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Statement-1 : Chemical equation H^(+)(aq...

Statement-1 : Chemical equation `H^(+)(aq) + OH^(-)(aq) rarr H_(2)O(I), Delta H = -X` kJ represents the enthalpy of formation of water
And
Statement-2 : `Delta H_("neutralisation")` of strong acid and strong base is constant.

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1

B

Statement-1 is True, Statement-2 is True, Statement-2 is Not a correct explanation for Statement-1

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False, Statement-2 is True

Text Solution

Verified by Experts

The correct Answer is:
D
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From the following data, mark the option (s) where Delta H is correctlt written for the given reaction. Given H^(+)(aq) + OH^(-)(aq) rarr H_(2)O(l), Delta H = -57.3 kJ Delta H_("solution") of HA(g) = -70.7kJ/mol Delta H_("solution") of BOH(g) = 20kJ/mol Delta H_("ionization") of HA = 15 kJ/mol and BOH is a strong base Reaction Delta H_(r)(kJ//mol)

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HA+OH^(-) to H_(2)O+A^(-)+q_(1) kJ H^(+)+OH^(-) to H_(2)O+ q_(2) kJ The enthalpy of dissociation of HA is

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) ?

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) If enthalpy of neutralization of CH_(3)COOH by NaOH is -49.86KJ // mol then enthalpy of ionization of CH_(3)COOH is:

Knowledge Check

  • H_2+Cl_2 rarr 2HCl,Delta H =- 194 kJ. In this reaction, heat of formation of HCl in KJ is

    A
    `+ 194 kJ `
    B
    `+97 kJ`
    C
    `-97 kJ`
    D
    `-194 kJ`.

  • 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_(r)H^(@) = -55.84 KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero. When a dilute solution of a weak acid or base is neutalized, teh enthalpy of neutralization is some what less because of the absorption of heat in the ionization of the weak acid or base, for weak acid/base DeltaH_("neutrilization")^(2) = DeltaH_("ionization")^(@) + Delta_(r)H^(@) " " (H^(+) + OH^(-) rarr H_(2)O) Under the same condition 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 100 mL produce the highest rise in temperature:

    A
    `25:75`
    B
    `50:50`
    C
    `75:25`
    D
    `66.66:33.33`

  • From the following data, mark the option (s) where Delta H is correctlt written for the given reaction. Given H^(+)(aq) + OH^(-)(aq) rarr H_(2)O(l), Delta H = -57.3 kJ Delta H_("solution") of HA(g) = -70.7kJ/mol Delta H_("solution") of BOH(g) = 20kJ/mol Delta H_("ionization") of HA = 15 kJ/mol and BOH is a strong base Reaction Delta H_(r)(kJ//mol)

    A
    `HA(aq)+BOH(aq) rarr BA(aq)+H_(2)O - 42.3`
    B
    `HA(g) + BOH(g) rarr BA(aq)+H_(2)O -93.0`
    C
    `HA(g) rarr H^(+)(aq)+A^(-)(aq)-55.7`
    D
    `B^(+)(aq)+OH^(-)(aq) rarr BOH (aq) - 20.0`