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A) How many milliliters of a stock solution of 5.20 M HNO₃ would you have to use to prepare 0.160 L of 0.550 M HNO₃?

B) If you dilute 20.0 mL of the stock solution to a final volume of 0.330 L , what will be the concentration of the diluted solution?

User Lucuma
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1 Answer

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Final answer:

To prepare 0.160 L of 0.550 M HNO₃ from a 5.20 M stock solution, you need 17 mL of the stock solution. When diluting 20.0 mL of this stock to a final volume of 0.330 L, the final concentration is 0.315 M.

Step-by-step explanation:

The calculation of the volume of a stock solution required to make a diluted solution, and the determination of the final concentration after dilution, can be accomplished using the dilution equation M1V1 = M2V2, where M1 and M2 are the molarities of the stock and diluted solutions, respectively, and V1 and V2 are the volumes.

A) To prepare 0.160 L of 0.550 M HNO₃ from a 5.20 M stock solution, you would use the following calculation:

(5.20 M)(V1) = (0.550 M)(0.160 L)

V1 = (0.550 M × 0.160 L) / 5.20 M

V1 = 0.017 L or 17 mL of the stock solution.

B) If you dilute 20.0 mL of the stock solution to a final volume of 0.330 L, the final concentration would be:

(5.20 M × 20.0 mL) / 330 mL

Concentration = 0.315 M after the dilution.

User Rafael Piccolo
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