In the titration of solution of a weak acid HA and NaOH, the pH is 5.0 after 10 mL of NaOH solution has been added and 5.60 after 20 mL NaOH has been added. What is the value of `pK_(a)` for HA?
If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :
A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?
An aqueous solution of ethanol has density 1.025 g/mL and it is 2 M. What is the molality of this solution ?
During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:
pH of 0.01 M aq. Solution of HA is 4. Find the value of pK_(a) of HA at 25^(@)C.
A sample of NaOH weighing 0.38 g is dissolved in water and solution is made to 50.0 mL in a volumetric flask. What is the molarity of the solution?
An aqueous solution containing 6 g of ureas in 500 mL of solution has a density equal to 1.05. if the molar mass of urea is 60. then the molality of solution is
100 mL of a solution containing 5 g of NaOH are mixed with 200 mL of M/5 NaOH solution. Calculate the molarity of the resulting solution.
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 pH of solution in which 25.0 mL of 0.1 M NaOH is added to 25 mL of 0.08 M HCl and final solution is diluted to 500 mL?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
