A solution is prepared by adding 45.0g of Na2SO4*6H2O to pure water to make 150mL of solution. What are molar concentrations of these ions in the resulting solution?

Sodium Ion? Sulfate Ion? Phosphate Ion?

I've determined the solution is 1.2M
45/250.16g/mol Na2SO4*6H2O = .180 mol

.180 mol Na2SO4*6H2O/.150 L=1.2M

Where do I go now?

1 answer

You've done the hard part.
(Na2SO4.6H2O) = 1.2 M.
Now there is 1 sulfate/1 Na2SO4 so (SO4^2-) must the same as (Na2SO4). Right? Right.

Now there are 2 Na/1 Na2SO4 so (Na^+) = 2 x (Na2SO4) = 2*1.2 = 2.4. Right?
Similar Questions
  1. I need help starting this question:A buffer solution is prepared by adding 30.0g of pure acetic acid to 41.0g of sodium acetate
    1. answers icon 0 answers
  2. I need help starting this question...A buffer solution is prepared by adding 30.0g of pure acetic acid to 41.0g of sodium
    1. answers icon 1 answer
    1. answers icon 1 answer
    1. answers icon 1 answer
more similar questions