Given that delta Hrxn for OH- ions is -229.6 kJ/mol, calculate the enthalpy of neutralization when I mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at 25-degrees C.
226.9
To calculate the enthalpy of neutralization, we can use the formula:
ΔHneutralization = ΔHrxn/moles of acid or base
First, we need to determine the number of moles of acid reacting with the base. Since we have 1 mole of acid (HCl) and 1 mole of base (KOH), the number of moles of acid or base is 1.
Now, we can substitute the values into the formula:
ΔHneutralization = -229.6 kJ/mol / 1 mol
Therefore, the enthalphy of neutralization is -229.6 kJ/mol.