InterviewSolution
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InterviewSolution
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When 0.1 mole of `NH_(3)` is dissolved in water to make 1.0 L of solution , the `[OH^(-)]` of solution is `1.34 xx 10^(-3)`M. Calculate `K_(b)` for `NH_(3)`. |
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Answer» Degree of dissociation of `NH_(3) " or " NH_(4)OH i.e. alpha = (1.34 xx 10^(-3))/(0.1) = 1.34 xx 10^(-2)` According to Ostwald Dilution formula `alpha=sqrt((K_(b))/(C)) " or " K_(b) =alpha^(2)C` `K_(b) = (1.34 xx 10^(-2))^(2)xx (0.1) =1.8 xx 10^(-5)` |
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