Question

If the DCP solution is 0.01538M and you need 24.39 mLs of the DCP solution to completely react with the ascorbic acid, how many grams of ascorbic acid are in your sample? Do not write the answer in scientific notation. Make sure you use the correct number of significant figures and the correct units.

Answer 1

we know that

moles = molarity x volume (L)

given

molarity = 0.01538

volume = 24.39 ml

we know that

1 ml = 10-3 L

so

volume = 24.39 x 10-3 L

now

moles of DCP = 0.01538 x 24.39 x 10-3

moles of DCP = 3.751182 x 10-4

now

we know that

1 mole of ascorbic acid reacts with 1 mole of DCP

the reaction is

ascorbic acid + DCP --> products

we can see that

moles of ascorbic acid = moles of DCP taken

so

moles of ascorbic acid = 3.751182 x 10-4

now

we know that

mass = moles x molar mass

so

mass of ascorbic acid = 3.751182 x 10-4 x 176

mass of ascorbic acid = 0.066

so

0.066 grams of ascorbic acid is present in the sample