SALTS OF WEAK ACID AND WEAK BASES

Hydrolysis OF Salt OF Strong Acid Weak Base || Hydrolysis OF Salt OF Weak Acid Strong Base || Hydrolysis OF Salt OF Weak Acid Weak Base

Salts Of Weak Acids And Strong Bases

Salts Of Strong Acids And Weak Bases

Estimation of pH OF Weak Acid-Weak Base

Acids|Concentrated And Diluted Acids|Strong Acids And Weak Acids|Diluting The Acids|Bases And Strong Bases & Weak Bases

Match Column -I with Column -II : Column -I Column-II (A) Ph of water ( p ) ( 1)/( 2) p K_(w) ( B ) Ph of a salt of strong acid and strong base ( q) pH = (1)/(2) [ pK_(w) + pK_(a) + log c ] (C ) Ph of a salt of weak acid and strong base ( r ) pH = ( 1)/( 2) [ pK _(w) + pK_(a) - pK_(b)] (D) Ph of a salt of weak acid and weak base (s) 7 where K_(a) , K_(b) are dissociation constants of weak acid and weak base and K_(w) = Ionic product of water.

Number of statement(s) that is/are correct : (a) On increasing temperature, pH of pure water decreases On increasing temperature, pOH of pure water decreases (c) On increasing dilution, dissociation of weak electrolyte increases (d) pH of 10^(-7) M NaOH (aq) is 7 at 25^(@)C . (e) At equivalence point (during titration of acid ad base) solution must be neutral. (f) Generally, pH of buffer solution does not change on dilution. (g) pH of salt of weak acid and weak base depends on concentration of salt.

pH of a solution of salt of weak acid and weak base is : pH=1/2pK_w+1/2pK_a-1/2pK_b and that of weak acid and strong base is pH=1/2pK_w+1/2pK_a+1/2logc pH of 0.1 M solution of ammonium cyanide ( pK_a =9.02 and pK_b =4.76 ) is