Asked by Monte;

a. How many moles of Na2Co3 were present in the 15mL sample?
b. How many grams of Na2CO3 were present in the 15mL sample?
c.How many grams of Na2CO3 are present in the 575L of the Na2CO3 solution?
Answered by DrBob222
See my response below. I assume you have a molarity somewhere in the problem but we can't help if you don't tell us more about the problem.
Answered by Monte;
This is a Lab Report on Stoichiometry and Gravimetric Analysis.
I have a balance equation for the reaction. Na2Co3+ CaCl2--> CaCo3+ 2NaCl. (CHALK)
I think I know the Precipitate: Na2Co3 and CaCl2
- Calulate the dry precipitate and the mole of the precipitate produced in the reaction? (I Don't Understand)
I don't know the Empirical Formula.

Answered by DrBob222
That information helps a little but not enough to help you much. CaCO3 is the precipitate. All three of the other reagents are soluble. Usually in an analysis like this, you are given a mass of the precipitate, in this case CaCO3, and asked to calculate mols and percent Na2CO3. You have the empirical formulas of all four reagents listed correctly.
Answered by Monte;
Thanx for the Help
Answered by Monte;
Quick Question what is the dry Precipitate?
Answered by DrBob222
The dry ppt is the CaCO3 after it has been dried, usually in an oven. You probably weighed the dry ppt and you have a mass for it.
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