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 ?
A
`1%`
B
`3.57%`
C
`35.7%`
D
0.1
Text Solution
Verified by Experts
The correct Answer is:
B
`HArarrH^(+)+A^(-),Delta_(r)H=1.4` kJ/mol `DeltaH_("neutralization")=DeltaH_("ionization")+Delta_(r)H` `(H^(+)+OH^(-)rarrH_(2)O)` `-55.95=DeltaH_("ionization")-57.3` `DeltaH_("ionization")" for 1 M HA = 1.35 kJ"//"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
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