Find the amount of `(NH_(4))_(2)SO_(4)` required to be added to 500 mL 0.2 (M) `NH_(3)` to prepare a buffer solution of `pH=9.35.` [Given: `K_(b)(NH_(3))=1.78xx10^(-5)`].

Calculate the amount of (NH_4)^2SO_4 in g which must be added to 500 mL of 0.2 MNH_3 to yield a solution of pH=9.35, K_b for NH_3 = 1.78xx10^-5

An aqueous solution of (NH_(4))_(2)SO_(4) is acidic. Explain.

Calculate the amount of HCOONa that is to be added to 0.05 (M) 1 L HCOOH to make the overall pH of the solution 4.00 (Given : K_(a) of HCOOH = 2.4 xx 10^(-4) ).

100 mL of a buffer solution (pH=9.5) is to be prepared using 0.3(M) NH_(3) and 0.1(M) HCl solution. What are the volumes (in mL) of NH_(3) and HCl required to prepare this buffer solution? Given: pK_(b)(NH_(3))=4.74 .

What happens when a mixture of (NH_(4))_(2)SO_(4) and NaNO_(3) is heated ?

The ratio of volumes of 0.1(N) CH_3COOH to 0.1(N) CH_3COONa required to prepare a buffer solution of pH 5.74 is (given : pK_a of CH_3COOH is 4.74_-

The ratio of volumes of CH_3COOH 0.1 (N) to CH_3COONa 0.1 (N) required to prepare a buffer solution of pH5.74 is (given: pKa of CH_3COOH is 4.74)

If the concentration of ammonia and ammonium chloride in a buffer solution of ammonia-ammonium chloride are 0.2 M and 0.3 M respectively , determine the pH of the buffer solution. (Given : K_(p) (NH_(3)) = 1.76 xx 10^(-5))

Determine the pH of a buffer solution consisting of 0.01(M) CH_(3)COOH and 0.03(M)" "CH_(3)COONa. Given: K_(a)(CH_(3)COOH)=1.8xx10^(-5) .

The pH of 0.02 M solution of ammonium chloride at 25^@C is [ k_b(NH_3)=1.8xx10^-5]