An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at 272.813 K. If the value of Kf for water is 1.86 K/m, what is the molecular mass of the monobasic acid

Question

An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at 272.813 K. If the value of Kf for water is 1.86 K/m, what is the molecular mass of the monobasic acid (A) 50 g/mol (B) 46 g/mol (C) 55 g/mol (D) 60 g/mol

Tardigrade Admin · Accepted Answer

m=(Kf × w×1000/Δ Tf × W) =60 g /mole

Q. An aqueous solution of a weak monobasic acid containing $0.1 g$ in $21.7 g$ of water freezes at $272.813 K$ . If the value of $K_{f}$ for water is $1.86 K / m$ , what is the molecular mass of the monobasic acid

50 g/mol

46 g/mol

55 g/mol

60 g/mol

$m = \frac{K _{f} \times w \times 1000}{Δ T _{f} \times W}$
$= 60 g / m o l e$

Q. An aqueous solution of a weak monobasic acid containing 0.1g in 21.7g of water freezes at 272.813K. If the value of Kf​ for water is 1.86K/m, what is the molecular mass of the monobasic acid