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Which of the following statement(s) is/a...

Which of the following statement(s) is/are correct?
(A) The pH of `1xx10^(-8)` M HCl solution is 8.
(B) The conjugate base of `H_2PO_4^-`is `HPO_4^(2-)`
(C)`K_w` increases with increase in temperature
(D)When a solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point,pH = 1/2 `pK_a`.
Choose the correct answer from the options given below:

A

(B),(C)

B

(B),(C),(D)

C

(A),(B),(C)

D

(A),(D)

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Which of the following statement (s) is (are) correct ? (1) . The pH of 1.0 xx 10^(-8) M solution of HCI is 8 (2). The conjugate base of H_(2)PO_(4)^(-) " is " HPO_(4)^(2-) (3). Autoprotolysis constant of water increases with temperature (4). When a solution of a weak monoprotic acid is titrated against a strong base at half neutralization point pH = (1//2) pK_(a)

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

The pH of 1 M PO_(4)^(3-) (aq) solution (given pK_(b) of PO_(4)^(3-) = 2 ) is

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.

A weak base (BOH) with K_(b) = 10^(-5) is titrated with a strong acid (HCl) , At 3//4 th of the equivalence point, pH of the solution is:

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. Which of the following statements are wrong ? (1) Increase in temperature has no effect on neutral nature of water. (2) Increase in temperature of pure water decreases its pH. (3) Increase in temperature of pure water decreases its autoprolysis. (4) Increase in temperature of pure increase its ionic product. (5) Increase in temperature of pure water decreaseas degree of dissociation of water.

H_(2) A is a weak diprotic acid. If the pH of 0.1 M H_(2)A solution is 3 and concentration of A^(2-) is 10^(-12) at 25^(@)C. Select correct statement (s)

Titration of diprotic acid (H_(2)A) by strong base has been summarised in following graph What is composition of mixture when pH of solution is 10.137?

Calcuate the degree of ionisation and pH of 0.05 M solution of a weak base having the ionization constant (K_(b)) is 1.77xx10^(-5). Also calculate the ionisation constnat of the conjugate acid of this base.

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