Calculate the molality ( m ) of each solution (assumethe density of the solution

Question

Calculate the molality (m) of each solution (assumethe density of the solution is 1.0 g/mL). (a) 43.8 g of NaOHdissolved in enough water to form 0.526 Lof solution
____________ m

(b) 12.0 g ofC6H12O6 (dextrose) dissolved inenough water to form 0.264 L ofsolution
_____________ m

(c) 23.2 g of urea(NH2CONH2) dissolved in enough water to form106.0 mL of solution
______________ m
Calculate the molality (m) of each solution (assumethe density of the solution is 1.0 g/mL). (a) 43.8 g of NaOHdissolved in enough water to form 0.526 Lof solution
____________ m

(b) 12.0 g ofC6H12O6 (dextrose) dissolved inenough water to form 0.264 L ofsolution
_____________ m

(c) 23.2 g of urea(NH2CONH2) dissolved in enough water to form106.0 mL of solution
______________ m
(a) 43.8 g of NaOHdissolved in enough water to form 0.526 Lof solution
____________ m

(b) 12.0 g ofC6H12O6 (dextrose) dissolved inenough water to form 0.264 L ofsolution
_____________ m

(c) 23.2 g of urea(NH2CONH2) dissolved in enough water to form106.0 mL of solution
______________ m

Explanation / Answer

We Know that :         Molality = number of moles of the solute / weight ofsolvent ( Kg )                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                        =     43.8 g / 40 g / mole /   0.526 L x1000 Kg / m3                       = 0.00208 molal.           Molality = number of moles of the solute / weight ofsolvent ( Kg )                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                        = 12.0 g / 180 g / mole   / 0.264 L x 1.54 x1000 Kg / m3                         = 1.639 x 10-4 molal.             Molality = number of moles of the solute / weight ofsolvent ( Kg )                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                       = 23.2 g / 60 g / mole / 106.0ml x 1 g / ml * 1000                        = 3.6477 molal.                         = 1.639 x 10-4 molal.             Molality = number of moles of the solute / weight ofsolvent ( Kg )                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                       = 23.2 g / 60 g / mole / 106.0ml x 1 g / ml * 1000                        = 3.6477 molal.                        =   numberof moles of the solute   /   Volume of thesolution x density of the solution                       = 23.2 g / 60 g / mole / 106.0ml x 1 g / ml * 1000                        = 3.6477 molal.

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