Chlorides in mg/L from AgNO3 titration...?

Question

If I use a 1mL sample diluted with DI water, add three drops of Potassium Chromate, then titrate with 0.282 N AgNO3 to a rusty red color. How do I calculate mg/L Chlorides from my sample volume and particular normality titrant? I hope someone understands this question....

Answer 1

You can calculate this however you need more information. The milliliters of silver nitrate would be helpful. One you have that here is what you do:

the balanced equation is

AgNO3 + Cl- >> AgCl + NO3-
Note what is bonded to the nitrate group depends on what is bonded to the Cl- initially.

You would take the mL of silver nitrate and multiply it times the normaility and that will give you moles of silver nitrate titrated. In this case normal or equivalents=molar so use the mole to mole ratio(1 to 1) and obtain moles of Cl- in the initial sample. Use the molecular weight of chloride(35.45) and obtain grams of chloride. Then convert it to milligrams and then divide it by 0.001 and you will get mg/L.

Answer 2

I understand the question. It came from a text book. You did not master the subject matter and need to get an assignment done and hope someone will do your homework for you.

Here are the needed hints

1. At the equivalence point, the equivalents of titrant = equivalents of sample - this is the critical info and what you do not seem to understand; the equivalence point is where titrant and sample are equal.
2. equivalents of titrant in meq = titrant normality x ml titrant used. (0.282 * ml used which you did not specify)
3.the meq of the sample = 0.282 * ml titrant / 1 ml (volume of sample.

Answer 3

You're a tard! Hey, my new phone number is 479-601-4243.

C'mon Eric... you can do it!!