Answer asap need by wednesday morning calculate the ph of 0.16m ch3cooh which has ka = 1.74 x 10-5 mol dm-3 best answer will be brainliest

5.555.

Explanation:

∵ pH = - log[H⁺],

[H⁺] for weak acids = √Ka.C.

Ka for CH₃COOH = 1.74 x 10⁻⁵, C = 0.16 M.

∴ [H⁺] = √Ka.C = √(1.74 x 10⁻⁵)(0.16 M) = 2.784 x 10⁻⁶ M.

∴ pH = - log[H⁺] = - log(2.784 x 10⁻⁶ M) = 5.555.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.