Suppose you wish to make 0.879 l of 0.250 m silver nitrate by diluting a stock solution of 0.675 m silver nitrate. how many milliliters of the stock solution would you need to use?

Question

Barclay

Chemistry

2 March, 15:58

Suppose you wish to make 0.879 l of 0.250 m silver nitrate by diluting a stock solution of 0.675 m silver nitrate. how many milliliters of the stock solution would you need to use?

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Answers (1)

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Edith · Answer 1

Answer is: 325.5 mL of the stock solution.

c₁ (AgNO₃) = 0.675 M.

V ₂ (AgNO₃) = 0.879 L.

c ₂ (AgNO₃) = 0.250 M.

V ₁ (AgNO₃) = ?

c ₁ - original concentration of the solution, before it gets diluted.

c ₂ - final concentration of the solution, after dilution.

V ₁ - volume to be diluted.

V ₂ - final volume after dilution.

c ₁ · V₁ = c₂ · V₂.

V ₁ (AgNO₃) = c₂ · V₂ : c₁.

V ₁ (AgNO₃) = 0.250 M · 0.879 L : 0.675 M.

V ₁ (AgNO₃) = 0.325 L · 1000 mL = 325 mL.