An aqueous solution of `0.01 M CH_(3) COOH` has van't Hoff factor `1.01` . If `pH = - "log"[H^(+)]`, pH of `0.01` M `CH_(3)COOH` solution would be :

An aqueous solution of 0.01 M CH_3COOH has Van't Hoff factor 1.01. If pH=-log [H^+] , pH of 0.01 M CH_3COOH solution would be

Calculate pH solution: 0.1 M CH_(3)COOH (K_a=1.8 xx 10^(-5))

pK_(a) of CH_(3)COOH is 4.74 . The pH of 0.01 M CH_(3)COONa IS

Why is the molar conductivity of a 0.01 M HCl solution greater than that of a 0.01 M CH_(3)COOH solution?

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

The pH of 0.1 M solution of CH_(3)COOH if it ionizes to an extent of 1% is .