A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in...
- A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in a 100.0-mL volumetric flask and diluting to the mark with water. A standard solution was then prepared by transferring 2.00 mL of the stock solution to a second 25.00-mL volumetric flask and diluting to the mark.
- What is the concentration (in M) of Cu2+(aq)in the stock solution?
- What is the concentration (in M) of Cu2+(aq)in the standard solution?
Homework Answers
a)
Answer
0.03937M
Explanation
Molar mass of Cu(NO3)2.2.5H2O = 232.591g/mol
moles of Cu(NO3)2.2.5H2O = 0.9157g/232.591g/mol = 0.003937mol
molarity is defined as number of moles of solute dissolved per liter of solution
concentration of Cu2+ = ( 0.003937mol/100ml)× 1000ml = 0.03937M
b)
Answer
0.003150M
Explanation
Dilution formula
C1 × V1 = C2 × V2
C1 = initial solution concentration, 0.03937M
V1 = Initial solution volume, 2.00mL
C2 = Final solution concentration, ?
V2 = Final solution volume, 25.00mL
C2 = C1×V1/V2
= 0.03937M × 2.00mL/25.00mL
= 0.003150M
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