Benzaldehyde ( = 106.1 g/mol), also known as oil of almonds, is used in the manufacture of dyes and perfumes and in flavorings. what would be the freezing point of a solution prepared by dissolving 75.00 g of benzaldehyde in 850.0 g of ethanol? kf = 1.99°c/m, freezing point of pure ethanol = –117.3°c.

The question to your answer is: Tc = -118.97°C

Explanation:

data

MW Benzaldehyde = 106.1 g/mol

Tc = ?

Mass Benzaldehyde = 75 g

Mass ethanol = 850 g

Kf = 1.99

Freezing point of ethanol = -117.3°C

Formula

                -Tc + Tc (solvent) = Kcm

molality

            106.1 g 1 mol

              75 g    x

    x = 75 / 106.1 = 0.71 mol

molality = #moles / kg solvent = 0.71 / 0.85 = 0.84

Substitution

                     -Tc + Tc (solvent) = Kcm

                     -Tc -117.3 = (1.99)(0.84)

                     -Tc = 117.3 + 1.67

                    - Tc = 118.97°C

                       Tc = -118.97°C

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.