" At "25^(@)C" ,if the pHof a solution is "4" o ben its port would be "(k_(n)=10^(-14))

When 2.5 mL of 2//5M weak monoacidic base (K_(b) = 1 xx 10^(-12) at 25^(@)C) is titrated with 2//15 M HCI in water at 25^(@)C the concentration of H^(o+) at equivalence point is (K_(w) = 1 xx 10^(-14) at 25^(@)C)

For a (N)/(10) solution of KMnO_4 , its molarity will be:

25.Which of the following statement(s) is/are correct about the ionic product of water? A) K_(i) "(ionization constant of water) " B) pK_(i) > pK_(W) C) At 25^(@)C , K_(i) = 1.8times10^(-14) D) lonic product of water at 10^(@)C is 10^(-14)

The dissociation of weak electrolyte (a weak base or weak acid) is expressed in terms of Ostwald's dilution law. An acid is substance which furnishes a proton or accepts an electron pair, where a base is proton acceptor or electron pair donor. Stronger is acid, weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base (K_(b)) are related by K_(w)=K_(a)xxK_(b) , where K_(w) is ionic product of water equal to 10^(-14) at 25^(@)C . The numerical value of K_(w) however increase with temperature. In a solution of an acid or base [H^(+)][OH^(-)]=10^(-14) . Thus the [H^(+)] in a solution is expressed as: [H^(+)]=10^(-pH) and pH+pOH=14 . Buffer solution are the solutions which do not show appreciable change in the pH on addition of small amount of acid or base. The pK_(a) value of NH_(4)^(+) is 9. The pK_(b) value of NH_(4)OH would be: