1.

Find the pH at equivalence points when a soluiton of 0.1M acetic acid is titrated with a solution of 0.3M NaOH K_(a) for acetic acid =7.5xx10^(-6)

Answer»

Solution :AT equivalence point `CH_(3)COONa` will be formed.
`M_("base")V_("base")=M_("acid")V_("acid")rArr V_("acid")=(0.3)/(0.1)V_("base")=3V_("base")`
`[CH_(3)COONa]_("Equivalent point")=("Total moles")/("Total volume")=(0.3xxV_("base"))/(V_("acid")+V_("base"))=(0.3V_("base"))/(4V_("base"))=0.075`
`[OH^(-)]=sqrt((K_(W))/(K_(a))XXC)=sqrt((10^(-14))/(7.5xx10^(-6))xx0.075)xx10^(-5)rArrpOH=5 :.pH=9`


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