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.

Question

Chemistry

Mattie Lang

11 October, 08:14

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.

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Elijah Garcia · 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