Home
Class 11
CHEMISTRY
The dissociation of weak electrolyte (a ...

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 ?

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 these

Text Solution

Verified by Experts

The correct Answer is:
A
Blood buffer contains this mixture.
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    P BAHADUR|Exercise Exercise|85 Videos

  • IONIC EQUILIBRIUM

    P BAHADUR|Exercise Exercise6|24 Videos

  • GASEOUS STATE

    P BAHADUR|Exercise Exercise -9|1 Videos

  • MOLE AND EQUIVALENT CONCEPT

    P BAHADUR|Exercise Exercise 9 Advanced numerical problems|61 Videos

Similar Questions

Explore conceptually related problems

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 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 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) 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 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) 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 removal of PO_(4)^(3-) in qualitative analysis of basic radicals after II gp. is made by using a buffer solution of:

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 protonation constant for NH_(3) from water is 6xx10^(5) . The deprotonation from NH_(4)^(+) to H_(2)O has rate constant 5.6xx10^(-10) . The rate constant for NH_(4)^(+) and OH^(-) reaction to give NH_(3) and H_(2)O 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. At 50^(@)C , liq. NH_(3) undergoes autoprotlysis to give ammonium and azide ions having dissociation constant equal to 10^(-30) . The number of azide ions present 1 cm^(3) of liq. NH_(3) 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. 0.16g of N_(2)H_(4)(K_(b)=4xx10^(-6)) are dissolved in water and the total volume of solution is made upto 500 mL. The percentage of N_(2)H_(4) that reacts with water is:

P BAHADUR-IONIC EQUILIBRIUM-Exercise7
  1. The dissociation of weak electrolyte (a weak base or weak acid) is exp...

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

  6. The dissociation of weak electrolyte (a weak base or weak acid) is exp...

    Text Solution

    |

  7. The dissociation of weak electrolyte (a weak base or weak acid) is exp...

    Text Solution

    |

  8. The dissociation of weak electrolyte (a weak base or weak acid) is exp...

    Text Solution

    |

  9. The dissociation of weak electrolyte (a weak base or weak acid) is exp...

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

  16. The pH of basic buffer mixtures is given by : pH=pK(a)+log((["Base"])/...

    Text Solution

    |

  17. The pH of basic buffer mixtures is given by : pH=pK(a)+log((["Base"])/...

    Text Solution

    |

  18. The pH of basic buffer mixtures is given by : pH=pK(a)+log((["Base"])/...

    Text Solution

    |

  19. The ratio of pH of solution (1) containing 1 mole of CH(3)COONa and 1 ...

    Text Solution

    |

  20. The pH of basic buffer mixtures is given by : pH=pK(a)+log((["Base"])/...

    Text Solution

    |