Chapter 16 Review WS
11-12
1. What value does Kw have at 25ºC? 1.0 x 10-14
2. What are [H+] and [OH-] in pure water at 25º? 1.0 x 10-7
3. How does [H+] compare to [OH-] in an acidic solution? [H+] > [OH-]
4. How does [H+] compare to [OH-] in a basic solution? [H+] < [OH-]
5. What range of pH values corresponds to acidic solutions? pH < 7
6. What range of pH values corresponds to basic solutions? pH > 7
7. Identify each as an acid or a base:
a) H2SO4 acid
b) HCl
acid
c)
HNO3
acid
d) NaOH base
e) H3PO4
acid
f)
Mg(OH)2
base
8. Classify each solution as neutral, acidic, or basic.
a) [H+] = 1 x 10-5
acidic
b) [H+] = 1 x 10-7 neutral
c) [OH-] = 1 x 10-5
basic
9. A solution has a pH of 3. What is the [H+] concentration? 0.001 M
10. A solution has a [H+] concentration of 1.0 x 10-5. What is the pH? 5.00
11. A solution has a [OH-] concentration of 2.7 x 10-5. What is the pH? 9.43
12. Fill in the blanks.
In the reaction of an acid with a base, hydrogen ions and _hydroxide_ ions react to produce _water_ and a
salt. This reaction is called _neutralization_.
13. Write the formula for these acids:
hydrochloric acid
HCl
acids_bases_review.doc
sulfuric acid
H2SO4
phosphoric acid
H3PO4
acetic acid
HC2H3O2
nitric acid
HNO3
Write the equation for the neutralization reactions.
14.
Write the equation for the dissociation (breaking up into ions!) of the following acids and bases.
a) HCl  H+ + Clb) H3PO4  3 H+ + PO43c) NaOH  Na+ + OHd) NH4OH  NH4+ + OH-
15.
3 HCl + Al(OH)3  AlCl3 + 3 H2O
16.
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O
17.
How many moles of sulfuric acid are needed to react with 3.5 moles of sodium hydroxide?
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O
3.5 mol NaOH 1 mol H2SO4

= 1.8 mol H2SO4
1
2 mol NaOH
18.
How many liters of 0.75 M sodium hydroxide are needed to react with 2.7 L of 0.55 M hydrochloric
acid?
HCl + NaOH  NaCl + H2O
2.7 L HCl 0.55 mol HCl 1 mol NaOH
1 L NaOH



= 2.0 L NaOH
1
1 L HCl
1 mol HCl 0.75 mol NaOH
19. How many milliliters of 0.35 M phosphoric acid will completely neutralize 450.0 mL of 0.50 M calcium
hydroxide?
2 H3PO4 + 3 Ca(OH)2  Ca3(PO4)2 + 6 H2O
1 L H3PO4
450.0 mL Ca(OH)2
0.50 mol Ca(OH)2 2 mol H3PO4
1L
1000 mL
×
×
×
×
×
= 428.6 mL H3PO 4
1
1000 mL
1 L Ca(OH)2
3 mol Ca(OH)2 0.35 mol H3PO4
1L
acids_bases_review.doc