1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 ?

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Q. A saturated solution of iodine in water is $1.25 \times 10^{-3} (M)$. In any saturated solution of $I_{2}$ concentration of $I_{2}$ is $1.25 \times 10^{-3}( M ) .$ In $1 \,L$ of $0.1( M )$ solution $I ^{-},$ it is seen that $51.25 \times 10^{-3} mol$ of $I _{2}$ can be dissolved maximum. In the aqueous solution of $I^{-}(a q), I_{2}(a q)$ undergoes complex formation, $I _{2}( aq )+ I^{-} \xrightleftharpoons{K_{C}} I _{3}( aq )$.
What is the value of $K_{C}$ ?

Equilibrium

Solution:

image
$K_{C}=\frac{50 \times 10^{-3}}{50 \times 10^{-3} \times 1.25 \times 10^{-3}}$
$=\frac{1000}{1.25}=800$