The molal elevation constant of water =0.52 K m -1. The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

Question

The molal elevation constant of water =0.52 K m -1. The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be (A) 100.52° C (B) 101.04° C (C) 99.48° C (D) 98.96° C

Tardigrade Admin · Accepted Answer

Δ T b =K b × m=0.52 × 1 × 2=1.04 ∴ T b =100+1.04=101.04° C

Q. The molal elevation constant of water $= 0.52 K m^{- 1}$ . The boiling point of $1.0$ molal aqueous $K Cl$ solution (assuming complete dissociation of $K Cl$ ) should be

$100.5 2^{\circ} C$

$101.0 4^{\circ} C$

$99.4 8^{\circ} C$

$98.9 6^{\circ} C$

$Δ T_{b} = K_{b} \times m = 0.52 \times 1 \times 2 = 1.04$
$∴ T_{b} = 100 + 1.04 = 101.0 4^{\circ} C$

Q. The molal elevation constant of water =0.52Km−1. The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

100.52∘C

101.04∘C

99.48∘C

98.96∘C