1. Will a precipitation reaction occur when the following aqueous solutions are
ID: 561778 • Letter: 1
Question
1. Will a precipitation reaction occur when the following aqueous solutions are mixed? (Answer yes or no.) If the answer is yes, identify the precipitate formed. REACTION? PRECIPITATE A. Na2CO3(aq) + Mg(NO3)2(aq) B. AICl3(aq) +KOH(aq) C. CuBr2(aq) + MgSO4(aq) Wri te a balanced molecular equation for any ONE precipitation reaction identified above. added to 5.0 mL of 0.50 M potassium phosphate? [You must first write the balanced chemical equation. Which reactant is present in excess? 2. Calculate the theoretical yield in grams of precipitate formed when 10.0 mL of 0.50 M magnesium nitrate isExplanation / Answer
1)
A)YES. a precipitate of MgCO3 is formed.
Mg(NO3)2(aq) + Na2CO3 (aq) ----------> 2NaNO3(aq) + MgCO3(s)
B)YES. A white gelatinous precipiate of AL(OH)3 is formed.
AlCl3 (aq)+ 3KOH (aq) -----------> Al(OH)3 (s) + 3KCl(aq)
C) NO
CuBr2(aq) + MgSO4(aq) -------------> No precipitation/reaction
2) 3 Mg(NO3)2(aq) + 2K3PO4 (aq) -------------> Mg3(PO4)2 (s) + 6 KNO3(aq)
10x 0.5=5 5x0.5 =2.5 0 0
[5/3 =1.67 2.5/2=1.25 as the ratio of Magenisium nitrate is less , it is the limiting reagent and ppotassium phosphate is the excess reagent]
When 3 moles of Mg(NO#)2 reacts one mole of Magensium phosphate is formed
3x148g of magnesium nitrate gives 1x 262 g of magnesium phosphate
5 x10-3 moles of magnesium nitrate gives = 5 x10-3 molx262 g/3mol
= 0.436g
the theoretical yield of magnesiu phosphate = 0.436g
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