0.1 M formic acid solution is titrated against 0.1 M NaOH solution. What would be the difference in pH between 1/5 and 4/5 stages of neutralization of acid?
10 mL of H_(2)A (weak diprtic acid) solutio is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following obserbation is made Ip pH of the solution at first equivalence point is pH_(1) and at secnd equibalence point is pH_(2^.) Calculate the value of (pH_(2)-pH_(1)) at 25^(@)C Given for H_(2)A,pK_(a_1) =4.6 and pK_(a_2) =8, log 25=1.4
10mL of 0.1 M HCl solution reacts completely with 10 mL of 0.1 M NaOH solution. What will be the pH of the resulting solution?
What is the normality of 1.0 M NaOH?
When 100 mL of 0.1 M NaCN solution is titrated with 0.1 M HCl solution the variation of pH of solution with volume of HCl added will be :
What is the pH of 0.1 M HCl ?
Fixed volume of 0.1 M benzoic acid (pK_(a)=4.2) solution is added into 0.2 M sodium benzoate solution and formed a 300 mL, resultant acidic buffer solution. If pH of this buffer solution is 4.5 then find added volume of benzoic acid :
The compound whose 0.1 M solution is acidic :
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
