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 that 51.25 × 10-3 mol of I 2 can be dissolved maximum. In the aqueous solution of I-(a q), I2(a q) undergoes complex formation, I 2( aq )+ I- xrightleftharpoonsKC I 3( aq ). What is the value of KC ?

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 that 51.25 × 10-3 mol of I 2 can be dissolved maximum. In the aqueous solution of I-(a q), I2(a q) undergoes complex formation, I 2( aq )+ I- xrightleftharpoonsKC I 3( aq ). What is the value of KC ? (A) 750 (B) 800 (C) (1000/51.25) (D) 1

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/d7c107cdd19517b525dc4d4fa7959406-.png" /> KC=(50 × 10-3/50 × 10-3 × 1.25 × 10-3) =(1000/1.25)=800

750

800

$\frac{1000}{51.25}$

1

$K_{C} = \frac{50 \times 1 0 ^{- 3}}{50 \times 1 0 ^{- 3} \times 1.25 \times 1 0 ^{- 3}}$
$= \frac{1000}{1.25} = 800$

750

800

51.251000​

1

KC​=50×10−3×1.25×10−350×10−3​ =1.251000​=800

$\frac{1000}{51.25}$

$K_{C} = \frac{50 \times 1 0 ^{- 3}}{50 \times 1 0 ^{- 3} \times 1.25 \times 1 0 ^{- 3}}$
$= \frac{1000}{1.25} = 800$