 3.81
4. 4.63

A buffer solution is made by dissolving 0.45 moles of a weak acid (HA) and 0.33 moles of KOH into 710 mL of solution. What is the pH of this buffer? K_a = 6 × 10^-6 for HA.

1. 13.23
2. 5.22
3. 5.66
4. 8.34

Which one of the following combinations is NOT a buffer solution?

1. NH₃ and (NH₄)₂SO₄
2. CH₃COOH and NaCH₃COO
3. HCN and NaCN
4. HBr and KBr

Which of the following mixtures will be a buffer when dissolved in a liter of water?

1. 0.2 mol HBr and 0.1 mol NaOH
2. 0.3 mol NaCl and 0.3 mol HCl
3. 0.2 mol HF and 0.1 mol NaOH
4. 0.1 mol Ca(OH)₂ and 0.3 mol HI

What is the pH of a solution which is 0.600 M in dimethylamine ((CH₃)₂NH) and 0.400 M in dimethylamine hydrochloride ((CH₃)₂NH₂Cl)? K_b for dimethylamine = 7.4 × 10^-4

1. 11.05
2. 10.87
3. 10.78
4. 11.21

What would be the final pH if 0.0100 moles of solid NaOH were added to 100mL of a buffer solution containing 0.600 molar formic acid (ionization constant = 1.8 × 10^-4) and 0.300 M sodium formate?

1. 3.65
2. 3.44
3. 3.84
4. 4.05

A buffer was prepared by mixing 0.200 moles of ammonia (K_b = 1.8 × 10^-5) and 0.200 moles of ammonium chloride to form an aqueous solution with a total volume of 500 mL. 250 mL of the buffer was added to 50.0 mL of 1.00 M HCl. What is the pH of this second solution?

1. 8.38
2. 8.53
3. 8.78
4. 8.18

A solution is 0.30 M in NH₃. What concentration of NH₄Cl would be required to achieve a buffer solution with a final pH of 9.0? K_b = 1.8 × 10^-5 for NH₃.

1. 0.54 M
2. 0.32 M
3. 0.45 M
4. 0.10 M

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.1 M KOH(aq)? For HNO₂, K_a = 4.3 × 10^-4.

1. 2.01
2. 7.00
3. 2.31
4. 3.37

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH (aq), calculate the pH after the addition of 55.0 mL of the base. For salicylic acid, pK_a = 2.97.

1. 10.98
2. 11.26
3. 7.00
4. 11.02

Consider the titration of 50.0 mL of 0.0200 M HClO(aq) with 0.100 M NaOH(aq). What is the formula of the main species in the solution after the addition of 10.0 mL of base?

1. HClO
2. NaOH
3. ClO₂
4. ClO-

50.0 mL of 0.0018 M aniline (a weak base) is titrated with 0.0048 M HNO₃. How many mL of the acid are required to reach the equivalence point?

1. 4.21 mL
2. 18.8 mL
3. This is a bad titration as HNO₃ is not a strong acid.
4. 133 mL

When we titrate a weak base with a strong acid, the pH at the equivalence point will be...

1. It is impossible to know unless we are given the K_b of the weak base.
2. pH > 7
3. pH = 0
4. pH < 7

What is the pH at the equivalence point in the titration of 10.0 mL of 0.35 M unknown acid HZ with 0.200 M NaOH? K_a = 2.4 × 10^-7 for the unknown acid HZ

1. 7.00
2. 9.86
3. 10.1
4. 4.14

What is the pH at the equivalence point of the titration pictures below?

1. 8
2. 5
3. 9
4. 2

Look at the titration diagram in the question above. What type of titration is occurring?

1. a weak base titrated with a strong acid
2. a strong base titrated with a weak acid
3. a strong base titrated with a strong acid
4. a weak base titrated with a weak acid

The acid form of an indicator is yellow and its anion is blue. The K_a of this indicator is 10^-5. What will be the approximate pH range over which this indicator changes color?

1. 6 < pH < 8
2. 4 < pH < 6
3. 5 < pH < 7
4. 3 < pH < 5

The unionized form of an acid indicator is yellow and its anion is blue. The K_a of this indicator is 10^-5. What will be the color of the indicator in a solution of pH 3?

1. orange
2. blue
3. green
4. yellow

Aspartic acid is a polypeptide side chain found in proteins. The pK_a of aspartic acid is 3.86. If this polypeptide were in an aqueous solution with a pH of 7, the side chain would have what charge?

1. positive
2. negative
3. neutral
4. there is no way to know

Blood contains a buffer of carbonic acid (H₂CO₃) and hydrogen carbonate ion (HCO₃^–) that keeps the pH at a relatively stable 7.40. What is the ratio of [HCO₃^–] / [H₂CO₃] in blood? K_a1 = 4.30 × 10^-7 for H₂CO₃ (Hint: Assume [CO₃^2–] = 0)

1. 10.8
2. 3.98 x 10^-8
3. 0.0926
4. 1.71 x 10^-14

H₂SO₄ is a strong acid because the first proton ionizes 100%. The K_a of the second proton is 1.1 × 10^-2. What would be the pH of a solution that is 0.100 M H₂SO₄? Account for the ionization of both protons.

1. 0.955
2. 0.963
3. 2.05
4. 1.00