Question

In: Chemistry

An aqueous solution of glycerin, 7% by weight, is prepared. The solution is found to have...

An aqueous solution of glycerin, 7% by weight, is prepared. The solution is found to have a density of 1.0149 g/mL. The density of pure glycerin (MW=92.0473) is 1.2609 g/mL. What is the molarity and molality concentration of the solution?

Solutions

Expert Solution

Solution :-

Lets assume we have 100 ml solution (0.100 L)

then mass of solution = volume * density

                                 = 100 ml * 1.0149 g per ml

                                 = 101.49 g

now lets find mass of glycerin

101.49 g * 7 % glycerin / 100 % = 7.1043 g

now lets calculate moles of glycerin

moles = mass / molar mass

moles of glycerin = 7.1043 g / 92.0473 g per mol

                            = 0.07718 mol glycerin

Now lets calculate the molarity

molarity = moles / volume in liter

             = 0.077181 mol / 0.100 L

            = 0.77181 M

now lets calculate the molality

molality = moles / kg solvent

mass of water = 101.49 g - 7.1043 g = 94.3857 g = 0.0943857 kg

molality = 0.7718 mol / 0.0943857 kg

             =0.81771 m


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