Question 1

Write the balanced chemical reaction between methyl amine (CH3NH2)and hydrobromic acid (HBr).

Accepted Answer

CH₃NH₂ + HBr...

Question 2

All of the following species are involved in the blood buffer system except

Accepted Answer

A)  CO2.
B)  H2CO3.
C)  HCO3-.
D)  CO32-.
E)  None of the above.

Question 3

Of the following four substances,which would form a basic solution when dissolved in water:
NH4Cl Cu(NO3) 2 K2CO3 NaF

Accepted Answer

A)  NH4Cl,Cu(NO3) 2
B)  K2CO3,NH4Cl
C)  NaF,K2CO3
D)  NaF only
E)  none of them

Question 4

Match the following.
-conjugate base

Accepted Answer

A)  the species that results when a base accepts a proton
B)  an acid-base theory that bases reactions on hydrogen and hydroxide ions
C)  a theory that treats acid-base reactions as proton-transfer reactions
D)  a substance which can behave as either an acid or a base
E)  the species that results when an acid donates a proton

Question 5

Acetic acid is a weak acid in water because it is

Accepted Answer

A)  dilute.
B)  only slightly soluble.
C)  unable to hold onto its hydrogen ion.
D)  only slightly dissociated into ions.
E)  completely dissociated into hydronium ions and acetate ions.

Question 6

Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?

Accepted Answer

A)  Ba2+ + 2 NO3- → Ba(NO3) 2
B)  H+ + NO3- → HNO3
C)  Ba2+ + 2 OH- → Ba(OH) 2
D)  H+ + OH- → H2O
E)  Ba(NO3) 2 + H2O → Ba2+ + 2 NO3-

Question 7

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

Accepted Answer

A)  12.61
B)  1.39
C)  1.10
D)  12.90
E)  4.10

Question 8

How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

Accepted Answer

A)  19.8 mL
B)  31.5 mL
C)  39.6 mL
D)  79.3 mL
E)  126 mL

Question 9

Which of these,if dissolved in 1.0 L of pure water,would produce a buffer solution?

Accepted Answer

A)  0.1 mol NaCl + 0.1 mol KCl
B)  0.1 mol H3O+ + 0.1 OH-
C)  0.1 mol NaH2PO4 + 0.1 mol Na2HPO4
D)  0.1 mol HCl + 0.1 mol NaOH
E)  0.1 mol H3O+ + 0.1 mol Cl-

Question 10

According to Brønsted-Lowry theory,acid-base reactions can be described as ________ reactions.

Accepted Answer

A)  electrolytic
B)  electron transfer
C)  gas phase
D)  nuclear transfer
E)  proton transfer

Question 11

The net ionic equation for the reaction of formic acid,a weak acid,with potassium hydroxide,a strong base,is

Accepted Answer

A)  HCO2H(aq) + KOH(aq) → KHCO2(aq) + H2O(l) .
B)  HCO2H(aq) + K+(aq) + OH-(aq) → K+(aq) + HCO2-(aq) + H2O(l) .
C)  HCO2H(aq) + OH-(aq) → HCO2-(aq) + H2O(l) .
D)  HCO2-(aq) + KOH(aq) → KHCO2(aq) + OH-(aq) .
E)  H+(aq) + HCO2-(aq) + K+(aq) + OH-(aq) → K+(aq) + HCO2-(aq) + H2O(l) .

Question 12

What is the value of [H3O+] in a solution with pH = 10.82?

Accepted Answer

A)  6.6 × 10-4 M
B)  1.5 × 10-11 M
C)  1.03 M
D)  10.82 M
E)  3.18 M

Question 13

A Brønsted-Lowry base is a substance which

Accepted Answer

A)  produces hydrogen ions in aqueous solution.
B)  produces hydroxide ions in aqueous solution.
C)  donates protons to other substances.
D)  accepts protons from other substances.
E)  accepts hydronium ions from other substances.

Question 14

Which statement concerning Arrhenius acid-base theory is not correct?

Accepted Answer

A)  An Arrhenius acid produces hydrogen ions in water solution.
B)  An Arrhenius base produces hydroxide ions in water solution.
C)  A neutralization reaction produces water plus a salt.
D)  Acid-base reactions must take place in aqueous solution.
E)  none of the above

Question 15

Which compound has a very large value of Ka in aqueous solution?

Accepted Answer

A)  NaCl
B)  HNO3
C)  H3PO4
D)  KOH
E)  NH3

Question 16

In an aqueous solution that is basic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Accepted Answer

A)  greater;less
B)  less;greater
C)  greater;greater
D)  less;less
E)  none of the above

Question 17

Which statement is correct for pure water?

Accepted Answer

A)  Pure water contains equal amounts of hydroxide,[OH-],and hydronium,[H3O+],ions.
B)  Pure water contains larger amounts of hydroxide,[OH-],ions than hydronium,[H3O+],ions.
C)  Pure water contains larger amounts of hydronium,[H3O+],ions than hydroxide,[OH-],ions.
D)  Pure water is an electrolyte.
E)  Pure water contains no ions.

Question 18

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Accepted Answer

A)  7.65 M
B)  6.35 M
C)  4.5 × 10-7 M
D)  0.80 M
E)  2.2 × 10-8 M

Question 19

A necessary requirement for a Brønsted base is

Accepted Answer

A)  the presence of water as a reaction medium.
B)  the presence of hydroxide in its formula.
C)  a lone pair of electrons in its Lewis dot structure.
D)  the production of hydronium ion upon reaction with water.
E)  the presence of a metal ion in its formula.

Question 20

At 25°C,the value of Kw is

Accepted Answer

A)  1.00.
B)  1.00 × 10-7.
C)  1.00 × 10-14.
D)  1.00 × 107.
E)  1.00 × 1014.

Exam 10: Acids and Bases

How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

Correct AnswerverifiedShow Answer

Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?

Correct AnswerverifiedShow Answer

What is the value of [H3O+] in a solution with pH = 10.82?

Correct AnswerverifiedShow Answer

At 25°C,the value of Kw is

Correct AnswerverifiedShow Answer

Which statement is correct for pure water?

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Which compound has a very large value of Ka in aqueous solution?

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Which of these,if dissolved in 1.0 L of pure water,would produce a buffer solution?

Correct AnswerverifiedShow Answer

In an aqueous solution that is basic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Correct AnswerverifiedShow Answer

Which statement concerning Arrhenius acid-base theory is not correct?

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Match the following. -conjugate base

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A Brønsted-Lowry base is a substance which

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According to Brønsted-Lowry theory,acid-base reactions can be described as ________ reactions.

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Write the balanced chemical reaction between methyl amine (CH3NH2)and hydrobromic acid (HBr).

Correct AnswerverifiedCH3NH2 + HBr...View AnswerShow Answer

All of the following species are involved in the blood buffer system except

Correct AnswerverifiedShow Answer

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

Correct AnswerverifiedShow Answer

A necessary requirement for a Brønsted base is

Correct AnswerverifiedShow Answer

The net ionic equation for the reaction of formic acid,a weak acid,with potassium hydroxide,a strong base,is

Correct AnswerverifiedShow Answer

Of the following four substances,which would form a basic solution when dissolved in water: NH4Cl Cu(NO3) 2 K2CO3 NaF

Correct AnswerverifiedShow Answer

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Correct AnswerverifiedShow Answer

Acetic acid is a weak acid in water because it is

Correct AnswerverifiedShow Answer

How many mL of 0.241 M H₂SO₄ will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

Correct Answer
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What is the value of [H₃O⁺] in a solution with pH = 10.82?

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At 25°C,the value of K_w is

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Which compound has a very large value of K_a in aqueous solution?

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In an aqueous solution that is basic,[H₃O⁺] is than 1.0 × 10^-7 and than [OH^-].

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Write the balanced chemical reaction between methyl amine (CH₃NH₂)and hydrobromic acid (HBr).

Correct Answer
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CH₃NH₂ + HBr...
View Answer

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What is the pH of a solution in which [H₃O⁺] = 4.1 × 10^-2 M?

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Of the following four substances,which would form a basic solution when dissolved in water: NH₄Cl Cu(NO₃) ₂ K₂CO₃ NaF

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