Question

The solubility of aspirin in water is 1 g per 300 mL at 25 degrees celsius. Assuming that your crystallization and washing with water were done at this temperature, what weight of aspirin did you lose in the filtrate and washings? How much was your percent yield lowered by this loss?

Answer 1

The weight of aspirin lost is
`W =0.03267(V_A +V_B) N`

The percent yield is lowered by
`A = (Amount \ of \ aspirin \ obtained - Lost Amount )/(Expected\ Amount\ of \ Aspirin ) *(100)/(1)`

Step-by-step explanation:

From the question we are told that

Since the solubility of aspirin in water is 1 g per 300 mL it implies that after crystallization the solution would contain 1 g for every 300mL of water at 25°

Let assume that the volume of the solution is
`V_A`

The the aspirin lost after filtration would be

`= (1)/(300) * V_A`

`=(V_A)/(300)g`

Let assume that you used water of volume
`V_B` to wash the crystallized aspirin then the lost during washing would be

`= (1)/(300) * V_B`

`= (V_B)/(300)`

So the total loss is

`= (V_A)/(300) + (V_B)/(300)`

`(V_A +V_B)/(300)g`

So the weight of aspirin lost denoted by W is

`W = (V_A +V_B)/(300) *9.8`

`W =0.03267(V_A +V_B) N`

Let denote How much was your percent yield lowered by this loss by A

So

`A = (Amount \ of \ aspirin \ obtained - Lost Amount )/(Expected\ Amount\ of \ Aspirin ) *(100)/(1)`