Ionic EquilibriumHard
Question
A recent investigation of the complexation of SCN– with Fe3+ led to values of 125, 20 and 1.0 for K1, K2 and K3, respectively. What is the dissociation constant of Fe(SCN)3 into its simplest ions on the basis of these data?
Options
A.2.5 × 103
B.4.0 × 10–4
C.1.0
D.8.0 × 10–3
Solution
$K_{\text{formation}} = K_{1}.K_{2}.K_{3} = 125 \times 20 \times 1 = 2500$
$\therefore K_{\text{dissociation}} = \frac{1}{K_{\text{formation}}} = 4 \times 10^{- 4}$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
The equilibrium constant for the following reaction will be: 3A + 2B → C...A volume of 10 ml of a strong acid solution of pH = 2.0 are mixed with 990 ml of a buffer solution of pH = 4.0. The pH o...The pH value of ordinary water is :...The solubility product of AgCl is 1.8 × 10-10. Precipitation of AgCl will occur only when equal volumes of solution...Equal volumes of equimolar solutions of a weak acid and a weak base both having dissociation constant equal to 5 × ...