1. Label the substance below as an acid, base or neutral substance.
(a)pH = 7
(c) pH = 3
(e) pH = 13
(b) pOH = 9
(d) pOH = 4
(f) pOH = 7

1. Label the substance below as an acid, base or neutral substance.
(a)pH = 7 N
(c) pH = 3 A
(e) pH = 13 B
(b) pOH = 9
(d) pOH = 4
(f) pOH = 7
A
B
N

2. How does the Arrhenius theory define an acid?

2. How does the Arrhenius theory define an acid?
• An acid produces H
3
O + ions when dissolved in water.

3. How does the Arrhenius theory define an base?

3. How does the Arrhenius theory define an base?
• A base produces OH ions when dissolved in water.

4. Differentiate between an electrolyte and a nonelectrolyte.

4. Differentiate between an electrolyte and a nonelectrolyte.
• An electrolyte dissolves into ions when placed in water whereas a nonelectrolyte dissolves into molecules.

5. What type of substances are electrolytes?

5. What type of substances are electrolytes?
Acids, Bases, Salts

6. When H+ ions are dissolved in water they become hydronium ions. What is the formula for a hydronium ion?

6. When H+ ions are dissolved in water they become hydronium ions. What is the formula for a hydronium ion?
H
3
O +

7. What is the pH of a solution with a [H + ] = 4.32 x 10 -12 ?

7. What is the pH of a solution with a [H + ] = 4.32 x 10 -12 ?
pOH = 11.365

8. What is the pOH of a solution with a [OH ] = 6.83 x 10 -3 ?

8. What is the pOH of a solution with a [OH ] = 6.83 x 10 -3 ?
pOH = 2.166

9. What is the pOH of a solution with a pH = 3.8?

9. What is the pOH of a solution with a pH = 3.8?
pOH = 10.2

10. What is the [H + ] in a solution with a pH = 7.3?

10. What is the [H + ] in a solution with a pH = 7.3?
[H + ] = 5.0 x 10 -8

11. What is the [OH ] in a solution with a pOH = 10.7?

11. What is the [OH ] in a solution with a pOH = 10.7?
[OH ] = 2.0 x 10 -11

12. What is the pH of a solution with a [OH ] = 8.62 x 10 -5 ?

12. What is the pH of a solution with a [OH ] = 8.62 x 10 -5 ?
pH = 9.936

13a) Write the balanced equation for the acid-base neutralization of H
2
SO
4 and Ba(OH)
2
.

13a) Write the balanced equation for the acid-base neutralization of H
2
SO
4 and Ba(OH)
2
.
H
2
SO
4
+ Ba(OH)
2
→ BaSO
4
+ 2H
2
O

13b) Write the balanced equation for the acid-base neutralization of HF and NaOH.

13b) Write the balanced equation for the acid-base neutralization of HF and NaOH.
HF + NaOH → NaF + H
2
O

13c) Write the balanced equation for the acid-base neutralization of HI and Sr(OH)
2
.

13c) Write the balanced equation for the acid-base neutralization of HI and Sr(OH)
2
.
2HI + Sr(OH)
2
→ SrI
2
+ 2H
2
O

13d) We often use the equation
M acid x V acid
= M base x V base
.
Which of the acid-base neutralization reactions above could we not use this formula for? Explain.

13d) We often use the equation
M acid x V acid
= M base x V base
.
Which of the acid-base neutralization reactions above could we not use this formula for? Explain.
• The reaction between HI and Sr(OH)
2 could not be used because the acid and the base do not react in a 1:1 ratio.

13e) In an acid-base neutralization reaction
26 ml of Ba(OH)
2 reacts with 16 ml of
0.48M H
2
SO
4
. What is the molarity of the Ba(OH)2?

13e) In an acid-base neutralization reaction
26 ml of Ba(OH)
2 reacts with 16 ml of
0.48M H
2
SO
4
. What is the molarity of the Ba(OH)2?
0.30M

13f) How many milliliters of 0.57M HF will react with 39 ml of 0.86M NaOH in an acid-base neutralization reaction?

13f) How many milliliters of 0.57M HF will react with 39 ml of 0.86M NaOH in an acid-base neutralization reaction?
59 ml