Question

Table 9: Mass Data Item Calcium Chloride (CaCl2) Sodium Carbonate (Na,CO3) Filter Paper Caco,(Experimental Yield) Weight of filter paper and CaCO3=3.9 Mass (6) 2.0 2.5 2.2 3.9-2.2=1.7 Experimental Observations: Insert Photo of precipitate: POST-LAB QUESTIONS (Show your work!) 1. Would there be any effect on an experiment if tap water containing calcium ions is used instead of deionized water to dissolve reactants? Explain your answer. 2. Balance the following chemical reaction. __Na2CO3 + _CaCl2 (aa) — CaCO3(s+_ Nac.(a) 3. What happened to the excess reactant after the reaction was complete? Use your data in table 9 and the balanced equation from question 2 to answer the remaining questions: 4. What is the limiting reagent? 5. What is the theoretical yield of CaCoz? 6. What is the experimental yield (actual yield) of CaCO,? 7. What is the percent yield of CaCo3 ?

Answer 1

Experimental Calcium and sodium compounds becamation: chlaude is Carbonate is soluble also ionic soluble compound lance Nadl cog) CaCO3 lag Calle reacts with Na Coz to give CaCO3 (insoluble compounds) and Nadl (sodium inic compounds). This kind of geaction is double displacement method .. #1) yes, IS tap water containing calcium ions is used to dissolve reactants , they will be effects on the chemical reaction that takes places are of the reactant species is calcium ions il we use top water containing calcium ions , it increases the inoles & calcium ions in a solution which geacts with carbonate can to give a Calcium carbonate

Ca y Whereas decorized water does not have any ions, so it does not give excess products due to interfaring ions is tap water #2) Balance the chemical reaction : Step 1. Identify the reactants and the products in the reaction and write down their formula Step 2: Write reactants on the left of the arrow and products on the right of the 000w Step 3: Count each elements separately the number of in reactants atoms of and products Naco + Reactant co) acer altrace (ppt) Product Na - 1 cal 0-3 o d-1

and A Step 4 chleaire atoms on both sides does not match, change the coefficients Nad to two to get balanced ! equations Na, Cos Cage + Cacha (ag) → Caloog Reactants Na - 2 Products Na - 2 C-1 C- a - 3 d-2 Ca- l-2 Balanced chemical equation: Na, CO3(aq) + Cachacag) - CaCO3(3) * + 2 Nad cog) #3) When the limiting reactant react completely with excess Icoctart to complete the / geaction. After the reactant was complete there other is no more reactant to react to give product. The excess reactant gemains because there is nothing to react with it

#4) Balanced chemical reaction Nas Coz (ag) + Cachlag) - CaCOo(s) + Nachos) One mole of Na co react with one se o cach to give one mole of CaCO₃ Mass Number molar mas Number of moles of Na, com les mas Mass of NaCO3 = 2.59 Molaa mass of NaCO3 = 105.99 g/mol Na co a23 105.998/mal n = 0.02359 mol Na coz Number of moles of Call = 2008 119.98 g/mol mol = 0.01802 mol Linching reactant is a geactant which consumers' completely 0.01202 mol of cad reacts with 0.01802 mol of Na co to produce 201802 mol of CaCO₃

Cache is a limiting reactant cohereas Na co is an excess reactant # 5) Theoretical 0.01802 nd of of NaCo to yield could cada reacts with produce 0.01802 mol of Cacoa Mass og Cacao - malo x mdar mass = 0.01802 mol x 100.09 g/mol Mass of Ca CO₂ = 1.80 g Theoretical yield of cocoa = 1-809 #6) Kacperimental yield (actuel yokes g cacoe- Actual yield = 1.7g. #y) Peacent yield of cacos Porcent vield - (Actual yield Theoretical yield) =( 170 ) x 100% 2 x 100% 1.8e - 0.9444 x 1007 Peacent yeld- 94%

#1) yes, tap water containing calcium ions interfere with the chemical reaction

#2) Na₂CO_3(aq) + CaCl_2(aq)  $\rightarrow$_​​​​ CaCO_3(s) + 2NaCl_(aq)

#3) the excess reactant remains because there is nothing to react with it.

#4) CaCl₂ is limiting reagents.

#5) Theoretical yield of CaCO₃ is 1.8g

#6) Actual yield of CaCO₃ is 1.7g

#7) Percent yield of CaCO₃ is 94%