Home
Class 11
CHEMISTRY
Strong acids are generally used as stand...

Strong acids are generally used as standard solution in acid-base titrations because:

A

The `pH` at the equivalent point will always be `7`.

B

They can be used to titrate both strong and weak bases.

C

Strong acids from more stable soluitons than weak acids.

D

The salts of strong acids do not hydrolyse.

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 8.5|6 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises Subjective (Weak Acid And Weak Bases)|15 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 8.3|38 Videos

  • HYDROGEN, WATER AND HYDROGEN PEROXIDE

    CENGAGE CHEMISTRY ENGLISH|Exercise Subjective Archive (Subjective)|3 Videos

  • ISOMERISM

    CENGAGE CHEMISTRY ENGLISH|Exercise Assertion-Reasoning Type|1 Videos

Similar Questions

Explore conceptually related problems

Discuss the various types of acid-base titrations using indicators.

Conductance measurements and be used to detect the end point of acid-base titrations. Which of the following plots correctly represents the end point of the titration of strong acid and a strong base?

During titration H_2SO_4 is preferably used over HCl and HNO_3 to make the solution acidic because

Explain why phenolphthalein is used as an indicator in acid-base titration. ""^(**"**)

Which of the following are true for an acid- base titration?

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid /base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) What is DeltaH^(@) for complate neutralization of strong diacidic base A(OH)_(2)by HNO_(3) ?

Which of the following is/are true for an acid- base titration?

The rapid change of pH near the stoichiometric point of an acid-base titration is the basic of indicator detection. pH of the solution is related to the ratio of the concentration of conjugate acid (Hin) and base (In^(-)) forms of the indicator by the expression

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid // base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) under same conditions ,how many mL of 0.1 m NaOH and 0.05 M H_(2)A (strong diprotic acid ) solution should be mixed for a total volume of 100mL to producce the hight rise in temperature ?

Following two graphs are based on the conductometric titration of acid-base reaction. Answer the questions given at the end of it. Select correct statement,

CENGAGE CHEMISTRY ENGLISH-IONIC EQUILIBRIUM-Ex 8.4
  1. The pH indicators are

    Text Solution

    |

  2. In which of the following acid-base titration, the pH is greater than ...

    Text Solution

    |

  3. Strong acids are generally used as standard solution in acid-base titr...

    Text Solution

    |

  4. The best indicator for detection of end point in titration of a weak a...

    Text Solution

    |

  5. The precipitate of CaF(2) (K(sp)=1.7xx10^(-10)) is obtained when equal...

    Text Solution

    |

  6. The solubility of A(2)B(3) is "x mol dm"^(-3). Its K(sp) is

    Text Solution

    |

  7. The pH of Ca(OH)(2) is 10.6 at 25^(@)C. K(sp) of Ca(OH)(2) is

    Text Solution

    |

  8. Solubility of AgI in 0.05M BaI(2) solution is 10^(-15)M. The solubilit...

    Text Solution

    |

  9. Solubility of a solute in water is dependent on temperature as given b...

    Text Solution

    |

  10. The solubility of CaF(2) in a solution of 0.1M Ca(NO(3))(2) is

    Text Solution

    |

  11. The volume of water needed to dissolve 1mg of PbSO(4) (K(sp) = 1.44 xx...

    Text Solution

    |

  12. The volume of water needed to prepare a satured solution of Ag^(o+) ha...

    Text Solution

    |

  13. How many grams of KBr can be added to 1L of 0.12 M solution of AgNO(3)...

    Text Solution

    |

  14. The solubility of silver benzoate (C(6)H(5)COOAg) in H(2)O and in a bu...

    Text Solution

    |

  15. The solubility of CH(3)COOAg in a buffer solution with pH = 4, whose K...

    Text Solution

    |

  16. the ratio of solubility of CH(3)COOAg in a buffer solution with pH = 4...

    Text Solution

    |

  17. What is the maximum molarity of Co^(+2) ions in 0.1M HC1 saturated wit...

    Text Solution

    |

  18. The following curve shows the change of pH during the course of titrat...

    Text Solution

    |

  19. If the salts M(2)X,QY(2), and PZ(3) have the same solubilities (lt(4)/...

    Text Solution

    |

  20. Arrange the following solutions in decreasing order of [Ag^(o+)] ion: ...

    Text Solution

    |