`6.0` g weak acid HA (mol.mass=60 g/mol.) is dissolved in water and formed 10 `m^(3)` solution. If `K_(a)(HA)=10^(-9),` then pOH of solution is : [Given: log 4=0.6]
10.6 g Na_2CO_3 are dissolved in water to give 2 M solution. What is the volume of the solution in ml?
5.85g of NaCl (mol. wt. 58.5) is dissolved in water and the solution is made up to 500 ml. The molarity of the solution will be
4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.
6g. of Urea is dissolved in 90g. of water. The mole fraction of solute is
6 g. of Urea is dissolved in 90 g. of water. The mole fraction of solute is
0.84 g of a acid (mol wt. 150) was dissolved in water and the volume was made up to 100 ml. 25 ml of this solution required 28 ml of (N/10) NaOH solution for neutralisation. The equivalent weight and basicity of the acid
9.5g of MgCl_(2) is dissolved in 100 g of water . The freezing point of the solution is -4.836^(@)C Then .
6 g of urea is dissolved in 90g of boiling water. The vapour pressure of the solution is
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
