What is value of the depression of freezing point of the resulting solution if 0.1M KI and 0.2 M AgNO3 are mixed in 3: 1 volume ratio? [Kf= 1.86 K kg mol-1]

Question

What is value of the depression of freezing point of the resulting solution if 0.1M KI and 0.2 M AgNO3 are mixed in 3: 1 volume ratio? [Kf= 1.86 K kg mol-1] (A) 3.72 K (B) 1.86 K (C) 0.93 K (D) 0.279 K

Tardigrade Admin · Accepted Answer

(Kl)aq+(AgNO)3 (aq) arrow (AgI)s downarrow+(KNO)3 (aq) Kl+AgNO3 arrow KNO3+AgI downarrow <img class="img-fluid question-image" alt="Solution" src="https://cdn.tardigrade.in/q/nta/c-kni5j38cbni3lvvi.jpg" /> Total moles of solute ions =(0 .1 + 0 .2)× 2(∵ i = 2) [Solute] =(0 .6/M)M Δ Tf=Kf.(0 .6/4)=1.86× (0 .6/4)=0.279 K

Q. What is value of the depression of freezing point of the resulting solution if 0.1M KI and 0.2 M AgNO₃ are mixed in 3 : 1 volume ratio? [K_f= 1.86 K kg mol^-1]

3.72 K

1.86 K

0.93 K

0.279 K

$(K l)_{a q} + (A g NO)_{3 (a q)} \to (A g I)_{s} ↓ + (K NO)_{3 (a q)}$
$K l + A g N O_{3} \to K N O_{3} + A g I ↓$

Total moles of solute ions $= (0.1 + 0.2) \times 2 (∵ i = 2)$
[Solute] $= \frac{0.6}{M} M Δ T_{f} = K_{f} . \frac{0.6}{4} = 1.86 \times \frac{0.6}{4} = 0.279 K$

Q. What is value of the depression of freezing point of the resulting solution if 0.1M KI and 0.2 M AgNO3 are mixed in 3 : 1 volume ratio? [Kf= 1.86 K kg mol-1]