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?

The weight of aspirin lost is  

The percent yield is lowered by  

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

          The the aspirin lost after filtration would be

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

So the total loss is

So the weight of aspirin lost denoted by W is

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

    So

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g