6. a. Compute or show the value [H^+] Or [H3O^+] in a 0.034 M nitric acid soluti

Question

6. a. Compute or show the value [H^+] Or [H3O^+] in a 0.034 M nitric acid solution. b. Correctly finish the chemical equation for the equilibrium dissociation or autoionization of H2O(I) (Part 1). Then write the algebraic expression (in terms of concentrations)for the equilibrium constant for this process (Part 2). (1) equilibrium chemical equation: (2) H2O(I) (2) equilibrium constant expression or formula KW = c. Then use the value of KW (= 1.0 x 10^-14) to compute the value of [OH^-] the hydroxide ion concentration in this 0.034 M nitric acid solution.

Explanation / Answer

6.

a) HNO3 = 0.034 M

As HNO3 has one proton in it,

[H^+] = [H3O^+] = 0.034 M

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b)

1) 2H2O(l) <-------------> H3O^+(aq) + OH^-(aq)

2) Kw = [H3O^+][OH^-]

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c)

Kw = [H3O^+][OH^-]

[H3O^+] = 0.034 M

[OH^-] = (1.0 x 10^-14) / 0.034

[OH^-] = 2.94 x 10^-13 M

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