A 48.8-mL sample of a 7.8 M KNO3 solution is diluted to 1.20 L .
1.What volume of the diluted solution contains 10.0 g of KNO3? (Hint: Figure out the concentration of the diluted solution first.)Express your answer using two significant figures.
2. To what volume should you dilute 130 mL of an 8.00 M CuCl2 solution so that 50.0 mL of the diluted solution contains 5.7 g CuCl2?
Express your answer using two significant figures.
dilute solution concentrated solution
M1 = M2 = 7.8M
V1 = 1.2L = 1200ml V2 = 48.8ml
M1V1 = M2V2
M1 = M2V2/V1
= 7.8*48.8/1200
= 0.3172M
no of moles of KNO3 = W/G.M.Wt
= 10/101 = 0.099 moles
molarity = no of moles/volume in L
0.3172 = 0.099/volume in L
volume in L = 0.099/0.3172 = 0.31L
volume of KNO3 = 310ml
part-B
no of moles of CuCl2 = W/G.m.Wt
= 5.7/134.452 = 0.0424moles
molarity = no of moles/volume in L
= 0.0424/0.05 = 0.848M
diluted solution concentrated solution
M1 = 0.848M M2 = 8M
V1 = V2 = 130ml
M1V1 = M2V2
V1 = M2V2/M1
= 8*130/0.848
= 1226.4ml
= 1.2*10^3ml >>>>answer
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