CALCULATION OF PH AND CONCENTRATION OF [H+] OR [OH-]

A solution of 0.01M concentration of NH_(4)OH is 2.6% dissociated. Calculate [H^(+)], [OH^(-)],[NH_(4)^(+)], [NH_(4)OH] and pH of solution.

At 298 K, the pH of a lemon juice is 2.32. Calculate its [H_(3)O^(+)]" and "[OH^(-)].

pH is the negative logarithm of H^(+) pH=log[H^(+)] HCllt H^(+)+Cl^(-) H_(2)OhArrH^(+)+OH^(-) K_(W)=[H^(+)][OH^(-)] K_(W) depend on the temperatue. With rise in temperature K_(W) increases. At 298 K, pH of pure water = 7 At 373 K, pH of the pure water is

pH is the negative logarithm of H^(+) pH=log[H^(+)] HCllt H^(+)+Cl^(-) H_(2)OhArrH^(+)+OH^(-) K_(W)=[H^(+)][OH^(-)] K_(W) depend on the temperatue. With rise in temperature K_(W) increases. At 298 K, pH of pure water = 7 The exact concentration of H^(+) in 10^(-6) M HCl given by

A solution of an acid has pH= 4.70 . Find out the concentration of OH^(-) ions (pK_(w)=14) .

Calculate the [H^(o+)] and [overset(Theta)OH] of 0.0315g of HNO_(3) in 500 mL of water. Calculate pH and pOH also.

The Ph OF NEUTRAL WATER AT 25^(@)C is 7.0. As the temperature increases, ionisation of water increases, however the concentration of H^(+) ions nad OH^(-) ions equal. What will be the ph of puire water at 60^(@)C ?