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)`.

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

The pH of a solution containing 0.1 M HCOOH and 0.050 M HCOONa (K_(a)= 2.0 xx 10^(-4)) is equal to

Calculate [H^+],[HCOO^(-)] and [OCN^(-)] in a solution that contains 0.1 M HCOOH (K_a=2.4xx10^(-4)) and 0.1 M HOCN (K_a=4xx10^(-4)) .

Calculate [H^+],[HCOO^(-)] and [OCN^(-)] in a solution that contains 0.1 M HCOOH (K_a=2.4xx10^(-4)) and 0.1 M HOCN (K_a=4xx10^(-4)) .

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )