Ostwald Dilution Law

The strength of elctrolytes is expressed in terms of degree of dissociation alpha For strong electrolyte alpha is close to one and for weak electrolytes alpha is quite small. According to Ostwald Dilution Law alpha=sqrt((K)/(C)) For an acid [H^(+)] = sqrt(K_(a)C) For a base [OH^(-)] =sqrt(K_(b)C The relative strengths of acids or bases can be compared in terms of the square roots of their K_(a) " or " K_(b) values. A monoprotic acid in 0.1 M solution ionises to 0.001 % . Its ionisation constant is :

Ionic Equilibrium - Ostwald'S Dilution Law

Arrhenius Theory OF Electrolytic Dissociation|| Ostwald's Dilution Law

Classification OF Substance (Electrolyte and Non - electrolyte) || Arrhenius Theory OF Electrolytic Dissociation || Strong and Weak Electrolyte || Ostwald’s Dilution Law || Factors Affecting Degree OF Dissociation

The dissociation of weak electrolyte (a weak base or weak acid) id expressed in terms of Ostwald dilution law. An acid is a substance which furnishes a proton or accepts an electron pair whereas a base is proton acceptor or electron pair donor. Storonger is the acid weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base are related by (K_(w)=K_(a)xxK_(b) , where K_(w) is ionic prodcut of water equal to 10-14 at 25^(@) C. The numerical value of K_(w) however increases 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 solutions are the solutions which do not show appreciable change in the pH on addition of small amount of acid or base. Which of the following solution is most important buffer for human living?

The dissociation of weak electrolyte (a weak base or weak acid) id expressed in terms of Ostwald dilution law. An acid is a substance which furnishes a proton or accepts an electron pair whereas a base is proton acceptor or electron pair donor. Storonger is the acid weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base are related by (K_(w)=K_(a)xxK_(b) , where K_(w) is ionic prodcut of water equal to 10-14 at 25^(@) C. The numerical value of K_(w) however increases 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 solutions 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 :

The dissociation of weak electrolyte (a weak base or weak acid) id expressed in terms of Ostwald dilution law. An acid is a substance which furnishes a proton or accepts an electron pair whereas a base is proton acceptor or electron pair donor. Storonger is the acid weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base are related by (K_(w)=K_(a)xxK_(b) , where K_(w) is ionic prodcut of water equal to 10-14 at 25^(@)C . The numerical value of K_(w) however increases 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 solutions are the solutions which do not show appreciable change in the pH on addition of small amount of acid or base. Which of the following statements are correct? (P) At 25^(@)C,pH of 10^(-10)MNaOH is nearly 7. (Q) The degree of dissociation of a weak acid is given by (1)/(1+10^((pk_(a)-pH))) . (R) For weak electrolytes of polyprotic acid nature having no other electrolyte, the anion concentration produced in II step of dissocitation is always equal to K_(2) at reasonable concentration of acid. (S) The concentraion of amide ions produced during self ionisation of NH_(3) is equal to concentration of ammonium ions. Ostwld dilution law is valid for strong electrolytes.