Let `K_(w)` at `100^(@)C` be `5.5xx10^(-13) M^(2)`. If an aqueous solution at this temperature has `pH=6.2`. Its nature will be

At 20^@C water has K_w=6.807xx10^(-15) .What is the pH of pure water at this temperature ?

The value of the ion product constant for water, (K_(w)) at 60^(@) C is 9.6xx10^(-14) M^(2) what is the [H_(3)O^(+)] of a neutral aqueous solutoin at 60^(@) C and an aqueous solution with a pH=7.0 at 60 ^(@) C are respectively?

The value of the ion product constant for water, (K_(w)) at 60^(@) C is 9.6xx10^(-14) M^(2) what is the [H_(3)O^(+)] of a neutral aqueous solutoin at 60^(@) C and an aqueous solution with a pH=7.0 at 60 ^(@) C are respectively?

The value of the ion product constant for water, (K_(w)) at 60^(@) C is 9.6xx10^(-14) M^(2) what is the [H_(3)O^(+)] of a neutral aqueous solutoin at 60^(@) C and an aqueous solution with a pH=7.0 at 60 ^(@) C are respectively?

At 900^(@)C , pK_(w) is 13. At this temperature an aqueous solution with pH =7 will be

At 900^(@)C , pK_(w) is 13. At this temperature an aqueous solution with pH =7 will be

The value of K_w in neutral solution is 5.474 xx 10 ^(-14) " at " 50 ^(@) C . Calculate the pH of the solution at this temperature.

The pH of 2.5xx10^(-1) M HCN solution (K_(a)=4xx10^(-10)) is :

At 90^(@)C pure water has K_(w) = 10^(-12) . The solution with pH value 6.5 is