Question

A beverage contains tartaric acid, H2C4H4O6, a substance obtained from grapes during wine making. If the beverage is 0.190 tartaric acid, what is the molal concentration? What is the mole fraction of tartaric acid and water? Calculate the mass percent of tartaric acid. The density of the solution is 1.016g/mL.

Answer 1

1)
`molality = 0.19`

2)
`Mole\ fraction= 0.003486`

3)
`Mass\ percent = 2.8%`

Step-by-step explanation:

Concentration of Tartaric acid=0.190mole /l

1)

Generally

`Mass\ of\ tartaric\ acid = 150.087 *0.190`

`Mass\ of\ tartaric\ acid = 28.5 g`

Since 1L of solution tartartic acid is

`T_(1l)= density * volume`

`T_(1l)= 1.016Kg / L X 1 L`

`T_(1l)= 1016`

Therefore

`Mass of solvent = 1016-28.5`

`Mass of solvent = 987.5 g`

Generally the equation for molality is mathematically given by

`molality = (moles)/(Kg)`

`molality = (0.190 * 1000)/(987.5)`

`molality = 0.19`

2.

Generally the equation for Moles of water is mathematically given by

`Moles\ of\ water = (mass)/(mol wt)`

`Moles\ of\ water = (987.5)/(18 )`

`Moles\ of\ water= 54.86`

Therefore

`Mole\ fraction = (Moles\ of\ solute)/(total\ moles)`

`Mole\ fraction= (0.190)/(54.5)`

`Mole\ fraction= 0.003486`

3

Generally the equation for Mass Percent is mathematically given by

`Mass\ percent = (mass\ of\ tartaric\ acid)/(total mass)`

`Mass\ percent = (28.5* 100)/(1016)`

`Mass\ percent = 2.8%`