the reaction is: CaCl 2 (aq) + Na 2 CO 3 (aq) ? CaCO 3 (s) + 2NaCl(aq) Mass Gram
ID: 705813 • Letter: T
Question
the reaction is: CaCl2(aq) + Na2CO3(aq) ? CaCO3(s) + 2NaCl(aq)
Mass Grams Mass of CaCl Mass of Na2CO Mass of Filter Paper Mass of Product, CaCO3 (Experimental Yield) Experimental Observations 2 gm 2.5 gm 2.3 gm 2.4 gm 1. What is the proper name of CaCO? When is it used in real life? 2. What happened to the excess reactant after the reaction was complete? 3. What was the limiting reagent in your experiment? Show your calculations that prove this. 4. What was the theoretical yield of CaCO? Show your calculations. 5. What was your experimental yield of CaCO2 (from Table 9)? 6. Use the following equation to find your percent yield of CaCO. Show your calculations. Experimental Yield of Prodiu Theoretical Yield of Product Percent Yield 7- lf your percent yield was not 100% (ie., it was above or below), discuss some potential sources of error that may have caused your increased or decreased yield. 8. Would there have been any effect on your experiment if tap water containing calcium ions was used instead of deionized water to dissolve the reactants. Explain.Explanation / Answer
1. Calcium carbonate, also called lime stone. In daily life used in the form of lime coating to walls and as marble stones.
5. 2.4grams
8. If tap water is used then more carbonate is required because tap water has carbonates and bicarbonate of calcium and magnesium. So hard water if used, calcium ions in the water combines with sodium carbonate and thereby excess amounts of sodium carbonate is added.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.