The enthalpy of neutralization of a Weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 KJ/mol . If the unionized acid required 1.4 KJ/mol heat for it's comptate ionzatation and enthalpy of netralization of the strong monobasic acid with a strong monoacidic base is -57.3 KJ/mol . What is the % ionzation of the weak acid in molar solution ?

Options

A. `1%`
B. `3.57%`
C. `35.7%`
D. `10%`

Answer

2

Explanation

`HArarrH^(+)+A^(-),Delta_(f)H=1.4kJ//mol`
`DeltaH_("neutralization")=DeltaH_("Ionization")+Delta_(r)H` of `(H^(+)+OH^(-)rarrH_(2)O)`
`-55.95=Delta H_("ionization")-57.3`
`DeltaH_("ionization")` for `1MHA=1.35kJ //mol`
`%` heat utilized by `1` M acid for ionization
`=(1.35)/(1.4)xx100=96.43%`
So, acid is `100-96.43=3.57%` ionized