Homework GOB Week 4

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Question #1

For many reactions of acids with bases, the resulting products are a salt and water.

A FALSE

B TRUE

Question #2

An aqueous solution with [OH-] = 1.0 x 10-12 has a pH of 12.0.

A TRUE

B FALSE

Question #3

In any water solution, [H3O+] [OH-] = 1.0 x 10-7.

A FALSE

B TRUE

Question #4

A solution with a pH greater than 7 is basic.

A FALSE

B TRUE

Question #5

An acidic solution has a pH less than 7.0.

A TRUE

B FALSE

Question #6

If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.

A FALSE

B TRUE

Question #7

According to the Bronsted-Lowry definition,

A a base produces H+ ions in aqueous solutions.

B an acid acts as the solvent.

C a base is a proton acceptor.

D a base is a proton donor.

E an acid is a proton acceptor.

Question #8

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is

A 0.115 M.

B 0.390 M.

C 0.212 M.

D 0.137 M.

E 0.500 M.

Question #9

Which of the following is a neutralization reaction?

A HNO3 + KOH → H2O + KNO3

B H2O + SO3 → H2SO4

C 2NO2 → 2NO + O2

D KCl + NaNO3 → KNO3 + NaCl

Question #10

The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula

A NO3OH.

B Al(NO3)3.

C H2O.

D AlNO3.

Question #11

Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 by Ca(OH)2?

A H3PO4 + Ca(OH)2 → Ca3(PO4)2 + H2O

B 4H3PO4 + 6Ca(OH)2 → 2Ca3(PO4)2 + 12H2O

C H3PO4 + Ca(OH)2 → CaHPO4 + 2H2O

D 3H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5H2O

E 2H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6H2O

Question #12

In a neutralization reaction

A two acids react to form water.

B a base and a salt react to form water and an acid.

C an acid and a base react to form a salt and water.

D an acid and a salt react to form water and a base.

E water and a salt react to form an acid and a base.

Question #13

An acid and base react to form a salt and water in a(n) ________ reaction.

A dissociation

B neutralization

C reduction

D ionization

E oxidation

Question #14

Ammonium hydroxide is a weak base because

A is a poor acceptor of protons.

B it is a dilute solution.

C it dissociates only slightly in water.

D it is completely ionized in aqueous solution.

E it is only slightly soluble in water.

Question #15

A solution with [ OH-] of 5 x 10-3 has a pH of ________.

A 11.7

B 5.0

C 2.3

D -2.3

E 7.0

Question #16

The name given to an aqueous solution of HBr is

A bromic acid.

B hydrogen bromide.

C hydrobromic acid.

D bromous acid.

E hypobromous acid.

Question #17

Which of the following is the strongest acid?

A H3PO4

B H2CO3

C NaOH

D NH4+

E HCl

Question #18

The [H3O+] of a solution with pH = 8.7 is

A 2 x 10-9 M.

B 8.7 x 10-1 M.

C 5 x 10-6 M.

D 8.7 M.

E 5.3 M.

Question #19

The [H3O+] of a solution with pH = 2.0 is

A 1 x 102 M.

B 1 x 10-12 M.

C 10 M.

D -10 M.

E 1 x 10-2 M.

Question #20

What is the pH of a solution with [OH-] = 1 x 10-4 M?

A 4.0

B -10.0

C 10.0

D -4.0

E 1.0 x 10-10

Question #21

What is the [OH-] in a solution that has a [H3O+] = 1 x 10-6 M?

A 1 x 10-6 M

B 1 x 10-2 M

C 1 x 10-12 M

D 1 x 10-10 M

E 1 x 10-8 M

Question #22

What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M?

A 1 x 10-2 M

B 1 x 10-7 M

C 1 x 10-8 M

D 1 x 10-12 M

E 1 x 102 M

Question #23

For Kw, the product of [H3O+] and [OH-] is

A 1.0 X 10-7

B 1.0

C 1.0 X 1014

D 1.0 X 10-14

E 1.0 X 10-1

Question #24

In water, a substance that ionizes completely in solution is called a

A nonconductor.

B nonelectrolyte.

C weak electrolyte.

D semiconductor.

E strong electrolyte.

Question #25

What mass of KCl is in 350 mL of 0.24 M KCl?

A 0.84 g

B 84 g

C 6.3 g

D 18 g

E 1.1.g

Question #26

What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH?

A 0.75 L

B 0.083 L

C 0.075 L

D 750 L

E 0.25 L

Question #27

What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?

A 2.00 M

B 1.50 M

C 1.00 M

D 0.500 M

E 4.00 M

Question #28

The molarity (M) of a solution refers to

A moles of solute/L of solution.

B moles of solute/100 mL of solution.

C moles of solute/ L of solvent.

D grams of solute/L of solution.

E grams of solute/100 mL of solution.

Question #29

In a solution, the solvent

A can be a solid, liquid, or gas.

B is the substance present in the smallest concentration.

C is never a solid.

D can be a liquid or gas.

E is a liquid.

Question #30

The mass percent concentration refers to

A grams of solute in 100 g of solvent.

B grams of solute in 1 kg of solvent.

C grams of solute in 100 g of solution.

D grams of solute in 1 kg of solution.

E grams of solvent in 100 g of solution.

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