Calculate the `[CH_(2)FCOOH]` (fluoroacetic acid) which is required to get `[H^(o+)] = 1.5 xx 10^(-3)M. K_(a)` of acid `=2.6 xx 10^(-3)`.

What concentration of dichloroacetic acid gives [H^(+)]=8.5xx10^(-3)M ? ("Given": K_(a)"of acid" = 5.0xx10^(-2)) .

The concentration of fluroacetic acid (K_(a)of acid =2.6xx10^(-3)) , which is required to get [H^(+)]=1.50xx10^(-3)M is:

Calculate the pH at which an acid indicator with K_(a) = 1.0 xx 10^(-5) changes colour when the indicator is 1.00 xx 10^(-3)M .

Glycine [NH_(2)CH_(2)COOH) is basic and acidic due to presence of -NH_(2) and -COOH group. It acquires a H^(o+) to form overset(o+)NH_(3)COOH , which is a diprotic acid with K_(1) = 4.5 5 10^(-3) and K_(2) = 1.7 xx 10^(-10) . In a 0.01M solution of neutral glycine, a. What is the pH and b. What percent of the glycine is in the cationic form at equilibrium?

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) .

Citric acid (H_(3)A) is a polyprotic acid with K_(1),K_(2) , and K_(3) equals to 7.4 xx 10^(-4), 1.7 xx 10^(-5) , and 4.0 xx 10^(-7) , respectively. Calculate the [H^(o+)], [H_(2)A^(Theta)], [HA^(2-)] , and [A^(3-)] in 0.01M citric acid.