Deck 12: Acids and Bases

Question 1

The Brønsted-Lowry definition of acid and base is limited to aqueous (that is, water) solutions.

Answer 1

False

Question 2

H⁺ ions and H₃O⁺ ions are often considered interchangeable when writing chemical equations.

Answer 2

True

Question 3

Salts with ions that are part of weak acids or bases will not hydrolyze, while salts with ions that are part of strong acids or bases will hydrolyze.

Answer 3

False

Question 4

If pOH < 7, then the solution is acidic.

Question 5

A reaction between an acid and a base is called a combustion reaction.

Question 6

HClO₄ is a weak acid.

Question 7

A base is always the titrant.

Question 8

An Arrhenius acid is an ionic compound.

Question 9

NaCl is an Arrhenius base.

Question 10

Mg(OH)₂ is a weak base.

Question 11

If pH > 7, then the solution is basic.

Question 12

The product of the two concentrations-[H⁺][OH⁻]-is always equal to 1.0 × 10⁻¹⁴.

Question 13

Consider the product of the two concentrations, [H⁺][OH⁻]. If one concentration goes up, the other must go up to compensate so that their product equals the value of the autoionization constant of water.

Question 14

An Arrhenius acid is a compound that increases the hydroxide ion concentration in aqueous solution.

Question 15

In the reaction H₃PO₄ + OH⁻ $\rightarrow$ H₂PO₄⁻ + H₂O, H₃PO₄ and H₂PO₄⁻ are a conjugate acid-base pair.

Question 16

The titrant is added to the analyte using a precisely calibrated volumetric delivery tube called a buret.

Question 17

LiOH is strong base.

Question 18

When ammonia reacts with water, ammonia acts like a Brønsted-Lowry base.

Question 19

HCOOH is a strong acid.

Question 20

HCl is an Arrhenius acid.

Question 21

Chemistry defines the _____ ion as the actual chemical species that represents an H⁺ ion.

A) phosphate
B) sulfate
C) nitrate
D) nitrite
E) hydronium

Question 22

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. H₂C₂O₄ + 2F⁻ $\rightarrow$ ?

A) 2H₂C₂O₄ and F⁻
B) C₂O₄²⁻ and 2HF
C) C₂O₄ and 2F⁻
D) H₂C₂O₃^- and F₂
E) C₂O₃^- and 2F₂

Question 23

Which of the following is required to react with Zn(OH)₂ to produce Zn₃(PO₄)₂?

A) H₂PO₃
B) H₂PO₄
C) HPO₄
D) H₃PO₄
E) H₂P₂O₄

Question 24

Small amounts of weak acids and bases can change the pH of a solution very quickly.

Question 25

[OH⁻] = 10^{−pOH + pH}

Question 26

Which of the following statements is true about acids?

A) Acids turn litmus, a plant extract, red.
B) Acids react with hydrogen carbonate to give of N₂ gas.
C) Acids that are ingested typically have a sweet taste.
D) Acids are slippery to touch.
E) Acids increase the concentration of hydroxide ions in a solution.

Question 27

What is the conjugate acid of ClO₄^-?

A) HClO₃^2-
B) ClO₄^-
C) HClO₄
D) H₂ClO₄⁺
E) H₂ClO₄^-

Question 28

Pure water (pOH = 7) is an acidic solution.

Question 29

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. HCOOH + C₅H₅N $\rightarrow$ ?

A) HCOON and C₆H₆
B) HCOO^- and C₅H₅NH⁺
C) HCOOH₂⁺ and C₅H₄N^-
D) H₂COOH₂⁺ and C₅H₃N^-
E) CHCOOH and C₄H₅N^-

Question 30

A Brønsted-Lowry acid is any species that can donate a(n) _____to another molecule.

A) hydroxide (OH^-) ion
B) water (H₂O) molecule
C) proton (H⁺)
D) ammonium (NH₄⁺) ion
E) electron (e^-)

Question 31

HN₃ and NH₃ can make a buffer.

Question 32

Complete the following reaction. ? + H₂O $\rightarrow$ C₆H₅COO^- + H₃O⁺

A) C₆H₅COOH
B) C₇H₈COOH
C) C₆H₁₃COOH
D) C₅H₁₁COOH
E) C₇H₁₅COOH

Question 33

A reaction between an acid and a base is called a(n):

A) combustion reaction.
B) decomposition reaction.
C) hydrogenation reaction.
D) neutralization reaction.
E) alkylation reaction.

Question 34

Which of the following is an Arrhenius base?

A) HC₂H₃O₂
B) HClO₃
C) Al(OH)₃
D) PCl₅
E) HgCl₂

Question 35

Which of the following is formed when H₂SO₃ reacts with KOH?

A) K₂SO₄
B) K₂SO₃
C) K₂(SO₄)₃
D) KH
E) KOH

Question 36

pH + pOH = 14

Question 37

What is the conjugate acid of H₂O?

A) H₂O⁺
B) H₂O₂^-
C) HO₃^-
D) HO₃⁺
E) H₃O⁺

Question 38

Complete the following reaction. ? + 2HNO₃ $\rightarrow$ Sr(NO₃)₂ + 2H₂O

A) Sr(OH)₂
B) SrNO₃
C) Sr₂NO₃
D) SrOH₂
E) SrON₃

Question 39

Which of the following is an Arrhenius acid?

A) H₂SO₃
B) NaOH
C) Na₂CO₃
D) HgI₂
E) Al₂(SO₄)₃

Question 40

Which of the following is not an Arrhenius acid?

A) H₂SO₃
B) H₂SO₄
C) HClO₄
D) HI
E) Li₂SO₄

Question 41

What is the conjugate base of HClO₃?

A) HClO₃^-
B) HClO₃⁺
C) ClO₃^-
D) H₂ClO₃^-
E) ClO₄^-

Question 42

Which of the following is a weak acid?

A) HCl
B) H₂SO₄
C) H₃PO₄
D) HI
E) HClO₄

Question 43

What is the pH of a solution when [OH^-] is 8.04 × 10⁻¹³ M?

A) 0.904
B) 1.91
C) 0.975
D) 14.0
E) 12.09

Question 44

What is [H⁺] in a 0.0066 M solution of Ba(OH)₂?

A) 7.6 * 10^-13 M
B) 1.0 * 10¹⁴ M
C) 1.0 * 10^-13 M
D) 1.5 * 10^-12 M
E) 0.0066 M

Question 45

Which of the following is an acidic salt?

A) RbCl
B) Sr(NO₂)₂
C) CaNO₂
D) CaBr₂
E) MnI₂

Question 46

Which of the following is a strong base?

A) Sr(OH)₂
B) Hg(OH)₂
C) Mn(OH)₂
D) Fe(OH)₂
E) Fe(OH)₃

Question 47

Which of the following acids ionizes 100% in aqueous solution?

A) HBr
B) HBrO₃
C) HNO₂
D) HCOOH
E) CH₃COOH

Question 48

What is [OH⁻] for an aqueous solution whose pH is 3.89?

A) 7.76 *10^-11 M
B) 1.29*10^-12 M
C) 1.29 * 10¹² M
D) 2.58 * 10¹² M
E) 3.86 * 10^-12 M

Question 49

What is the conjugate base of C₅H₅NH⁺?

A) C₅H₅NH²⁺
B) C₅H₅NH^-
C) C₅H₅NH₂⁺
D) C₅H₅NH₂
E) C₅H₅N

Question 50

Which of the following bases does not ionize 100% in aqueous solution?

A) LiOH
B) Mg(OH)₂
C) KOH
D) Ca(OH)₂
E) Ni(OH)₂

Question 51

A 0.0788 M solution of HC₂H₃O₂ is 3.0% ionized into H⁺ ions and C₂H₃O₂⁻ ions. What is [OH⁻] for this solution?

A) 8.5 *10^-12 M
B) 2.1 *10^-12 M
C) 4.2 *10^-12 M
D) 8.5 * 10¹² M
E) 0.0788 M

Question 52

A 0.0111 M solution of Sn(OH)₂ is 0.585% ionized into Sn²⁺ and OH^- ions. What is [H⁺] for this solution?

A) 1.54 * 10^-10 M
B) 7.70 *10^-11 M
C) 3.08 *10^-10 M
D) 7.70 * 10¹¹ M
E) 0.0111 M

Question 53

What is [OH^-] in a 0.077 M solution of HClO₄?

A) 7.6 *10^-13 M
B) 1.3 *10^-13 M
C) 6.5 * 10^-14 M
D) 6.5 * 10¹⁴ M
E) 0.077 M

Question 54

The concentration of both H⁺(aq) and OH⁻(aq) in a sample of pure H₂O is about:

A) 1.0 * 10⁷ M.
B) 1.0 * 10^-7 M.
C) 1.0 *10^-14 M.
D) 1.0 * 10^-10 M.
E) 1.0 * 10^-21 M.

Question 55

Which of the following is a basic salt?

A) LiCl
B) RbBr
C) KNO₂
D) NaI
E) NH₄Cl

Question 56

What is [H⁺] for an aqueous solution whose pOH is 9.89?

A) 2.33 * 10^-6 M
B) 7.76 *10^-5 M
C) 2.33 * 10⁶ M
D) 4.11 M
E) 1.55*10^-6 M

Question 57

Which of the following is a neutral salt?

A) Al₂(SO₄)₃
B) Ti(NO₃)₂
C) Ti(PO₄)₃
D) Fe(ClO₃)₂
E) Ba(NO₃)₂

Question 58

What is [H⁺] of an aqueous solution if [OH⁻] is 1.0 × 10⁻⁵ M?

A) 1.0*10^-8 M
B) 1.0 * 10^-14 M
C) 1.0 * 10⁷ M
D) 1.0 * 10^-7 M
E) 1.0 * 10^-9 M

Question 59

What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO₃? The balanced chemical equation is as follows: AgOH + HNO₃ $\rightarrow$ AgNO₃ + H₂O

A) 0.485 g
B) 0.00388 g
C) 258 g
D) 1.13 g
E) 2.27 g

Question 60

What is [OH⁻] of an aqueous solution if [H⁺] is 1.0 × 10⁻⁷ M?

A) 1.0 * 10^-14 M
B) 1.0 *10^-5 M
C) 1.0 * 10⁵ M
D) 1.0 * 10^-7 M
E) 1.0 * 10^-21 M

Question 61

What is the pOH of a solution when [H⁺] is 5.88 × 10⁻¹¹ M?

A) 10.1
B) 7.88
C) 10.23
D) 3.77
E) 15.6

Question 62

Briefly describe conjugate acid-base pairs.

Question 63

Which of the following can be a component in a buffer?

A) LiBr
B) NaI
C) KNO₃
D) K₃PO₄
E) SrI₂

Question 64

Why is ammonia unique from the other bases? Describe the hydrolysis of ammonia.

Question 65

Which of the following combinations of compounds can make a buffer solution?

A) HCOOH and CH₃COOH
B) NaCl and BaCl₂
C) HCl and Ca(OH)₂
D) H₃PO₄ and Li₃PO₄
E) NH₃ and NaOH

Question 66

Which of the combinations of compounds can make a buffer solution?

A) HCl and LiCl
B) HNO₂ and HF
C) RbOH and CsOH
D) Rb₂SO₄ and HNO₃
E) NH₄NO₃ and NH₃

Question 67

Describe the process of titration.

Question 68

Differentiate between Arrhenius acids and Arrhenius bases.

Question 69

Differentiate between strong bases and weak bases. Give an example of two strong acids and two strong bases.

Question 70

Which of the combinations of compounds can make a buffer solution?

A) Ca(HCO₃)₂ and Ca(OH)₂
B) CH₃NH₂ and CH₃NH₃Br
C) NaOH and NaCl
D) HCl and NaCl
E) NH₃ and Ca(OH)₂

Question 71

Explain how the pH scale can be used to determine whether a given aqueous solution is acidic, basic, or neutral.

Question 72

Explain why KNO₃ cannot be a component in either an acidic or a basic buffer.

Question 73

Explain neutralization reactions with examples.

Question 74

Describe amphiprotic substances with an example.

Question 75

Differentiate between strong acids and weak acids.

Question 76

Which of the combinations of compounds can make a buffer solution?

A) LiOH and LiCl
B) NaOH and NaBr
C) NaNO₃ and Ca(NO₃)₂
D) NaHCO₃ and Na₂CO₃
E) HN₃ and NH₃

Question 77

Demonstrate how a buffer works.

Question 78

What are the rules required to determine whether a solution is acidic or basic?

Question 79

Differentiate Brønsted-Lowry acids and Brønsted-Lowry bases.

Question 80

Briefly describe autoionization of water. What is the autoionization constant of water?