2.5 mL of `(2)/(5)M` weak monoacidic base `(K_(b)=1xx10^(-12)` at `25^(@)C)` is titrated with `(2)/(15)`M HCl in water at `25^(@)C`. Calculate the concentration of `H^(+)` at equilibrium point. `(k_(w)=1xx10^(-14))`

2.5 ml 0.4 (M) weak monoacidic base ( k_b=1 xx 10^(-12) at 25^@ C ) is titrated with 2/15(M) HCl in water at 25^@C . The concentration of H^+ at equivalence point is ( K_w=1xx10^(-14) , at 25^@C )

Calculate the concentration of OH^_ ions of 0.01 M NH_4OH : K_b = 1.58 xx 10^(-5)

The concentration of an aqueous solution of the weak acid, HA is 0.1(M). Calculate the pH and concentrations of A^- ion and HA at equilibrium in the solution. Given: K_b(HA)=1.35xx10^(-3)

At 25^(@)C what is the concentration of H_(3)O^(+) ions in an aqueous solution in which the concentration of OH^(-) ions is 2xx10^(-5)(M) ?

if K_(sp)(CaF_2)=4xx10^(-11) at 25^(@) C then find the molar solubility of CaF_2 in pure water

The volume of the water needed to dissolve 1g of BaSO_4 (K_(sp)=1.1xx10^-10 ) at 25^@C is

Determine the pH of an aqueous solution of ammonia if the concentration of the solution is 3(M). K_(b) (ammonia) =1.8xx10^(-5) .

For the equilibrium 2SO_(3(g))hArrSO_(2(g))+O_(2(g)) , the value of equilibrium constant is 4.8xx10^(-3) at 700^(@)C . At equilibrium, if the concentration of SO_(3) and SO_(2) are 0.60M and 0.15M respectively. Calculate the concentration of O_(2) in the equillibrium mixture.

The value of K_(c) for the reaction 3O_(2)(g)hArr 2O_(3)(g) is 2.0xx10^(-50) at 25^(@)C . If the equilibrium concentration of O_(2) in air at 25^(@)C is 1.6xx10^(-2) , what is the concentration of O_(3) ?

Calculate the osmotic pressure when 2.5xx10^(-2) gm K_2SO_4 is added in 2L water at 25^@C (Consider complete dissociation of K_2SO_4 )