Home
Class 11
CHEMISTRY
Enthalpy of neutralization is defined as...

Enthalpy of neutralization 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))^(-) rarr H_(2)O_((l)), Delta H_(r )^(0) -= - 55.84 kJ//mol`
If enthalpy of neutralization of `CH_(3)COOH` by NaoH is -49.86 kJ/mol then enthalpy of ionisation of `CH_(3)COOH` is

A

5.98 kJ/mol

B

`-5.98` kJ/mol

C

105.7 kJ/mol

D

none of these

Text Solution

Verified by Experts

The correct Answer is:
A
Expected `rarr 55.84`
`Delta H_("neutralization") = 49.86`
`Delta H_("ionization") = 55.84 - 49.86 = 5.98` kJ/mol
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE- II) (LEVEL- II (ADVANCED) MATRIX MATCHING TYPE QUESTIONS)|2 Videos

  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE- II) (LEVEL- II (ADVANCED) INTEGER TYPE QUESTIONS)|6 Videos

  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE- II) (LEVEL- II (ADVANCED) MORE THAN ONCE CORRECT ANSWER TYPE QUESTIONS)|6 Videos

  • CHEMICAL THERMODYANMICS

    AAKASH SERIES|Exercise Questions For Descriptive Answers|28 Videos

  • ELECTRON MIGRATION EFFECTS

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|10 Videos

Similar Questions

Explore conceptually related problems

Enthalpy of neutralization 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))^(-) rarr H_(2)O_((l)), Delta H_(r )^(0) -= - 55.84 kJ//mol What is Delta H^(0) for complete neutralisation of strong diacidic base A(OH)_(2) " by " HNO_(3) ?

Enthalpy of neutralization 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))^(-) rarr H_(2)O_((l)), Delta H_(r )^(0) -= - 55.84 kJ//mol Under the same conditions how many mL of 0.1M NaOH and 0.05 M H_(2)A (strong diprotic acid) should be mixed for a total volume of 100mL to produce the highest rise in temperature:

Given that (1)/(2)S_(8(s)) + 6O_(2(g)) rarr 4SO_(3(g)), Delta H^(0) = - 1590kJ . The standard enthalpy of formation of SO_(3) is

Enthalpy of neutralisation of H_(3)PO_(3) acid is -106.68kJ//mol using NaOH. If enthaly of neutralisation of HCl by NaOH is -55.84 kJ/mol. Calculate DeltaH_("ionization") " of " H_(3)PO_(3) into its ions

Given N_(2)(g)+3H_(2)(g)to2NH_(3)(g),Delta_(r)H^(theta)=-92.4 kJ mol^(-1) What is the standard enthalpy of formation of NH_(3) gas ?

Calculate enthalpy of ionisation of OH^(-) ion. Given: H_(2)O_((l)) to H_((aq))^(+) + OH_((aq))^(-) , DeltaH^(@) = -285.83 KJ

The enthalpy of formation of ammonia is -46.0 KJ mol^(-1) . The enthalpy change for the reaction 2NH_3 rarr N_2 + 3H_2 is

H_(2(g)) + 1/2O_(2(g)) rarr H_2O_((l)) , DeltaH = -286.2KJ H_2O_((l)) rarr H_((aq))^(+) + OH_((aq))^(-) , DeltaH = +57.3 KJ Enthalpy of ionization OH^(-) in aqueons solution is

Given that the data for neutralization of a weak acid (HA) and strong acid with a strong base is: HA +OH^(-) rArr A^(-) + H_(2)O: DeltaH = -41.80kJ , H^(+) + OH^(-) rArr H_(2)O, Delta H= -55.90kJ The enthalpy of dissociation of weak acid would be