[" Q.9An aqueous solution contains "0.01MRNH_(2)(K_(b)=2times10^(-6))&10^(-4)MNaOH" .The concentration of "],[OH^(-)" is nearly: "]

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)

The pH of an aqueous solution of Ba(OH)_(2) is 10 . If the K_(sp) of Ba(OH)_(2) is 1xx10^(-9) , then the concentration of Ba^(2+) ions in the solution in mol L^(-1) is

The pH of an aqueous solution of Ba(OH)_(2) is 10 . If the K_(sp) of Ba(OH)_(2) is 1xx10^(-9) , then the concentration of Ba^(2+) ions in the solution in mol L^(-1) is

The pH an aqueous solution of Ba(OH)_(2) is 10.0 . If the K_(sp) of Ba(OH)_(2) is 1.0xx10^(-9) , the concetration of Ba^(2+) ions in the solution is

The P^(H) of saturated aqueous solution of Ba(OH)_(2) is 10 . If the K_(sp) of Ba(OH)_(2) is 5 xx 10^(13) , then the concentration of Ba^(2+) ions in the solution is

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 If solution contains only 0.1 M H_(2)CO_(3) then the concentration of CO_(3)^(2-) at equilibrium in the solution will be :