State two chemical properties each with equations of a solution containing (i) `H^(+)` ions (ii) `OH^(-)` ions.

An aqueous solution containing S^(-2) ions will not give

An aqueous solution containing S^(2-) ions will not give:

One litre of a strong acid solution contains 10^(-5) moles of H^(+) ions.Then:

A solution of NaOH possesses both H_3O^(+) and OH^(-) ions.

The pH of a solution at 25°C that contains 10^(-10) M hydroxide ions (OH^-) is

Calculate pH at which Mg(OH)_(2) begins to precipitate from a solution containing 0.10M Mg^(2+) ions. (K_(SP)of Mg(OH)_(2)=1xx10^(-11))

Define pH value. What would you say about the pH of a solution in which (i) H^(+) aq. Ions= OH^(-) ions (ii) evolves CO_(2) when heated with Na_(2)CO_(3) (iii) OH^(-) ions gt H^(+) aq ions

On the addition of a solution containing CrO_(4)^(2-) ions to the solution of Ba^(2+), Sr^(2+) and Ca^(2+) ions, the precipitate obtained first will be of:

A solutions containing NaOH and NaCl shows common ion effect.

MnO_(4)^(-) ions are reduced in acidic conditions to Mn^(2+) ions whereas they are reduced in neutral condition to MnO_(2) . The oxidation of 25 mL of a solution x containing Fe^(2+) ions required in acidic condition 20 mL of a solution y containing MnO_(4) ions. What value of solution y would be required to oxidize 25 mL of solution x containing Fe^(2+) ions in neutral condition ?