Home
Class 12
CHEMISTRY
The pH at the equivalence point of a tit...

The pH at the equivalence point of a titration may differ from `7.0` because of

A

the self ionization of water

B

hydrolysis of the salt formed

C

the indicator used

D

the concentration of the standard solutions.

Text Solution

Verified by Experts

The correct Answer is:
B

Equivalence point of a titrations may differ from 7 due to salt hydrolysis.
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    DINESH PUBLICATION|Exercise SELECTED STRAIGHT OBJECTIVE TYPE MCQs|10 Videos
  • IONIC EQUILIBRIUM

    DINESH PUBLICATION|Exercise MCQs with only one correct Answer|29 Videos
  • IONIC EQUILIBRIUM

    DINESH PUBLICATION|Exercise MULTIPLE CHOICE QUESTIONS|60 Videos
  • HYDROCARBONS

    DINESH PUBLICATION|Exercise All Questions|493 Videos
  • NO IDEA

    DINESH PUBLICATION|Exercise Unit Test -|1 Videos

Similar Questions

Explore conceptually related problems

What will be the pH at the equivalence point during the titration of a 100 mL 0.2 M solution of CH_(3)CCONa with 0.2 M solution of HCl ? K_(a)=2xx10^(-5)

What is the pH at the equivalenve point for the titration of 0.20 M aniline (K_(b) = 7.95 xx 10^(-10)) with 0.20 M HCL

The pH at the equivalent point for the titration of 0.10 M KH_(2)BO_(3) with 0.1 M HCl is (K_(a)" of "H_(3)BO_(3)=12.8xx10^(-10)) Report your answer by rounding it up to nearest whole number.

Calcualte the pH at the equivalence point when a solution of 0.1M acetic is titrated with a solution of 0.1M NaOH.(K_(a)for acid = 1.9xx10^(-5)) .

Calculate the pH at the equivalence point during the titration of 0.1M, 25 mL CH_(3)COOH with 0.05M NaOH solution. [K_(a)(CH_(3)COOH) = 1.8 xx 10^(-5)]

Calculate the pH at the equivalence point when a solution of 0.1M acetic acid is titrated with a solu- tion of 0.1M NaOH, K_a for acid =2 xx 10^(-5)-

DINESH PUBLICATION-IONIC EQUILIBRIUM -REVISION QUESTIONS FROM COMPETITVE EXAMS
  1. Degree of dissociation of 0.1 N CH(3)COOHis ( Dissociation constant =1...

    Text Solution

    |

  2. Which of the following is not a Lewis acid ?

    Text Solution

    |

  3. The pH at the equivalence point of a titration may differ from 7.0 bec...

    Text Solution

    |

  4. A weak monobasic acid is half neutralized by a strong base. If the Ph ...

    Text Solution

    |

  5. ZnS is not precipitated by passing H(2)S in acidic medium but CuS is p...

    Text Solution

    |

  6. When 30 mL of 5.93 millimolar solution of AgNO(3) was added to 2.0 mL ...

    Text Solution

    |

  7. Choose the correct order arranged in decreasing order of basicity

    Text Solution

    |

  8. HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degr...

    Text Solution

    |

  9. Which of the following solvents are aprotic ? (1) NH(3)" "(2)SO(2...

    Text Solution

    |

  10. The aqueous solutions of HCOONa, C(6)H(5)NH(3)CI, and KCN are, respect...

    Text Solution

    |

  11. An example of a Lewis acid is

    Text Solution

    |

  12. 100 cc of HCl of pH value 1 is mixed with 100 cc of distilled water. T...

    Text Solution

    |

  13. The pH of neutral water is 6.5 , then the temperature of water is

    Text Solution

    |

  14. For a 'C'M concentarted solution of a weak electrolyte A(x)B(y)alpha(d...

    Text Solution

    |

  15. The pH of a solution obtained by mixing 50 mL of 1N HCl and 30 mL of 1...

    Text Solution

    |

  16. The number of H^(+) ions present in 250 ml of lemon juice of pH=3 is

    Text Solution

    |

  17. The precipitate of Ag(2)CrO(4)(K(sp))=1.1 xx 10^(-12) is obtained when...

    Text Solution

    |

  18. When solid lead iodide is added to water, the equilibrium concentratio...

    Text Solution

    |

  19. A 0.010M solution of maleic acid, a monoprotic organic acid is 14% ion...

    Text Solution

    |

  20. The pH of a 0.1M solution of NH(4)Oh (having dissociation constant K(b...

    Text Solution

    |