An aqueous solution contains 0.01 M `RNH_2 (K_b=2 xx 10^(-6)) & 10^(-4) M NaOH.` The concentration of `OH^(-)` is nearly:

Successive dissociation constants of H_(2)CO_(3) are K_(a_(1)) = 10^(-3) and K_(a_(2)) = 10^(-6) . An aqueous solution contains 0.1 MH_(2)CO_(3) and 0.1 M HCI at 25^(@)C The concentration of CO_(3)^(2-) at equilibrium in solution is: (approximately)

Mg(OH)_(2) is precipitated when NaOH is added to a solution of Mg^(2+) . If the final concentration of Mg^(2+) is 10^(-10) .M, the concetration of OH^(-) (M) is the solution is b [Solubility product for Mg(OH)_(2)=5.6xx10^(-12) ]

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)) .

At 25^@ C , the dissociation constant of NH_4 OH is 2 xx 10^(-5) . If the molar concentration of NH_2 OH is 0.2 M , calculate the proton concentration of aqueous ammonia solution.

Calculate the pH of 0.1 M NH_4 OH if K_b =1.75 xx10^(-5) .

An acidic aqueous solution contains 0.02M - FeCI_(2) and 0.05 M -FeCI_(3) , at 25^(@)C . Now NaOH solution is added is this solution, drop bydrop. The pH range in which only the precipitation of Fe(OH) (s) occur without precipitation of Fe(OH)_(2)(s) differs by 'x' unit. The value of 'x' is given : K_(sp) of Fe(OH)_(2) = 8 xx 10^(-16) K_(sp) of Fe (OH)_(3) = 4 xx 10^(-28)