`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]
4.0 g of NaOH and 4.9 g of H_(2)SO_(4) are dissolved in water and volume is made upto 250 mL. The pH of this solution is:
What is the precent dissociation (alpha) of a 0.01 M HA solution? (K_(a)=10^(-4))
6.0 g of urea (molecules mass = 60)was dissolved in 9.9 moles of water. If the vspour presssure of pure water is P^(@) , the vapour pressure of solution is :
A 1.025 g sample containing a weak acid HX (mol. Mass=82) is dissolved in 60 mL. water and titrated with 0.25 M NaOH. When half of the acid was neutralised the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Calculate mass precentage of HX in sample :
Dissolving 120g of urea (mol.wt 60) in 1000g of water gave a solution of density 1.15g/ml. The molarity of solution is:
A solution contains 10 g per dm^3 of urea (molar mass 60 "g mol"^(-1) ) is isotonic with 5% solution of non-volatile solute, M_B of solute is
A solution is prepared by dissolving 1.0 g of NaOH in water to get 250 ml of solution . Calculate its molarity .
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
