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To 1L of a 1.6xx10^(-3)M aqueous solutio...

To `1L` of a `1.6xx10^(-3)M` aqueous solution of ethylene diamine `(K_(b_(1))=8xx10^(-5),K_(b_(2))=2.7xx10^(-8)),5xx10^(-4)` mole of `Ba(OH)_(2)` is added.Then:

A

`pH_(f)-pH_(i)=0.5`

B

`alpha_(i)-alpha_(f)=0.12`

C

`([C_(2)N_(2)H_(10)^(2+)])/([C_(2)N_(2)H_(10)^(2+)]_(f))=0.128`

D

`([C_(2)N_(2)H_(9)^(+)]_(i))/([C_(2)N_(2)H_(9)^(2+)]_(f))=0.128`

Text Solution

AI Generated Solution

To solve the problem, we need to analyze the effects of adding barium hydroxide (Ba(OH)₂) to the ethylene diamine solution. We'll follow these steps: ### Step 1: Calculate the initial degree of dissociation (α) of ethylene diamine. 1. **Write the equilibrium expression for the first dissociation of ethylene diamine:** \[ \text{C}_2\text{N}_2\text{H}_8 + \text{H}_2\text{O} \rightleftharpoons \text{C}_2\text{N}_2\text{H}_9^+ + \text{OH}^- \] ...
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