Ionic EquilibriumHard
Question
An amount of 0.16 g of N2H4 is dissolved in water and the total volume is made up to 500 ml. What is the percentage of N2H4 that has reacted with water in this solution? The value of Kb for N2H4 = 4.0 × 10−6.
Options
A.0.02%
B.0.014%
C.2%
D.2.82%
Solution
$\left\lbrack W_{2}H_{4} \right\rbrack_{O} = \frac{0.16/32}{500/1000} = 0.01\text{ M}$
$\therefore\alpha = \sqrt{\frac{4 \times 10^{- 6}}{0.01}} = 0.02\text{ or 2\%}$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
The sodium salt of a certain weak monobasic organic acid is hydrolysed to an extent of 3% in its 0.1M solution at 25oC. ...A sample of AgCl was treated with 5.00 ml of 2.0 M Na2CO3 solution to give Ag2CO3. The remaining solution contained 0.00...The only incorrect information related with 0.09 M solution of (NH2CH2CH2NH2) ethylenediamine(en) is(Kb1 = 8.1 × 10–5, K...When 0.1 mole solid NaOH is added in 1lt of 0.1 M NH3(aq) then which statement is wrong? (Kb = 2 × 10-5, log 2 = 0....The pH of 10-8 M solution of HCl in water is :...