If the concentration of ammonia and ammonium chloride in buffer solution of ammonia - ammonium chloride are 0.2 M and 0.3M respectively, deteimine the pH of the buffer solution. `
` (Given `K_b``(NH_3)` = 1.76 x `10^(-5)`

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))

In a buffer solution containing equal concentration of B^- and HB, the K_b for B^- is 10^(-10) . The pH of buffer solution is

Concentrations of CH_3COOH in the two aqueous solutions, A and B, are 10^(-2) (M) and 10^(-4) (M) respectively. Show that, the difference in pH values of the two solutions is one unit.

A certain buffer solution contains equal concentration of X^- and HX. Calculate pH of buffer solution.( k_b for X^- is 10^-9 )

The product of molar concentrations of hydrogen ions and hydroxide ions in a 0.01 M aqueous solution of sodium chloride is known as

Find the pH of ann ammonia-ammonium chloride buffer solution in which [NH_(3)]=0.2(M) and [NH_(4)^(+)]=0.3(M) . Given K_(b)(NH_(3))=1.76xx10^(-5) .

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

The pH of a buffer solution obtained by the combination of a weak base (B) and its conjugate acid (BH^+) is 9. If the concentrations of B and BH^+ in the buffer are 0.2(M) and 0.02(M) respectively, then find the ionisation constant of the weak base.