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 :
A buffer solution is prepared by mixing 50 mL of 0.2 M of acetic acid with .x. mL of 0.2 M of NaOH solutions. If pH of the resulting buffer solutions is 4. 7 then value of .x. is (Ka= 2xx10 ^(-5))
20 mL of 0.2 M sodium hydroxide solution is added to 40 mL of 0.2 M acetic acid solution. What is the pH of the solution? (pK_(a) " of "CH_(3)COOH=4.8)
Define pH. What is buffer solution? Derive Henderson-Hasselbalch equation for calculating the pH of an acid buffer solution.
2 g of NaOH per 250 ml of solution is added to a buffer solution of buffer capacity 0.2 . Then the change in pH is
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132 . Calculate the pH of the solution and the pK_(a) of bromoacetic acid.
50 ml of 0.2 M HCl is added to 30 ml of 0.1 MKOH solution. Find the pH of the solution.
200 ml of KMnO_4 solution is exactly reduced by 100 ml, 0.5M oxalic acid solution. Find the molarity of KMnO_4 solution.
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
