# An aqueous solution containing both Sr2+ and CO32– ions is mixed in order to precipitate SrCO3(s). Given there are 1.50 mL of 2.53 MSr2+ 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. Sr^2+(aq)+CO2^−3​(aq) --> SrCO3​(s) ____ g

Question

An aqueous solution containing both Sr2+ and CO32– ions is mixed in order to precipitate SrCO3(s). Given there are 1.50 mL of 2.53 MSr2+ 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.

Sr^2+(aq)+CO2^−3​(aq) --> SrCO3​(s)

____ g