sum of `H^(+)` and `OH^(-1)` ions concentration in pure water at `90^(o)`C pkw=12

Specific conductance of pure water at 25^(@)C is 0.58 xx 10^(-7) mho cm^(-1) . Calculate ionic product of wter (K_(w)) if ionic conductances of H^(+) and OH^(-) ions at infinite are 350 and 198 mho cm^(2) respectively at 25^(@)C

If a solution has of a pOH value of 14 at 25^(@)C , H^(+) ion concentration in mol L^(-1) should be

The no.of H_(3)O^(+) ions present in 10 ml of water at 25^(@) C is

The phenomenon of interaction of anions and cations furnished by a electrolyte with the H^(+) and OH^(-) ions of water to produce acidity or alkalinity is known as hydrolysis. In hydrolysis :

At 25^(@)C,4.0g of NaOH are dissolced in eater to produce soluton of volume 1 litre .Find (i) molarity of the solution (II) OH^(-) ion concentration (II) pH value of the solution. At masses (in u) , Na=23,O=16,H=1 )

At a certain temperature the hydronium ion concentration in pure water is found to be 1.7 xx 10 ^(-7) " mol " L^(-1) .What is the value of K_w at this temperature ?

The ionic product of water is 10^(-14) , The H^(+) ion concentration in 0.1 M NaOH solution is

The K_(sp) value of CaCO_(3) and CaC_(2)O_(4) in water are 4.7 xx 10^(-9) and 1.3 xx 10^(-9) , respectively, at 25^(@)C . If a mixture of two is washed with H_(2)O , what is Ca^(2+) ion concentration in water?

If H_(3)O^(+) ion concentration of a solution is increased by 10 times , its pH will

The H ion concentration of a solution is 4.75 xx 10^(-5) M. Then the OH ion concentration of the same solution is