What is the hydroxide ion concentration, [OH^-], in an aqueous solution where th

Question

What is the hydroxide ion concentration, [OH^-], in an aqueous solution where the hydronium ion concentration, [H_3O^+], equals 4.82 times 10^-8 M: [H_3O^+] = 4.82 times 10^-8 M? 4.76 times 10^-4 M 2.07 times 10^-7 M 3.35 times 10^-3 M 6.62 times 10^-13 M 0.0711 M What is the hydronium ion concentration, [H_3O^+], in an aqueous solution where the hydroxide ion concentration, [OH^-], equals 0.525 M: [OH^-] = 0.525 M? {[H_3O^+] [OH^-] = 1.0 times 10^-14} 1.65 times 10^-13 M 7.05 times 10^-11 M 1.90 times 10^-14 M 0.875 M 1.13 M What is the pH of a solution where the hydronium ion concentration, [H_3O^+], equals 4.71 times 10^-3 M, [H_3O^+] = 4.71 times 10^-3 M? (pH = - log [H_3O^+]) 2.33 12.9 5.22 8.19 13.3 What is the pH of a solution w here the hydroxide ion concentration, [OH^-], equals 3.97 times 10^-6 M: [OH^-] = 3.97 times 10^-6 M? (pH = - log [H_3O^+]) 7.86 4.12 6.11 8.59 3.65 What is the pH of a solution where the hydroxide ion concentration, [OH^-], equals 0.775 M: [OH^-] = 0.775 M? (pH = - log [H_3O^+]) 4.11

Explanation / Answer

P.6) Solution:

Given data:

[H3O+] = 4.82 * 10-8

We have,

[H3O+][OH-] = 1 * 10-14

[OH-] = 1 * 10-14/4.82 * 10-8

= 0.207 * 10-6

= 2.07 * 10-7 M

Answer is B

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