What is the `[H^+]` in a solution in which `[HA]=4.0xx10^(-2)` and `[A^-]=2.0xx10^(-2)` ? `[K_a=3.0xx10^(-6)]`

Calculate the concentrations of all the species present in 0.1 M H_3PO_4 solution. Given : K_1=7.5xx10^(-3), K_2=6.2xx10^(-8) and K_3=3.6xx10^(-13) .

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 ]

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 beer has a pH of 4.30. What is the [H_(3)O^(+)] ? (a) 3.0xx10^(-4) (b) 2.0xx10^(-4) (c) 2.0xx10^(5) (d) 5.0xx10^(-5)

10xx10^(3)*2.2xx10^(-6)*(10)/(0.4)

An aqueous solution contains 0.10 MH_2 S and 0.20 M HCl if the equilibrium constants for the formation of HS^(-) " from " H_2S " is " 1.0 xx 10^(-7) and " that of " S^(2-) " from " HS^(-) ions is 1.2 xx 10 ^(-13) then the concentration of S^(2-) ions in aqueous solution is 5 xx 10 ^(-8) 3 xx 10 ^(-20) 6 xx 10 ^(-21) 5 xx 10 ^(-19)

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)) .