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The dissociation of weak electrolyte (a ...

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?

A

`HCO_(3)^(-)`and `CO_(3)^(2-)`

B

`CH_(3)COO^(-)`and `CH_(3)COOH`

C

`NH_(4)^(-)` and `NH_(4)OH`

D

None of the above

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The correct Answer is:
a
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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) 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 follwoing statement are true? (P) CIO_(4)^(-) is weaker base than CIO_(3)^(-) (Q) The degree of dissociation of water at 25^(@)C is 1.8xx10^(-9) (R)The equilibrium constant for dissociation of H_(2)O is 1.8xx10^(-16) (S) PO_(4)^(3-) is conjugate acid of HPO_(4)^(2-)

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. Which of the following statements are true ? (1) CIO_(4)^(-) is weak base than CIO_(3)^(-) (2) The degree of dissociation of weak is 1.8xx10^(-9) (3) The equilibrium constant for dissociation of H_(2)O is 1.78xx10^(-16) (4) PO_(4)^(3-) is conjugate acid of HPO_(4)^(2-)

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. (Q) Increase in temperature of pure water decreases its pH. (R) Increase in temperature of pure water decreases its autoprotolysis. (S) Increase in temperature of pure water increases its ionic product. (T) Increase in temperature of pure water decreases degree of dissociation of water.

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. 0.16g of N_(2)H_(4)(K_(b)=4xx10^(-6)) is dissolved in water and the total volume of solution in made upto 500mL. The percentage of N_(2)H_(4) that reacts with water 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.

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 correct ? (1) pH of 10^(-10) M NaOH is nearly 7. (2) The degree of dissociation of a weak acid is given by (1)/(1+10^((pK_(aq)-pH)) (3) For weak electrolytes of polyprotic acid nature having no other electrotrolype, the anion concentration produced in II step of dissociation is always equal to K_(2) at reasonable concentration of acid. (4) The concentration of amide ions produced during self ionisation of NH_(3) is equal concentration of ammonium ions. (5) Ostwald's 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. The pK_(a) value of NH_(4)^(+) is 9. The pK_(b) value of NH_(4)OH would be:

GRB PUBLICATION-IONIC EQUILIBRIUM-All Questions
  1. The dissociation of weak electrolyte (a weak base or weak acid) id exp...

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  2. The dissociation of weak electrolyte (a weak base or weak acid) id exp...

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  3. The dissociation of weak electrolyte (a weak base or weak acid) id exp...

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  4. The dissociation of weak electrolyte (a weak base or weak acid) id exp...

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  5. The dissociation of weak electrolyte (a weak base or weak acid) id exp...

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  6. During the neutralisation of an acid by a base, the end point refers t...

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  7. During the neutralisation of an acid by a base, the end point refers t...

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  8. During the neutralisation of an acid by a base, the end point refers t...

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  9. During the neutralisation of an acid by a base, the end point refers t...

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  10. During the neutralisation of an acid by a base, the end point refers t...

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  11. During the neutralisation of an acid by a base, the end point refers t...

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  12. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  13. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  14. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  15. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  16. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  17. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  18. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  19. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  20. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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