Question 1

What is [OH-] for a solution at 25°C that has [H3O+] = 2.35 × 10-3 M?

Accepted Answer

A)   4.26 × 10-5 M
B)   2.35 ×10-11 M
C)   4.26 × 10-12 M
D)   2.35 × 10-17 M
E)   2.35 ×10-3 M

Question 2

The most acidic oxides are formed from elements found in the ________ region of the periodic table.

Accepted Answer

A)   upper right
B)   upper left
C)   center
D)   lower right
E)   lower left

Question 3

Below is a representation of an aqueous solution of a weak acid HA at equilibrium. (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.)  -3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.)    What is Ka of HA? A)  1.0 ×10-6 B)  6.0 ×10-3 C)  2.5 ×10-4 D)  3.6 ×10-5 E)  1.0 ×10-9" class="answers-bank-image d-inline" rel="preload" > What is Ka of HA?

Accepted Answer

A)   1.0 ×10-6
B)   6.0 ×10-3
C)   2.5 ×10-4
D)   3.6 ×10-5
E)   1.0 ×10-9

Question 4

Which is the weakest acid?

Accepted Answer

A)   HBrO3
B)   HClO
C)   HBrO2
D)   HBrO
E)   HClO3

Question 5

Which is a Lewis acid but not a Brønsted acid?

Accepted Answer

A)   HCN
B)   CO32-
C)   OH-
D)   Cl-
E)   Al3+

Question 6

What mass of sodium nitrite must be added to enough water to make 350.0 mL of a solution with pH = 8.40? [Ka(HNO2)  = 5.6 × 10-4]

Accepted Answer

A)   68 g
B)   1.7 × 10-4 g
C)   0.039 g
D)   8.7 g
E)   24 g

Question 7

Which is the most basic oxide?

Accepted Answer

A)   Bi2O3
B)   SiO2
C)   Cs2O
D)   Na2O
E)   H2O

Question 8

The pH of a Ba(OH) 2 solution is 10.00. What is the H+ ion concentration of this solution?

Accepted Answer

A)   4.0 × 10-11 M
B)   1.6 × 10-10 M
C)   1.3 × 10-5 M
D)   1.0 × 10-10 M
E)   10.00 M

Question 9

Equal volumes of two solutions, one containing a strong acid at pH 2 and the other containing a strong base at pH 12, are mixed. Once equilibrium is achieved, what is the final pH of the combined solution?

Accepted Answer

A)   6
B)   7
C)   10
D)   14
E)   24

Question 10

Calculate the pH of a 0.021 M NaCN solution. [Ka(HCN)  = 4.9 × 10-10]

Accepted Answer

A)   1.68
B)   3.19
C)   4.69
D)   9.31
E)   10.81

Question 11

The acid dissociation constant Ka equals 1.26 × 10-2 for HSO4- and is 5.6 × 10-10 for NH4+. Which statement about the following equilibrium is correct? HSO4-(aq)  + NH3(aq)  a equals 1.26 × 10-2 for HSO4- and is 5.6 × 10-10 for NH4+. Which statement about the following equilibrium is correct? HSO4-(aq)  + NH3(aq)    SO42-(aq)  + NH4+(aq)  A)  The reactants will be favored because ammonia is a stronger base than the sulfate anion. B)  The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion. C)  Neither reactants nor products will be favored because all of the species are weak acids or bases. D)  The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made. E)  This reaction is impossible to predict, since the strong acid and the weak base appear on the same side of the equation." class="answers-bank-image d-inline" rel="preload" > SO42-(aq)  + NH4+(aq)

Accepted Answer

A)   The reactants will be favored because ammonia is a stronger base than the sulfate anion.
B)   The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion.
C)   Neither reactants nor products will be favored because all of the species are weak acids or bases.
D)   The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made.
E)   This reaction is impossible to predict, since the strong acid and the weak base appear on the same side of the equation.

Question 12

What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3)  = 1.8 × 10-5]

Accepted Answer

A)   3.74
B)   4.98
C)   6.53
D)   9.02
E)   11.28

Question 13

If a strong acid such as HCl is diluted sufficiently with water, the pH will be higher than 7.

Accepted Answer

A) True 
 B)False

Question 14

What is the pH of a 0.050 M LiOH solution?

Accepted Answer

A)   1.30
B)   3.00
C)   11.00
D)   12.39
E)   12.70

Question 15

Which one of these salts will form a basic solution upon dissolving in water?

Accepted Answer

A)   NaCl
B)   NaNO2
C)   NH4NO3
D)   KBr
E)   AlCl3

Question 16

Which one of the following is a strong acid?

Accepted Answer

A)   H2CO3
B)   H2SO3
C)   H2SO4
D)   H3PO4
E)   CH3COOH

Question 17

Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4) , for which Ka = 2.3 × 10-2.

Accepted Answer

A)   1.25
B)   3.28
C)   1.17
D)   1.34
E)   1.64

Question 18

The substance (CH3CH2) 2NH is considered to be

Accepted Answer

A)   a weak acid.
B)   a weak base.
C)   a strong acid.
D)   a strong base.
E)   a neutral compound.

Question 19

After a substance acting as a strong base reacts, what remains of the base?

Accepted Answer

A)   a weaker base
B)   a strong conjugate acid
C)   a strong conjugate base
D)   a strong acid
E)   a weak conjugate acid

Question 20

Consider the weak bases below and their Kb values: C6H7O- Kb = 1.3 × 10-10
C2H5NH2 Kb = 5.6 × 10-4
C5H5N Kb = 1.7 ×10-9
Arrange the conjugate acids of these weak bases in order of increasing acid strength.

Accepted Answer

A)   C5H5NH+6H7OH 2H5NH
B)   C6H7OH 5H5NH+ 2H5NH
C)   C5H5NH+2H5NH3+ 6H7OH
D)   C6H7OH 2H5NH3+5H5NH+
E)   C2H5NH3+5H5NH+ 6H7OH

Exam 16: Acids and Bases

After a substance acting as a strong base reacts, what remains of the base?

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Which is a Lewis acid but not a Brønsted acid?

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The most acidic oxides are formed from elements found in the ________ region of the periodic table.

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Consider the weak bases below and their Kb values: C6H7O- Kb = 1.3 × 10-10 C2H5NH2 Kb = 5.6 × 10-4 C5H5N Kb = 1.7 ×10-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

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Calculate the pH of a 0.021 M NaCN solution. [Ka(HCN) = 4.9 × 10-10]

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The substance (CH3CH2) 2NH is considered to be

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Equal volumes of two solutions, one containing a strong acid at pH 2 and the other containing a strong base at pH 12, are mixed. Once equilibrium is achieved, what is the final pH of the combined solution?

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What is the pH of a 0.050 M LiOH solution?

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Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4) , for which Ka = 2.3 × 10-2.

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The pH of a Ba(OH) 2 solution is 10.00. What is the H+ ion concentration of this solution?

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Which is the most basic oxide?

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The acid dissociation constant Ka equals 1.26 × 10-2 for HSO4- and is 5.6 × 10-10 for NH4+. Which statement about the following equilibrium is correct? HSO4-(aq) + NH3(aq) SO42-(aq) + NH4+(aq)

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Which is the weakest acid?

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Which one of the following is a strong acid?

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What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 × 10-5]

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What is [OH-] for a solution at 25°C that has [H3O+] = 2.35 × 10-3 M?

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If a strong acid such as HCl is diluted sufficiently with water, the pH will be higher than 7.

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Which one of these salts will form a basic solution upon dissolving in water?

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Below is a representation of an aqueous solution of a weak acid HA at equilibrium. (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.) What is Ka of HA?

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What mass of sodium nitrite must be added to enough water to make 350.0 mL of a solution with pH = 8.40? [Ka(HNO2) = 5.6 × 10-4]

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Consider the weak bases below and their K_b values: C₆H₇O^-^K_b = 1.3 × 10^-10 C₂H₅NH₂K_b = 5.6 × 10^-4 C₅H₅N K_b = 1.7 ×10^-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

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Calculate the pH of a 0.021 M NaCN solution. [K_a(HCN) = 4.9 × 10^-10]

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The substance (CH₃CH₂) ₂NH is considered to be

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Find the pH of a 0.135 M aqueous solution of periodic acid (HIO₄) , for which K_a = 2.3 × 10^-2.

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The pH of a Ba(OH) ₂ solution is 10.00. What is the H⁺ ion concentration of this solution?

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The acid dissociation constant K_a equals 1.26 × 10^-2 for HSO₄^- and is 5.6 × 10^-10 for NH₄⁺. Which statement about the following equilibrium is correct? HSO₄^-(aq) + NH₃(aq) SO₄^2-(aq) + NH₄⁺(aq)

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What is the pH of a 0.20 M solution of NH₄Cl? [K_b(NH₃) = 1.8 × 10^-5]

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What is [OH^-] for a solution at 25°C that has [H₃O⁺] = 2.35 × 10^-3^M?

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Below is a representation of an aqueous solution of a weak acid HA at equilibrium. (Each circle represents 1.0 ×10^-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.) What is K_a of HA?

Correct Answer
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What mass of sodium nitrite must be added to enough water to make 350.0 mL of a solution with pH = 8.40? [K_a(HNO₂) = 5.6 × 10^-4]

Correct Answer
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