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 :
A 25.0ml sample of 0.1 M HCl is titrated with 0.1 M NaOH . What is the pH of the solution at the points where 24.9 and 25.1 ml of NaOH have been added ?
20 gm of sample Ba(OH)_(2) is dissolved in 10 ml of 0.5 N HCl solution, The excess of HCl was titrated with 0.2 NaOH. The volume of NaOh used was 10 mol. Calculate the % of Ba(OH)_(2) in the sample.
What is the pH of the NaOH solution when 0.04 g of it is dissolved in water and made to 100 ml solution?
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
20 ml of 0.1 M NH, solution is titrated with 0.025M HCI solution. What is the pH of the reaction mixture at equivalence point at 25^(@) C ? (K_(b) "of " NH_(3) "is " 2 xx 10^(-6)) .
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.
If the equlibrium constant for the reaction of weak acid HA with strong base is 10^(9) then calculate the pH of 0.1 M NaA.
The pH of 0.1 M solution of weak mono protic acid is 4.0. Calculate its [H^(+)] and Ka .
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
