When 0.1 mole of `NH_(3)` is dissolved in water to make 1.0 L of solution, the `[OH^(-)]`of solution is `1.30xx10^(-3)M.` Calculate `K_(b)` for ` NH_(3).`

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) .

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) .

When 0.10 mol of ammonia NH_3 is dissolved in sufficient water to make 1.0L of solution, the solution is found to have a hydroxide ion concentration of 1.34 xx 10^(-3) . Calculate k_b for Ammonia.

Calculate [OH^(-)] in 0.20M solution of NH_(3) , if K_(b) for NH_(3) is 1.8xx10^(-5) .

0.00135 mole of NH_(3) dissociates in 1.0 litre solution of 0.10M . Calculate the dissociation constant of NH_(3) .

To a solution of 0.01M Mg^(2+) and 0.8M NH_(4)CI , and equal volume of NH_(3) is added which just gives precipitates. Calculate [NH_(3)] in solution. K_(sp) of Mg(OH)_(2) = 1.4 xx 10^(-11) and K_(b) of NH_(4)OH = 1.8 xx 10^(-5) .

To a solution of 0.01M Mg^(2+) and 0.8M NH_(4)CI , and equal volume of NH_(3) is added which just gives precipitates. Calculate [NH_(3)] in solution. K_(sp) of Mg(OH)_(2) = 1.4 xx 10^(-11) and K_(b) of NH_(4)OH = 1.8 xx 10^(-5) .