17. For a solution that is found to have [OH ] = 2.50 × 10 8 M, determine the mo

Question

17. For a solution that is found to have [OH] = 2.50 × 108 M, determine the molarity of H3O+ and whether the solution would be acidic, basic or neutral.

            A) [H3O+] = 2.50 × 1022 and the solution would be basic

            B) [H3O+] = 2.50 × 1022 and the solution would be acidic

            C) [H3O+] = 4.00 × 107 and the solution would be basic

            D) [H3O+] = 4.00 × 107 and the solution would be acidic

            E) [H3O+] = 4.00 × 1023 and the solution would be basic

D is the answer but I need help understanding how to get that answer and how to judge if its acidic.

Explanation / Answer

[OH] = 2.50 × 108 M

[H3O+] [OH-] = Kw

[H3O+] [2.50 × 108] = 1.0 x 10^-14

[H3O+] = 4.00 x 10^-7 M

the solution would be acidic .

if [H3O+] concentration > 10^-7 , that is acidic .

if [H3O+] concentration < 10^-7 , that is basic

if if [H3O+] concentration = 10^-7 , that is neutral

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