This is from a lab, so I\'ll try to provide the most information that I can. Sin

ID: 895801 • Letter: T

Question

This is from a lab, so I'll try to provide the most information that I can.

Since the standard is known to contain 0.50 % wt asorbic acid, multiply the mass weighed on the balance, and recorded by 0.0050. Don't forget to convert to mg. This will be the mass of the unknown acid. (The value should be in the range of 1-2mg)

The mass weighed on the balance was - 00.300 g

To solve this, the 00.300 g needs to be converted to mg, and then it needs to be multiplied by 0.005. I just don't know how to do that.

mass asorbic acid in standard = ? mg

------------------------------------------------------------------------------------------------------------------------------------------------------

Question 2 -

Using the number of drops of DCP for the standard (which was 17), the number of drops of DCP for the drink sample (which was 11), and the known mass of asorbic acid calculated in question 1 above, what is the mass of asorbic acid in the drink sample?

This calculation requires this equation - (mass vitaminC) unknown = (mass vitaminC) known X drops DCP unknown over (like a fraction)drops DCP known

mass asorbic acid in drink = ? mg

---------------------------------------------------------------------------------------------------------------------------------------------------

Question 3 -

Compute the mass of asorbic acid in juice sample using the mass of asorbic acid in the known, and the number of drops of DCP used for the known and for the Juice sample.

Mass asorbic acid in Juice = ? mg

Thanks so much for any help in advance!

Explanation / Answer

standard contains 0.3 gms =0.3*1000 mg = 300mg

the sample contains 0.5% ascorbic acid =300*0.5/100= 1.5mg

b) mass of ascorbic acid * number of drops of DCP= mass of ascorbic acid* number od drops of DCP in unknown sample

mass vitamin unknown = (mass vitamin known)*drop DCP unknown/ Drops DCP known

Mass vitamin =1.5* 11/17= 0.9705 mg

mass ascorbic acid in juice= 0.5*x/17 ( where x is th number of drops of DCP in unknown)

Navigate

This is from a lab experiment. The orange fruit that was used to produce the jui

This is from a lab. The dropped used to deliver drops of DCP only delivers whole

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.

This is from a lab, so I\'ll try to provide the most information that I can. Sin

Question

Explanation / Answer

Related Questions

Navigate