Question

An aqueous solution containing both Sr2+ and CO32– ions is mixed in order to precipitate SrCO3(s). given there are 1.40 mL of 2.53 M Sr2+ ions, calculate the mass of SrCO3 that is formed. assume that all of the Sr2+ ions are consumed. the net ionic reaction is shown below.

Answer 1

First, we calculate the number of moles of Sr2+ ions.

moles Sr = 2.53 M * 0.0014 L

moles Sr = 0.003542 mol

 

There is 1 mole of Sr for every mole of SrCO3, so the moles is equal.

moles SrCO3 = 0.003542 mol

 

The molar mass of SrCO3 is 147.63 g/mol, so the mass is:

mass SrCO3 = 0.003542 mol * 147.63 g/mol

mass SrCO3 = 0.523 grams