Homework Help: Chemistry

Posted by Mika on Saturday, October 8, 2011 at 8:03pm.

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.

Chemistry - DrBob222, Saturday, October 8, 2011 at 9:16pm
That all depends upon how much of the Na2SO4 is involved. moles Na2SO4 = grams/molar mass

Determine the M of the BaCl2.2H2O soln. 5% means you have 5.0 g BaCl2.2H2O/100 mL. moles = grams/molar mass; then M BaCl2.2H2O = moles BaCl2.2H2O/0.1L = ?M.

Write the equation and convert moles Na2SO4 to moles BaCl2.2H2O. Then
M BaCl2.2H2O = moles Ba^2+ required/L soln and solve for L.

Answer this Question

Related Questions

Chemistry - Recently I solved for how many mL of 5% BaCl2.2H20 solution was ...
chemistry - how many mL of 5% BaCl2 X(multiplied) 2H2O are needed for 0.3500g ...
Chemistry - you add excess sodium sulfate to a solution of a soluble barium ...
Chemistry - you add excess sodium sulfate to a solution of a soluble barium ...
chemistry - 1. 15.0 g of sodium sulfate are dissolved in water to form 400.0 g ...
Chemistry - Silver(I) nitrate and sodium sulfate react to form silver(I) sulfate...
Chemistry please help! - Please help. I have no idea how to do these 4 homework ...
chem. - Silver(I) nitrate and sodium sulfate react to form silver(I) sulfate and...
chemistry - how much of a 1.50M solution sodium sulfate solution in milliliters ...
Chemistry - A 12 mL sample of 0.4 M silver nitrate solution is mixed with 8 mL ...

For Further Reading

First Name:
School Subject:
Answer: