Question

KBr is 80% ionized in solution. The freezing point of 0.4 molal solution of KBr is :
$K_f(H_2O) = 1.86 \frac{K kg}{mole}$
(a) 274.339 K
(b) – 1.339 K
(c) 257.3 K
(d) – 1.339°C

Answer 1

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KBr is 80% ionized in solution. The freezing point of 0.4 molal solution of KBr is :
$K_f(H_2O) = 1.86 \frac{K kg}{mole}$
(a) 274.339 K
(b) – 1.339 K
(c) 257.3 K
(d) – 1.339°C

→ [B]


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Answer 2

Answer :

KBr is 80% ionized in solution. The freezing point of 0.4 molal solution of KBr is :  

K_f(H_2O) = 1.86 \frac{K kg}{mole}

(a) 274.339 K  

(b) – 1.339 K

(c) 257.3 K  

(d) – 1.339°C

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The correct option is (B) : -1339 K

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