An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at −1.83°C. The freezing point depression constant for water is 1.86°C/m.

Molality for this solution is 0.98 mol/kg

Explanation:

ΔT = Kf . m . i

Freezing point depression, here

ΔT =  Freezing point of pure solvent - Freezing point of solution

i = Van't Hoff factor.

This solute, the amino acid glycine does not ionize, so the i in this case is 1

Let's replace the data given

0° - (-1.83°C) = 1.86 °C/m . m . 1

1.83°C =  1.86 °C/m . m . 1

1.83°C / 1.86 m/°C = 0.98 m

14 days is the half-life of phosphorus-32

2b2t

explanation:

2b2t