Calculate the molalities of the following aqueous solutions: (a) 1.21 M sugar (C12H22011) solution (density of solution = 1.12 g/mL) (b) 0.849 M NaOH solution (density of solution 1.04 g/mL) (c) 5.31 M NaHCO3 solution (density of solution 1.19 g/mL)
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Calculate the molalities of the following aqueous solutions:
(a) 1.21 M sugar (C12H22O11) solution (density of solution =
1.12 g/mL)
m
(b) 0.849 M NaOH solution (density of solution 1.04 g/mL)
(c) 5.31 M NaHCO3 solution (density of solution 1.19 g/mL)
m](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc69086fd-bbea-40ca-86f1-ef6ae0a979b0%2Fc732c095-2341-4cc1-8d92-d6cd156f720d%2F4qztwi4_processed.png&w=3840&q=75)
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Molality = no. of moles of solute/Mass of solvent (kg)
Now, we have to calculate 'no. of moles of solute' & mass of solvent using given data.
(a) Given data = 1.21 M sugar solution having density is equals to 1.12 g/mL.
Now, let us assume that we have 1 L (1000 mL) of solution, then the no. of moles of sugar would be = 1.21
Because, Molarity = no. of moles of solute / volume of solution (L) |
Mass of solution = density * volume = 1.12 g/mL * 1000 mL = 1120 g
Now, mass of solute = no. of moles of solute * molar mass of solute = 1.21 mol * 342 g/mol = 413.82 g
Mass of solvent = mass of solution - mass of solute = 1120 g - 413.82 g = 706.18 g
Molality = no. of moles of solute / mass of solvent (kg) = (1.21 mol * 1000) / 706.18 g = 1.713 m (Approx.)
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