Calculate approximate pH of the resultant solution formed by titration of 25 mL of 0.04 M Na_(2)CO_(3) with 50 mL of 0.025 M HCl. [Given : pK_(a1)=6.4 and pK_(a2)=10.3 for H_(2)CO_(3)]
Calculate pH of 0.1M HC1.
Calculate the pH of 0.2 M CH_3 COOH (K_a = 1.5 xx 10^-5) .
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
What is the pH of 0.1M NaOH solution?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions