Important equations pH = pK, + log[salt],[acid] pOH = pKb + log[salt]/[base] acidic basic pKalog Ka pK,log Kb Acid Acetic acid Benzoic acid CH2COOH CsH5COOH HCOOH Ka 1.8 x 10-5 Sodium salt NaCH3COC NaC6H.СОО NaCN | 63 X 10-5 Hydrocyanic acid HCN Formic acid Hypobromous acid HOBr Hypochlorous acid HOC Hypoiodous acid Nitrous acid Chlorous acid HCIO2 6.2 x 10-10 1.8 x 10-4 NaHCOO 2.3 x 109 NaOBr NaOCl NaOI NaNO2 2.9 x 10-8 2.3 X 10-11 7,1 x 10-4 1.1 x 10-2 HNO2 Chlorous acid NaCIO2 *Table values from Silberberg, 4th Edition Solve the following problems 1. Find the pH of a buffer in which [HCOOH] 1.24 M and [HCOONa] 0.82 M Given that Buffer A contains 20o.o mL o.050 M HOCl and 400.0 mL o.030 M NaoCl calculate 2. a. The pH of the buffer solution b. The pH of the solution after adding 10.0 mL 0.50 M HC. c. The pH of the solution after adding 20.0 mL o.40 M NaOH

Important equations pH = pK, + log[salt],[acid] pOH = pKb + log[salt]/[base] acidic basic pKalog Ka pK,log Kb Acid Acetic acid Benzoic acid CH2COOH CsH5COOH HCOOH Ka 1.8 x 10-5 Sodium salt NaCH3COC NaC6H.СОО NaCN | 63 X 10-5 Hydrocyanic acid HCN Formic acid Hypobromous acid HOBr Hypochlorous acid HOC Hypoiodous acid Nitrous acid Chlorous acid HCIO2 6.2 x 10-10 1.8 x 10-4 NaHCOO 2.3 x 109 NaOBr NaOCl NaOI NaNO2 2.9 x 10-8 2.3 X 10-11 7,1 x 10-4 1.1 x 10-2 HNO2 Chlorous acid NaCIO2 *Table values from Silberberg, 4th Edition Solve the following problems 1. Find the pH of a buffer in which [HCOOH] 1.24 M and [HCOONa] 0.82 M Given that Buffer A contains 20o.o mL o.050 M HOCl and 400.0 mL o.030 M NaoCl calculate 2. a. The pH of the buffer solution b. The pH of the solution after adding 10.0 mL 0.50 M HC. c. The pH of the solution after adding 20.0 mL o.40 M NaOH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 35Q: Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] =...

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