
Interpretation:
Volume of 5.0 M H2SO4 stock solutionis to be calculated to prepare 100 mL of 0.25 M H2SO4 solution.
Concept introduction:
In dilution, the amount of solute does not change, the number of moles is the same before and after dilution.
If subscript "1" represents initial and "2" represents the final values of the quantities involved, we have:
Here, molarity is used as a unit of concentration.
The equation for dilution is
Where
M1 = molarity of the stock solution
V1 = volume of stock solution
M2 = molarity of the diluted solution
V2 = volume of diluted solution

Answer to Problem 25PP
5 mL of 5.0 M H2SO4 stock solutionis required to prepare 100 mL of 0.25 M H2SO4 solution.
Given information:
The molarity of the stock solution M1 = 5.0 M
The molarity of the diluted solution M2 = 0.25 M
The volume of diluted solution V2 = 100 mL
Explanation:
The equation for dilution is
Where
M1 = molarity of the stock solution
V1 = volume of stock solution
M2 = molarity of the diluted solution
V2 = volume of diluted solution
V1 = volume of stock
Thus, 5 mL of 5.0 M H2SO4 stock solutionis required to prepare 100 mL of 0.25 M
Explanation of Solution
Given information:
The molarity of the stock solution M1 = 5.0 M
The molarity of the diluted solution M2 = 0.25 M
The volume of diluted solution V2 = 100 mL
The equation for dilution is
Where
M1 = molarity of the stock solution
V1 = volume of stock solution
M2 = molarity of the diluted solution
V2 = volume of diluted solution
V1 = volume of stock
Thus, 5 mL of 5.0 M H2SO4 stock solutionis required to prepare 100 mL of 0.25 M
Chapter 14 Solutions
Glencoe Chemistry: Matter and Change, Student Edition
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