At `25 C`,in pure water (or) in neutral aqueous solutions,`H^(+)=1*10^(-x)` mole /Lt.The value of `x` is

Why is pure water neutral although it contains H_3O^(+) ions?

The percentage of dissociation of CH_(3)NH_(2) , in an aqueous solution with [H^(+)] = 10^(-10) M in 0.1M concentration is'x'. The value of 10x is _________ ?

In 1L saturated solution of AgCl[K_(SP)(AgCl)= 1.6xx10^(-10)], 0.1 mole of CuCI [K_(SP)(CuCl)=1.0xx10^(-6)] is added. The resulrant concentration of Ag^(+) in the solution is 1.6xx10^(-x) . The value of "x" is:

At 80 ^(@ ) C , pure distilled water has [H_3O^(+) ]= 1 xx 10 ^(-6) " mol " L^(-1) The value of K_w at this temperature will be

Find the mole fraction of solute in its 10 molal aqueous solution.

At 90^(@)C , pure water has [H_(3)O^(o+)] = 10^(-7)mol L^(-1) . What is the value of K_(w) at 90^(@)C ?

The mole fraction of water in 20% (wt.//wt.) aqueous solution of H_(2)O_(2) is:

MnO_(4)^(2-) ( 1 mole) in neutral aqueous medium is disproportionate to

At 90^(@)C pure water has [H_(3)O^(+)] as 10^(-6) mol L^(-1) . What is the value of K_(w) at 90^(@)C ?

Percent by mass of solute (molar mass = 25 g/mol) in its aqueous solution is 30. The mole fraction and molality of the solute in solution are