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Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 10-* Complete Parts 1-4 before submitting your answer. NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) HCIO(aq) OH(aq) HO(1) + CIO (aq) RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040 < PREV NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HCIO(aq) + H:O(1) = HỌ (aq) CIO (aq) RESET 0.40 0.13 0.37 0.010 0.040 0.10 +x 0.13 + x 0.13-x 0.010 + x 0.010-x 0.040 + x 0.040-x 0.10+x 0.10-x 0.40+x 0.40-x < PREV 2 NEXT > Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89

Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 10-* Complete Parts 1-4 before submitting your answer. NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) HCIO(aq) OH(aq) HO(1) + CIO (aq) RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040 < PREV NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HCIO(aq) + H:O(1) = HỌ (aq) CIO (aq) RESET 0.40 0.13 0.37 0.010 0.040 0.10 +x 0.13 + x 0.13-x 0.010 + x 0.010-x 0.040 + x 0.040-x 0.10+x 0.10-x 0.40+x 0.40-x < PREV 2 NEXT > Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 10-* Complete Parts 1-4 before submitting your answer. NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) HCIO(aq) OH(aq) HO(1) + CIO (aq) RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040 < PREV NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HCIO(aq) + H:O(1) = HỌ (aq) CIO (aq) RESET 0.40 0.13 0.37 0.010 0.040 0.10 +x 0.13 + x 0.13-x 0.010 + x 0.010-x 0.040 + x 0.040-x 0.10+x 0.10-x 0.40+x 0.40-x
Transcribed Image Text:Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 10-* Complete Parts 1-4 before submitting your answer. NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) HCIO(aq) OH(aq) HO(1) + CIO (aq) RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040 < PREV NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HCIO(aq) + H:O(1) = HỌ (aq) CIO (aq) RESET 0.40 0.13 0.37 0.010 0.040 0.10 +x 0.13 + x 0.13-x 0.010 + x 0.010-x 0.040 + x 0.040-x 0.10+x 0.10-x 0.40+x 0.40-x
< PREV 2 NEXT > Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89
Transcribed Image Text:< PREV 2 NEXT > Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89
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