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A solution which resists the cahnge in i...

A solution which resists the cahnge in its pH value on addition of some amount of acid or base is called

A

A colloid

B

A crystalloid

C

A buffer

D

An indicator

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Assertion : Buffer solutions are those which resist change in pH value on the addition of a small amount of acid or a base to it. Reason: Mixture of NH_4OH and NH_4 Cl acts as basic buffer.

Assertion (A ) : A buffer solution has a capacity to resist the change in pH value on addition is small amount of acid or base to it. Reason (R ) : An aqueous solution of ammonium acetate can act as a buffer.

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) 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 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. 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.

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.

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 pH of II gp. filtrate during III gp. basic radicals precipitation in qualitative anlysis is maintained by using a buffer solution of:

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) 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: