# Chemistry

posted by Kevin

Show the calculation for the limiting reagent when 0.853g of sodium sulfate (95% pure) react with 1.707g of barium hydroxide octahydrate (87% pure) to produce a precipitate of barium sulfate.

I've determined the equation is Na2SO4+Ba(OH)2*8H2O=BaSO4+2NaOH

However, that is unbalanced and I'm not sure how to balance the equation with the hydrated compound.

What would the first steps be to balance each side?

1. DrBob222

You have it balanced except for the 8H2O. Just add 8H2O on the end.

Na2SO4+Ba(OH)2*8H2O=BaSO4+2NaOH + 8H2O
g Na2SO4 = 0.853 x 0.95 = ?
g Ba(OH)2*8H2O = 1.707 x 0.87 = ?

Convert to mols.
mols Na2SO4 = grams/molar mass = ?
mols Ba(OH)2*8H2O = grams/mola mass = ?

Using the coefficients in the balanced equation, convert mols Na2SO4 to mols either BaSO4 or NaOH.
Do the same and convert mols Ba(OH)2*8H2O to mols BaSO4 or NaOH (but use the same product for both calculations).It is likely that the two values will not agree; the correct value in limiting reagent problem is ALWAYS the smaller value and the reagent responsible for that is the limiting reagent.

## Similar Questions

1. ### AP Chem

A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4. How many grams of barium ion are in a 458-mg sample of the barium compound if a solution …
2. ### chemistry

1) All of the following are oxidation-reduction reactions except (a) 2Al(s) + Fe2O3(s) ¨A12O3(s) + 2Fe(s) (b) (NH4)2Cr2O7(s) ¨ Cr2O3(s) + N2(g) + H2O(1) (c) Cu(s) + 2H2SO4(aq) ¨ CuSO4(aq) + SO2(g) + 2H2O(1) (d) Hg(NO3)2 + …
3. ### Chemistry

Assuming the sample is pure sodium sulfate, how many mL of 5% BaCl2.2H20 solution would be required to precipitate the sulfate. Density of barium shloride solution of 1.00 g/mL.
4. ### Chemistry

you add excess sodium sulfate to a solution of a soluble barium compound in order to precipitate all of the barium ion as barium sulfate, BaSO4. Suppose a 458 mg sample of the barium compound is dissolved to create the solution. Then …
5. ### Chemistry

you add excess sodium sulfate to a solution of a soluble barium compound in order to precipitate all of the barium ion as barium sulfate, BaSO4. Suppose a 458 mg sample of the barium compound is dissolved to create the solution. Then …
6. ### Chemistry

A limiting reactants problem. 6.32g of sodium sulfate is reacted with 12.03g of barium nitrate. How many grams of the precipitate would you expect to collect. The answer my teacher gave me is 16.0g BaSO4, but I cannot get it. The equation …
7. ### chemistry

in a particular experiment, 150.0 g of ammonium chloride were reacted with 290.0 g of barium hydroxide octahydrate, producing 157.2 g of water 1. find the limiting reagent in this situation 2. calculate the theoretical yield of water …
8. ### Chemistry

From the equation below, how many grams of barium sulfate can be produced from 20.8 g of barium chloride?
9. ### chemistry

Aqueous sodium sulfate reacts with aqueous barium chloride to produce solid barium sulfate and aqueous sodium chloride. the solution contains 3.44g of barium chloride. you have a 0.282M solution of sodium sulfate. determine the volume …
10. ### Chemistry

The sulfate in a 0.2345 g sample of a mixture containing only K2SO4 (fm = 174.26) and Na2SO4 (fm = 142.04) is to beanalyzed by precipitating all the sulfate as barium sulfate, BaSO4 (fm = 233.39) by the addition of excess BaCl2. Na2SO4 …

More Similar Questions