# Problem: Toilet bowl cleaners often contain hydrochloric acid to dissolve the calcium carbonate deposits that accumulate within a toilet bowl.What mass of calcium carbonate (in grams) can be dissolved by 3.9 g of HCl? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)

###### FREE Expert Solution
• First thing is to setup the balanced reaction and then use stoichiometry to get the mass of CaCO3. We will need the molar masses of HCl and CaCOfor that.
• Reaction appears to be a double displacement reaction where counter ions are being switched
• HCl (hydrochloric acid) and CaCO3 (calcium carbonate) dissociates as Hand Cl-, Ca2+ and CO32-
• Products will appear as H2CO3 (from Hand CO32-) and CaCl2 (from Ca2+ and Cl-)
• H2CO3 will spontaneously transform to H2O (l) + CO(g) THIS IS A GAS EVOLUTION REACTION.
• CaCl2 will appear as aqueous species acc. to the solubility rules. All chlorides (Cl- ) are soluble except AgCl, Hg2Cl2 , and PbClwhich are insoluble.
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###### Problem Details

Toilet bowl cleaners often contain hydrochloric acid to dissolve the calcium carbonate deposits that accumulate within a toilet bowl.

What mass of calcium carbonate (in grams) can be dissolved by 3.9 g of HCl? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)