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Many household cleaning products contain oxalic acid, H2C2O4, a diprotic acid with the following dissociation constants: Ka = 5.9 × 102, Ka, = 6.4 × 10–5. Part A Calculate the equilibrium concentration of H30+ in a 0.20 mol L-1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [H30+] = 0.083 mol·L-1 Submit Previous Answers v Correct The fact that the initial acid concentration was not a thousand times bigger than the acid-dissociation constant was a clue that we would have to solve the full quadratic equation. Now that we know the value of x (0.083 mol L-1), we can verify that [H3O+] is more than 5 percent of the initial concentration, and therefore not negligible compared to 0.20 mol L-1. Part B Calculate the equilibrium concentration of C2042- in a 0.20 molL-1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) HA (C20,2-] = Value Units

Many household cleaning products contain oxalic acid, H2C2O4, a diprotic acid with the following dissociation constants: Ka = 5.9 × 102, Ka, = 6.4 × 10–5. Part A Calculate the equilibrium concentration of H30+ in a 0.20 mol L-1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [H30+] = 0.083 mol·L-1 Submit Previous Answers v Correct The fact that the initial acid concentration was not a thousand times bigger than the acid-dissociation constant was a clue that we would have to solve the full quadratic equation. Now that we know the value of x (0.083 mol L-1), we can verify that [H3O+] is more than 5 percent of the initial concentration, and therefore not negligible compared to 0.20 mol L-1. Part B Calculate the equilibrium concentration of C2042- in a 0.20 molL-1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) HA (C20,2-] = Value Units

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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I need help with part B please

Many household cleaning products contain oxalic acid, H2 C204, a diprotic acid with the following dissociation constants: Ka = 5.9 x 10-2, Ka, = 6.4 × 10-5. Part A Calculate the equilibrium concentration of H30+ in a 0.20 mol L- solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [H3O+] = = 0.083 mol·L-1 Submit Previous Answers Correct The fact that the initial acid concentration was not a thousand times bigger than the acid-dissociation constant was a clue that we would have to solve the full quadratic equation. Now that we know the value of x (0.083 mol L-), we can verify that [H3O*] is more than 5 percent of the initial concentration, and therefore not negligible compared to 0.20 mol L-. Part B Calculate the equilibrium concentration of C204- in a 0.20 molL- solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [C20,?-] = Value Units
Transcribed Image Text:Many household cleaning products contain oxalic acid, H2 C204, a diprotic acid with the following dissociation constants: Ka = 5.9 x 10-2, Ka, = 6.4 × 10-5. Part A Calculate the equilibrium concentration of H30+ in a 0.20 mol L- solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [H3O+] = = 0.083 mol·L-1 Submit Previous Answers Correct The fact that the initial acid concentration was not a thousand times bigger than the acid-dissociation constant was a clue that we would have to solve the full quadratic equation. Now that we know the value of x (0.083 mol L-), we can verify that [H3O*] is more than 5 percent of the initial concentration, and therefore not negligible compared to 0.20 mol L-. Part B Calculate the equilibrium concentration of C204- in a 0.20 molL- solution of oxalic acid. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) [C20,?-] = Value Units
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