Need help w / henderson-hasselbalch. Please?

How many moles NaF strength must increase. 1.0 L of 1.90 M HF solution to meet your buffer. pH 3.35 or assume any volume changes. (Ka for HF = 7.2 x 10 ^ -4 A.) 3.1 B. 2.3 C. 1.6 D. 1 E. 4.9 I think the answer will be lower. 1.9 So how do C or D, but actually I'm not sure my logic right. Please help.

Begin with. Henderson-pH equations Hasselbach = pKa + log ([⁻] / [HA]) for weak acid. [HA] is equal to the amount of acid and dissolved. [⁻] Equal to the amount caused by the separation of salt. From the equation above, you can come. Volume ratio: log ([⁻] / [HA]). pH = pKa - <=> [⁻] / [HA] = 10 ^ (pH - pKa) than if the pKa pH, salt concentration of smaller concentrations of acid and vice versa. For this problem, pKa =- log (Ka) =- log (7.2 x 10 ^ -4) = 3.14, so you'll need more. 1.9moles salt per liter. The exact value of the salt concentration is required:. F [⁻] = [HF] · 10 ^ (3.35-3.14) = 3.1 mol / L is the correct answer.

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