3 attempts left Check my work Be sure to answer all parts. The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a walue of zero to H ions; that is, AH [H'(aq)] = 0. a) For the following reaction HCIG) H20 - H'(aq) + CI (aq) AH = -74.9 kJ/mol rxn calculate AH for the CI ions. kJ/mol (b) Given that AH for OH ions is -229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25°C. kJ/mol < Prev 11 of 26

Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Be sure to answer all parts.
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a
value of zero to H ions; that is, AH [H*(aq)]
= 0.
(a) For the following reaction
H20
→ H'(aq) + CI (aq)
HC(g)
ΔΗ
= -74.9 kJ/mol
rxn
calculate AH for the CI ions.
kJ/mol
(b) Given that AH for OH ions is -229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of
a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25°C.
kJ/mol
< Prev
11 of 26
Transcribed Image Text:Saved ment 3 attempts left Check my work Be sure to answer all parts. The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H ions; that is, AH [H*(aq)] = 0. (a) For the following reaction H20 → H'(aq) + CI (aq) HC(g) ΔΗ = -74.9 kJ/mol rxn calculate AH for the CI ions. kJ/mol (b) Given that AH for OH ions is -229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25°C. kJ/mol < Prev 11 of 26
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