If the concentration of ammonia of ammonium chloride in a buffer solution of ammonia-ammonium chloride are 0.2M and 0.3M respectively, determine the pH of the solution. [Given `K_(b)(NH_(3))=1.76xx10^(-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))

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)

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) .

Calculate the pH of 0.1 (N) acetic acid solution. Given: K_(a) (acetic acid) =1.8xx10^(-5)

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

The pH of 0.01 (M) acetic solution at 25^@C ( K_a=1.85xx10^-5 )

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.

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

Determine the pH of an aqueous 1.0(M) CH_(3)COOH solution. If 1L of this acid solution is diluted with distilled water, then calculate the volume of the dilute solution for a two-fold increase in the pH of the solution? [K_(a)(CH_(3)COOH)=1.8xx10^(-5)] .