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Discussion9key_000 - 4 What is the pH of a 0.10 M solution...

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C118 Discussion Worksheet #9 Ch. 6 Neutralizing the Threat of Acid Rain Ch. 6 End of Chapter Problems: 1, 2, 3, 4, 6, 7, 8, 9, 11, 12, 13 End of Chapter Problems will not be graded but are highly recommended. 1. Calculate the pH of the following solutions. a. 5.4 x 10 -4 M HNO 3 b. 0.1 M NaOH c. 3 x 10 -5 M Mg(OH) 2 a. pH = 3.26 b. pH = 13 c. pH = 7.77 2. Calculate the [H+] in blood if the pH is 7.35. [H+] = 10 -7.35 = 4.46 x 10 -8 3. a. List the 6 strong acids HCl, HBr, HI, HNO 3 , H2SO 4 , HClO 4 b. List the strong bases hydroxides of group 1 and 2 metals c. What is the difference between a strong and weak acid? Strong means 100% dissociated in water and weak means only partially dissociated (or ionized).
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Unformatted text preview: 4. What is the pH of a 0.10 M solution of acetic acid (CH 3 COOH)? K a = 1.8 x 10-5 HA H+ + A-Initial 0.1 Change-x +x +x Equilibrium 0.1-x x x x = 1.34 x 10-3 = [H + ] Therefore, pH = - log [H + ] = 2.87 5. What is the K a of butanoic acid, CH 3 CH 2 CH 2 COOH, if a 0.025 M solution has a pH of 3.21? HA H+ + A-Initial 0.025 Change-x +x +x Equilibrium 0.025-x x x Since the pH = 3.21, the [H+] concentration can be calculated to be 6.17 x 10-4 . Therefore x = 6.17 x 10-4 ....
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