Question

A saturated solution of iodine in water is 1.25 × 10^–3 (M). In any saturated solution of I₂ concentration of I₂ is 1.25 × 10^–3 (M). In 1 L of 0.1 (M) solution I^–, it is seen 51.25 × 10^–3 mole of I₂ can be maximum dissolved. In the aqueous solution of I^–(aq), I₂ (ag) undergoes complex formation, I₂ (aq) + I^–$\mathrm { I } _ { 3 } ^ { - }$(aq).

What is the value of K_C ?

• A. 750
• B. 800
• C. $\frac { 1000 } { 51.25 }$
• D. 1

Answer 1

Answer: (B)

800

Answer 2

I₂ + I^– $\mathrm { I } _ { 3 } ^ { - }$

51.25 × 10^–3 0.1

At 1.25 × 10^–3(M) 50 × 10^–3(M) 50 × 10^–3(M)

Equilibrium

K_C = $\frac { 50 \times 10 ^ { - 3 } } { 50 \times 10 ^ { - 3 } \times 1.25 \times 10 ^ { - 3 } }$ = $\frac { 1000 } { 1.25 }$ = 800