Home
Class 11
CHEMISTRY
0.2 M solution of a weak acid HA is 1 % ...

`0.2 M` solution of a weak acid `HA` is `1 %` ionised `25^(@)C`. `K_(a)` for the acid is equal to

A

`(0.002xx0.002)/(0.198)`

B

`(0.02xx0.02)/(0.18)`

C

`(0.01xx0.01)/(0.19)`

D

`(0.19)/(0.01xx0.01)`

Text Solution

Verified by Experts

The correct Answer is:
A
`HA+H_(2)OhArr H_(3)O^(-)+A^(-)`
`[HA] =0.2-(0.02xx1)/(100)=0.198 M`
`[A^(-1)]=0.002 M`
`[H_(3)O^(+)]=0.002 M`
`K_(a)=([H_(3)O^(+)][A-])/([HA])=(0.002xx0.002)/(0.198)`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBIUM

    A2Z|Exercise Ph, Pkw And Ph Mixture Of Acid And Bases|55 Videos

  • IONIC EQUILIBIUM

    A2Z|Exercise Salt Hydrolysis|36 Videos

  • HYDROGEN

    A2Z|Exercise Section D - Chapter End Test|30 Videos

  • MOCK TEST

    A2Z|Exercise Mock Test 2|45 Videos

Similar Questions

Explore conceptually related problems

A 0.10 M solution of weak acid is 5.75% ionized. What is the K_a value for this acid ?

0.5 molar aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86 K kg mol^(-1) , the lowering in freezing point of the solution is

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86K kg mol^(-1) , the lowering in freezing point of the solution is

0.1 M solution of a salt of a weak acid a strong base hydrolysis. If K_(a) of the weak acid is 1 xx 10^(-5) , the percent hydrolysis of the salt is

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_(f) for water is 1.86^(@)C//m , the freezing point of the solution will be.

If 0.2 molal aqueous solution of a weak acid (HA) is 40% ionised then the freezing point of the solution will be ( K_f for water = 1.86^@ C

A2Z-IONIC EQUILIBIUM-Section D - Chapter End Test
  1. 0.2 M solution of a weak acid HA is 1 % ionised 25^(@)C. K(a) for the ...

    Text Solution

    |

  2. If the degree of ionization of water be 1.8xx10^(-9) at 298 K. Its ion...

    Text Solution

    |

  3. When a solution of benzoic acid was titrated with NaOH the pH of the s...

    Text Solution

    |

  4. 10^(-2) mole of NaOH was added to 10 litres of water. The pH will chan...

    Text Solution

    |

  5. If an acidic indicator HIn ionies as HInhArrH^(+)+In^(-). To which max...

    Text Solution

    |

  6. Let the solubilities of AgCl in pure water be 0.01 M CaCl(2), 0.01 M N...

    Text Solution

    |

  7. What would be the pH of an ammonia solution if that of an acetic acid ...

    Text Solution

    |

  8. pH of saturated solution of Ba(OH)(2) is 12. The value of solubility p...

    Text Solution

    |

  9. The hydrolysis constant for ZnCl(2) will be where K(b) is effective ...

    Text Solution

    |

  10. In which case pH will not change on dilution

    Text Solution

    |

  11. M(OH)(X) has K(SP) 4xx10^(-12) and solubility 10^(-4) M. The value of ...

    Text Solution

    |

  12. 1 M benzoic acid (pKa=4.20) and 1 M C6H5COONa solutions are given sepa...

    Text Solution

    |

  13. The pH of an aqueous solution of 0.1 M solution of a weak monoprotic a...

    Text Solution

    |

  14. pH of a 10^(-10) M NaOH is nearest to

    Text Solution

    |

  15. The dissocication constant of a weak acid is 1.0xx10^(-5), the equilib...

    Text Solution

    |

  16. The pH of 0.1 M solution of the following salts increases in the order

    Text Solution

    |

  17. In the equilibrium A^(-)+H(2)OhArrHA+OH^(-)(K(a)=1.0xx10^(-5)). The de...

    Text Solution

    |

  18. The sulphide ion concentration [S^(2-)] in saturated H(2)S solution is...

    Text Solution

    |

  19. The K(sp) of CuS, Ag(2)S and HgS are 10^(-31), 10^(-44) and 10^(-54) r...

    Text Solution

    |

  20. For a weak acid HA with dissociation constant 10^(-9), pOH of its 0.1 ...

    Text Solution

    |

  21. The concentration of [H^(+)] and concentration of [OH^(-)] of a 0.1 aq...

    Text Solution

    |