What is the boiling point of a solution that contains 3 moles of $K B r$ $KBr$ in 2000 g of water? ( $K_{b}$ $K_b$ = 0.512 C/m; molar mass of water = 18 g)?

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Answer 1 · 2018-04-20T15:26:35

$101.536 °C$ $"101.536 °C"$

When a solute is added in a solvent the boiling of solvent is elevated.

This elevation in boiling point ( $Delta"T"_b$ ) is given by the formula

$Δ"T" = i"K"_b"m"$

Where

Here solute is glucose & solvent is water.
Boiling point of pure water is $"100°C"$

$("T" - "100°C") = cancel"2" × "0.512°C/molal" × "3.00 mol"/(cancel"2.00" "kg")$

$"T = 100°C + 1.536°C = 101.536°C"$

What is the boiling point of a solution that contains 3 moles of KBrKBrKBr in 2000 g of water? (K_bKbK_b = 0.512 C/m; molar mass of water = 18 g)?