Ionic EquilibriumHard
Question
Calculate the formation constant for the reaction of a tri-positive metal ion with thiocyanate ions to form the monocomplex if the total metal concentration in the solution is 2 × 10–3 M, the total SCN– concentration is 1.51 × 10–3 M and the free SCN– concentration is 1.0 × 10–5 M.
Options
A.7.55 × 104
B.3 × 105
C.3.33 × 10−6
D.1.5 × 105
Solution
$M^{3 +} + SCN^{-} \rightleftharpoons M(SCN)^{2 +}$
$2 \times 10^{- 3}M\text{1.51} \times \text{1}\text{0}^{- 3}M0$
Eqn. $2 \times 10^{- 3} - xM\text{1.51} \times \text{1}\text{0}^{- 3} - xMx\text{ M}$
$= 5 \times 10^{- 4}M\text{=1.0} \times \text{1}\text{0}^{- 5}M\text{=1.5} \times \text{1}\text{0}^{- 3}\text{ M}$
$\therefore K_{f} = \frac{1.5 \times 10^{- 3}}{5 \times 10^{- 4} \times 1 \times 10^{- 5}} = 3 \times 10^{5}$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Solubility product constant (Ksp) of salts of types MX, MX2 and M3X at temperature ′T′ are 4.0 × 10-s, ...1.4 g of an organic compound was digested according to Kjeldahl′s method and the ammonia evolved was absorbed in 6...If 50 ml of 0.2 M KOH is added to 40 ml of 0.5 M HCOOH. the pH of the resulting solution is: (Ka = 1.8 × 10-4, log ...Which of the following properties given in pair are shown by sulphurdioxide :-...The dissociation constants of formic and acetic acids are 1.77 × 10−4 and 1.75 × 10−5, respectively. Which of the follow...