The `pH` in a solution that is made up of `0.015M HCOOH` and `0.01M HCl` is : (Given : `K_(a)(HCOOH)=1.8times10^(-4))`
(1) `2.3`
(2) `2`
(3) `1.3`
(4) `3.3`

What is the [HCOO^-] in the solution that contains 0.015 M HCOOH and 0.02 M HCl ? K_a(HCOOH)=1.8xx10^(-4)

Calculate [H^(o+)] in a soluton that is 0.1M HCOOH and 0.1 M HOCN. K_(a)(HCOOH) = 1.8 xx 10^(-4), K_(a) (HoCN) = 3.3 xx 10^(-4) .

The pH of a buffer solution of 0.1 M CH_(3)COOH and 0.1 MCH_(3)COONa is (pK_(a)CH_(3)COOH =4.745)

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

Calcualte the pH of solution when 100 mL, 0.1 M CH_(3)COOH and 100 mL, 0.1 M HCOOH are mixed together. ("Given : "K_(a)(CH_(3)COOH)=2xx10^(-5)), K_(a)(HCOOH)=6xx10^(-5)