Chapter 15 pH Study Guide

What is the concentration of hydronium ions in pure water?

1.0 x 10(-7) M

As the [H3O+] of a solution increases, the value of

a. log [H3O+] increases
b. -log [H3O+] decreases
c. the solution’s pH decreases
d. All of the above

All of the above

The pH of a solution is defined as

-log [H3O+]

Which of the following is not a property of an acidic solution?

[HO-] greater than 1 X 10(-7) M

A basic solution

has a lower concentration of hydronium ions than hydroxide ions

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Which of the following substances is a weak base?

a. NH3
b. KOH
c. N2O
d. NaOH

NH3

A solution that has a pH of 13 is a

Strong base

What is the pH of household ammonia in which the [H3O+] is 1.0 X 10(-12) M?

a. 2
b. 7
c. 10
d. 12

12

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What is the [OH-] in a sample of lime juice with a pH of 2.0?

1.0 X 10(-12) M

An acid-base indicator
a. is either a weak acid or a weak base.
b. has a different color at a different pH.
c. can be used to find the equivalence point.
d. All of the above

All of the above

A pH meter measures the

voltage difference between two electrodes in solution

A titration always involves the

controlled addition of a standard solution

For any acid titrated with a base, the equivalence point occurs when the

acid and base are present in chemically equivalent amounts

1×10-4 M HCl

HCl→H +Cl (1×10-4 H) (1×10-4 Cl) {H3O+}=1×10-4
kw=(H3O+)*(OH-)
1×10-14=(1×10-4)* (OH)
OH-=1×10-14/1×10-4=1×10-10M

1 x 10-4 M NaOH

NaOHNa+OH OH=1×10-4
H3O=1×10-14/1×10-4=1×10-10

What is the molarity of a solution of H2SO4 if 49.0 mL of it are neutralized by 68.4 mL of 0.333 M NaOH solution?

.0684L*0.333=0.023molNaOH
0.023x1molh2so4/2molNaOH=0.011mol H2SO4
1×10-5

1 x 10-4 M Ca(OH)2

Ca(OH)2Ca2 + 2OH- 2*(1*10-4) 2*10-4=OH
H3O 1×10-14/2×10-4 = 5×10-11

1 x 10-4 M HNO3

HNO3→H+NO3 1×10-4H 1×10-4NO3 kw=H3O*OH
OH=1×10-14/1×10-4=1×10-10M

5 x 10-4 M HClO4

H+ClO4 5×10-4 kw=1×10-14/5×10-4= 2×10-11

If 72.1 mL of 0.543 M H2SO4 are needed to neutralize 39.0 mL of KOH solution, what is the molarity of the KOH solution?

0.543M*0.0721L=0.039mol H2SO4
0.039molH2SO4x2molKOH/1molH2SO4=0.078mol
0.232M

What is the hydronium ion concentration of an aqueous solution that has a pH of 5.0?

H30=antilog (-pH)
1 x 10-5