The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* lons; that is, AHH* (aq)]=0. H₂O HCI (g) →→→ H (aq) + CI (aq) Part 1 of 2 Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 2 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. X AH = -74.7 rxn 00 kJ mol S Calculate the enthalpy of neutralization when I mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits.

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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.
H₂O
HC1 (g) →H (aq) + Cl¯ (aq)
Note: Reference the Thermodynamic properties of pure substances table for additional information.
Part 1 of 2
For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits.
Part 2 of 2
□
0x10
X
□
0.0
kJ
ΔΗ% = -14.7 mol
S
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. Round your answer to 3 significant digits.
010
Transcribed Image Text: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. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S 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. Round your answer to 3 significant digits. 010
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