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1442test3

# 1442test3 - 1442 Test 3 Chapters 18 and 19 Silberberg...

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1442 Test 3 Chapters 18 and 19 Silberberg Website: http://dipowell.home.mindspring.com pH = -log [H + ] pOH = -log [OH] pH + pOH = 14 [H + ][OH - ] = 1 x 10 -14 Ka X Kb = 1 X 10 -14 pH = pKa + log [base] / [acid] Simple pH problems ______ _____1. PH = 3.4, H + =____ (3.98 X 10 -4 ) ___________2. OH - = 1.2 X 10 -6 , pH = ______ (8.08) pH of Strong Acids and Bases ___________3. What is the pH of a 0.08 M HBr solution? (1.1) ___________4. What is the pH of a 0.05 M Ca(OH) 2 solution? (13) pH of Weak acids and Bases ___________ 5. What is the pH of a 0.5 M HOCl solution? Ka = 3.5 X 10 -8 (3.88) ___________6. What is the pH of a 0.3 M C 6 H 5 NH 2 solution? Kb = 4.2 X 10 -10 (9.05) ___________7. A 0.1 M HX solution is 3% ionized. What is the value of Ka? (9.28 X 10 -5 ) ___________8. A 0.10 M HX solution has a pH of 2. What is the Ka? (1.1 X 10 -3 ) pH of Buffer Solutions ___________9. 200 ml of 0.1 M HF and 300 ml of 0.1 NaF are mixed. What is the pH of the solution? Ka = 7.2 X 10 -4 (3.3) ___________10. 0.02 mole of NH 3 and 0.03 mole of NH 4 Cl are mixed in 300 ml. What is the pH of the solution? Kb = 1.8 X 10 -5 (9.1) Buffering Action ___________11. 0.01 mole of HCl is added to 1 liter of a buffer which contains 0.02 mole of NH 3 and 0.03 mole of NH 4 Cl. What is the pH of the solution after all are mixed? (Kb NH 3 = 1.8 X 10 -5 ) (8.65) ___________12. 0.040 mole of NaOH is added to a buffer containing 0.05 mole of CH 3 COOH and 0.07 mole of CH 3 COONa in 300 ml. What is the pH of the mixture. Ka CH 3 COOH = 1.8 X 10 -5 (5.8) ___________13. 0.05 mole of HCl is added to a liter of buffer containing 0.04 mole of NH 3 and 0.03 mole of NH 4 Cl. What is the pH? Kb = 1.8 X 10 -5 (2) Titration Problems

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___________14. 30 ml of 0.1 M NaOH is added to 28 ml of 0.10 M HCl. What is the pH? (11.5) ___________15. 30 ml of 0.20 M NH 3 and 25 ml of 0.20 HCl are mixed. What is the pH? Kb NH 3 = 1.8 X 10 -5 (8.6) Salt Solutions ___________16. What is the pH of a 0.10 M NaF solution? Ka HF = 7.2 X 10 -4 (8.1) ___________17. What is the pH of a 0.10 M NH 4 Cl solution? Kb NH 3 = 1.8 X 10 -5 (5.1) ___________18.
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