A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 53.60 mL of...
Homework Answers
= (0.08765mol/1000ml)*53.6ml
= 4.69804x10-3 mol
These moles are equal to the total number of mols of NaCl and KBr.
Let the percentage by mass for:
NaCl be X%
Therefore the % by mass for KBr becomes (100-X)%
Mol(NaCl) = mass of NaCl/Formula weight of NaCl
= (0.3146*X/100)/58.44
= 5.3833*10--5X
Mol(KBr) = mass of KBr/Formula weight of KBr
= (0.3146*(100-X)/100)/119.01
= 2.6435*10-5(100-X)
Since mol(NaCl) + mol(KBr) = mol(Ag+)
5.3833*10--5X + 2.6435*10-5(100-X) = 4.69804x10-3
2.7398*10--5X + 2.6435*10-3 = 4.69804x10-3
2.7398*10--5X = 2.05454*10-3
X = 74.99%
Therefore, the sample contains 74.99% and 25.01% of NaCl and KBr respectively
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A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 53.60 mL of...
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Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an excess of AgNO3 solution is added...
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A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution....
A 1.04 g sample of KBr is dissolved in water to give 155 mL of
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Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the
solution via precipitation as insoluble PbBr2(s).
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3. A 6.0 g sample that contains a mixture of CaCl2 and NaCl was dissolved in water, and the solution treated with sodium oxalate (Na2C204) to precipitate the calcium as calcium oxalate (CaC204). Suppose 3.50 g of calcium oxalate was isolated and recovered, what is the weight percent of NaCl in the original 6.0 g sample? + 2 NaCl (aq) CaCl2 (aq) + NaCl (aq) + Na2C2O4 (aq) NazC204 (aq) CaC204 (5) No reaction -
A 1.04 g sample of KBr is dissolved in water to give 155 mL of
solution. This solution is then added to 165 mL of 0.015 M aqueous
Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the
solution via precipitation as insoluble PbBr2(s).
The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq)
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molarity) of nitrate ions in the solution?
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