Calculate the percentage hydrolysis & the `pH` of `0.02M CH_(3)COONH_4`.
`K_(b)(NH_(3))-1.6xx10^(-5),K_(a)(CH_(3)COOH)=1.6xx10^(-5)`

Calculate the degree of hydrolysis and pH of 0.2M solution of NH_(4)C1 Given K_(b) for NH_(4)OH is 1.8 xx 10^(-5) .

Calculate the percent hydrolysis of acetic acid in a solution 2.3 M in CH_(3)COOH and 0. 1 in HCl . K_(a) = 1.8 xx10^(-5)

Calculate the pH of a solution obtained by mixing equal volume of 0.02MHOCl &0.2MCH_(3)COOH solutions Given that K_(a)(HOCl)=2xx10^(-4),K_(a)(CH_(3)COOH)=2xx10^(-5) Also calculate [OH^(-)],[OCl^(-)],[CH_(3)COOH] at equilibrium .Take log2=0.3

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

Calculate the e.m.f. of the cell Pt|H_(2)(1.0atm)|CH_(3)COOH (0.1M)||NH_(3)(aq,0.01M)|H_(2)(1.0atm)|Pt K_(a) (CH_(3)COOH) =1.8 xx 10^(-5), K_(b),(NH_(3)) = 1.8 xx 10^(-5)

Total number of solutions from the following which has pHlt7 at 25^(@)C . (K_(a)(CH_(3)COOH)=1.8xx10^(-5),K_(b)(NH_(4)OH)=1.8xx10^(-5)) (i) 10^(-8) MHCl (ii) 0.01 M solution of NH_(4)Cl (iii) 0.01 M solution of CH_(3)COONa (iv) 0.01M solution is B(OH)_(3) (v) 0.01M solution of CH_(3)COONH_(4)

Calculate the pH at the equivalence point during the titration of 0.1M, 25 mL CH_(3)COOH with 0.05M NaOH solution. [K_(a)(CH_(3)COOH) = 1.8 xx 10^(-5)]

Calculate the pH at the equivalence point during the titration of 0.1M, 25 mL CH_(3)COOH with 0.05M NaOH solution. [K_(a)(CH_(3)COOH) = 1.8 xx 10^(-5)]

What is the concentration of CH_(3)COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1 L H_(2)O ? [K_(a) (CH_(3)COOH))=1.8xx10^(-5)),K_(b) (NH_(4)OH)=1.8xx10^(-5))]

Calculate the percentage hydrolysis of decinormal solution of ammonium acetate given that k_(a) = 1.75 xx 10^(-5), K_(b) =1.80 xx 10^(-5) and K_(w) = 1.0 xx 10^(-14)