Question

In: Chemistry

Consider the solution formed from dissolving 11.20 ml of methylene chloride, CH2Cl2 (Mm=85.0g/mol, Density=1.33g/ml; non-electrolyte) into...

Consider the solution formed from dissolving 11.20 ml of methylene chloride, CH2Cl2 (Mm=85.0g/mol, Density=1.33g/ml; non-electrolyte) into 102.8 ml of carbon tetrachloride, CCl4 (Mm=154g/mol, density=1.59g/ml; non-electrolyte). Determine the molality and molarity of the resulting solution assuming additive volumes.

Expert Solution

volume of CH2Cl2 = 11.20 ml

density of CH2Cl2 = 1.33 g /ml

mass of CH2Cl2 = volume x density = 11.20 x 1.33 = 14.896 g

molar mass of CH2Cl2 = 85 g/mol

moles of CH2Cl2 (solute ) = mass / molar mass

= 14.896 / 85

= 0.175

total volume of solution = 102.8 + 11.20 = 114 ml = 0.114 L

molarity = moles of solute / volume of solution

= 0.175 / 0.114

= 1.54 M

molarity = 1.54 M

volume of solvent = 102.8 ml

density of solvent = 1.59 g /ml

mass of solvent = density x volume

= 1.59 x 102.8

= 163.45 g

= 0.16345 kg

molality = moles of solute / mass of solvent

= 0.175 / 0.16345

= 0.00107 m

molality = 0.00107 m

queen_honey_blossom answered 6 months ago

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