Calculate the pH 0.01 (m) ch_3COOH at 25^@C`.
(Given dissociation constant of CH_3COOH = 1.75 x 10^(-5)`

Calculate the pH of 0.01 (M) CH_(3) CO OH at 25^(@) C .

Calculate the pH of 0.1(M) NH_(4)OH at 25^(@)C . The dissociation constant of NH_(4)OH at 25^(@)C is 1.76xx10^(-5) .

Calculate the pH of 0.1 (M) NH_4OH at 25^@C . The dissociation constant of NH_4OH at 25^@C . The dissociation constant of NH_4OH at 25^@C is 1.76 xx10^-5 .

(i) State law of mass action. (ii) For the reaction N_(2)+3H_(2)hArr 2NH_(3) equilibrium constant is K_(1) and that of for the reaction NH_(3)hArr (1)/(2)N_(2)+(3)/(2)H_(2) is K_(2) . Then calculate the relation between K_(1) and K_(2) . (iii) Calculate the pH of 0.01 (M) CH_(3)COOH at 25^(@)C . (K_(a)" of "CH_(3)COOH=1.75xx10^(-5)) .

Find out the heat of formation of CH_3COOH . Given that the heat of combusion of CH_3COOH is -867 KJ mol^-1 and the heat of formation of CO_2 and H_2O are - 393.5 and - 285.9 KJ mol^-1 respectively.

Write the IUPAC name of CH_3CH_2COOH .

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) .

Calculate the pH of the buffer solution containing 50 mL 0.2(M) CH_3COOH and 50mL 0.1(M) CH_3COONa solution. [pK_a(CH_3COOH) = 4.74]

The measured freezing point depression for a 0.1m aqueous CH_(3)COOH solution is 0.19""^(@)C . The acid dissociation constant K_(e) at this concentration will be (Given K_(f) , the molal cryoscopic constant = 1.86 K kg mol^(-1) )

What is the pH of the solution when 0.2 mol of HCI is added to one litre of a solution containing 1M acetic acid and acetate ions. Assume that the total volume is one litre. K_a for CH_3COOH = 1.8 × 10^(-5) .