Ionic EquilibriumHard
Question
100 ml of 0.5M hydrazoic acid (HN3, Ka = 3.6 × 10-4) and 400ml of 0.1M cyanic acid (HOCN, Ka = 8 × 10-4) are mixed. which of the following is (are) true for the final solution?
Options
A.[H+] = 10-2 M
B.[N3-] = 3.6 × 10-3 M
C.[OCN-] = 6.4 × 10-3 M
D.[H+] = 1.4 × 10-2 M
Solution
Total [H+] = 
∴ [H+] = 10-2 M.
For HN3, [N3-] =
× 100 = 3.6 × 10-3 M.
For HOCN, [OCN-] =
= 6.4 × 10-3 M.
∴ [H+] = 10-2 M.
For HN3, [N3-] =
× 100 = 3.6 × 10-3 M.For HOCN, [OCN-] =
= 6.4 × 10-3 M.Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Protective sols are :-...Select the correct statements : 1. pH of NaHCO3 solution can be given by 2. AI3+ ion is amphoteric3. KSP values of metal...Which is/are correct statements : (a) When 100 ml of 0.1 M NaCN solution is titrated with 0.1 M HCl solution the variati...The pH of 0.1 M solution of the following salts increases in the order:...1.4 g of an organic compound was digested according to Kjeldahl′s method and the ammonia evolved was absorbed in 6...