Properties OF Water (Ionic Product,Ionisation Constant,Degree OF Dissociation,Molality etc.) || Types OF Solution (Acidic,Basic,Neutral) || PH Scale || Solved Numerical Class illustration

Titration and Types OF Titration,Acid Base Titration||Solved Numerical Class illustration

Basic Buffer || pH Determination Formula || Buffer Action OF Acidic Buffer || Solved Numerical Class illustration and Buffer Capacity

Class Illustration on Ionic Product OF Water||pH Calculation OF Different Types OF Solution||Acidic Solution||Strong Acid is dissolved in water

Ionization Constant Of Water And Its Ionic Product And Ph Scale

Solubility Product Case I :- Solubility in Pure Water for AB,AB2/A2B,AB3/A3B,A2B3/A3B2,AXBY,AXBYCZ type OF Salt || Solved Numerical Class illustration

Common Ion Effect||Properties OF Water||Ionic Product OF Water|| pH Scale||pH Calaculation for Strong Acids and Bases||Mixture OF Acids and Bases

The ionisation constant of acetic acid is 1.74xx10^(-5) . The degree of dissociation of acetic acid in its 0.05 m solution and its pH are respectively

Numericals on common ion effect || Properties OF water || Ionic product ph scale, ph calculation for strong monoprotic acids

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.