A buffer of pH 9.26 is made by dissolving x moles of ammonium sulphate and 0.1 mole of ammonia into 100 mL solution. If `pK_b` of ammonia is 4.74, calculate value of x.

A buffer solution contains 2 moles of ammonium hydroxide and 0.25 mole of ammonium chloride per dm^(3) of the solution. ( K_(b) for ammonium hydroxide = 1.8xx10^(-5) ). Calculate the pH of the buffer solution.

pH of when 50mL of 0.10 M ammonia solution is treated with 50 mL of 0.05 M HCI solution :- (pK_(b) "of ammonia"=4.74)

pH of when 50mL of 0.10 M ammonia solution is treated with 50 mL of 0.05 M HCI solution :- (pK_(b) "of ammonia"=4.74)

One litre of a buffer solution is prepared by dissolving 0.6 mole. of NH_3 and 0.4 mole of NH_4CI . What is the pH of the solution ? For NH_3K_b = 1.8 xx 10^(-5) . What is the pH of the buffer after addition of 0.1 mole of NaOH ?

One litre of a buffer solution is prepared by dissolving 0.6 mole. of NH_3 and 0.4 mole of NH_4CI . What is the pH of the solution ? For NH_3K_b = 1.8 xx 10^(-5) . What is the pH of the buffer after addition of 0.1 mole of of HCI ?

The pH of a solution obtained by dissolving 0.025 mole of an acid (HA) in 250 ml of the aqueous solution was found to be 4.0. Calculate the dissociation constant of HA.

Calculate the pH of a 0.1 M aqueous ammonium cyanide solution. Given pK_a =9.02 and pK_b =4.76

In a basic buffer, 0.0025 mole of 'NH_4 Cl' and 0.15 mole of NH_4OH are present. The pH of the solution will be (pK_a)=4.74