Top of Form1. According to the Brnsted-Lowry definition, an base(Points : 10)

increases the H3O+ concentration in an aqueous solution. increases the OH- concentration in an aqueous solution. is a proton acceptor. is a proton donor. is an electron pair-acceptor.

2. What is the OH- concentration of an aqueous solution with a pH of 8.47? (Kw = 1.0 10-14)(Points : 10)

3.5 10-12 M 9.4 10-10 M 3.0 10-6 M 2.8 10-3 M 7.8 10-2 M

3. What is the pH of 9.2 10-3 M aqueous cyanide ion? (Kb of CN- = 2.5 10-5)(Points : 10)

2.04 3.33 4.60 9.40 10.67

4. An aqueous solution with a pH of 9.87 is diluted from 1.0 L to 1.5 L. What is the pH of the diluted solution?(Points : 10)

4.84 7.07 10.05 10.42 10.78

5. What is the conjugate base of H2PO4 - (aq)?(Points : 10)

H3O+ H3PO4 - HPO4 - 2 PO4 - 3 H4PO4 +1

6. At 15 C, the water ionization constant, Kw, is 3.8 10-15. What is the H3O+ concentration in neutral water at this temperature?(Points : 10)

2.0 10-29 M 4.5 10-15 M 6.7 10-8 M 6.16 10-8 M 2.2 M

7. If the Ka for lactic acid is 1.4 x 10-4, what is the Kb for the conjugate base of this acid?(Points : 10)

7.14 x 10-11 7.97 x 10-11 1.03 x 10-11 1.05 x 10-11 1.32 x 10-11

8. Which of the following chemical equations corresponds to Ka3 for phosphoric acid?(Points : 10)

HPO42-(aq) + H2O(l) PO43-(aq) + H3O+(aq) PO43-(aq) + H2O(l) HPO42-(aq) + OH-(aq) H3PO4(aq) + H2O(l) H2PO4-(aq) + H3O+(aq) H3PO4(aq) + 3 H2O(l) PO43-(aq) + 3 H3O+(aq) H2PO4-(aq) + H2O(l) HPO42-(aq) + H3O+(aq)

9. An aqueous solution with a pH of 1.89 is diluted from 2.0 L to 4.0 L. What is the pH of the diluted solution?(Points : 10)

1.50 1.73 2.19 3.30 6.00

10. What is the OH- concentration of an aqueous solution with a pH of -0.78? (Kw = 1.0 10-14)(Points : 10)

1.3 10-15 M 1.65 10-15 M 3.4 10-7 M 0.13 M 7.6 M

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