0 calculate AH for the CI ions. f kJ/mol (b) Given that AH for OH¯ ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole f 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
0 calculate AH for the CI ions. f kJ/mol (b) Given that AH for OH¯ ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole f 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
General Chemistry - Standalone book (MindTap Course List)
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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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
HCl(g)
H₂O
→ H*(aq) + Cl¯(aq)
0
calculate ΔΗ for the CI ions.
f
kJ/mol
AHO
kJ/mol
rxn
= -74.9 kJ/mol
(b) Given that AH for OH ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole
ΔΗ
f
of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F813c1858-330a-4765-86df-c6b16594416a%2F500b89a0-a1a0-43fc-9617-9de066299258%2F46nf0hr_processed.png&w=3840&q=75)
Transcribed Image Text: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
HCl(g)
H₂O
→ H*(aq) + Cl¯(aq)
0
calculate ΔΗ for the CI ions.
f
kJ/mol
AHO
kJ/mol
rxn
= -74.9 kJ/mol
(b) Given that AH for OH ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole
ΔΗ
f
of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25°C.
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