What is the `pH` of `0.01 M` glycine solution? For glycine, `K_(a_(1))=4.5xx10^(-3)` and `K_(a_(2))=1.7xx10^(-10)` at `298 K`

A solution contains 0.1MH_(2) and 0.3MHCl. Calculate the concentration of S^(2) and HS- ions in the solution. For H_(2)S, K_(a_(1))=1.05xx10^(-7) and K_(a_(2))=1.3xx10^(-14) .

What is the pH of 10^(-3) M ammonia cyanide solution, if K_(HCN)=7.2 xx 10^(-11) and K_(NH_(3))=1.8 xx 10^(-5)mol L^(-1) ?

The pH of a 0.1 M solution of NH_(4)OH (having K_(b)=1.0xx10^(-5)) is equal to

Calculate the pH of 0.010M NaHCO_(3) solution. K_(1)=4.5xx10^(-7) , K_(2)= 4.7xx10^(-11) for carbonic acid.

Calculate the pH of a 0.01 M solution of benzoic acid, the K_a being 7.3xx10^(-5)

The pH of 0.01 (M) acetic solution at 25^@C ( K_a=1.85xx10^-5 )