Question

Nitric acid, $\mathrm{HNO}_{3},$ is available commercially at a concentration of $16 M$. (a) What volume would you need to obtain $0.150 \mathrm{~mol}$ $\mathrm{HNO}_{3} ?$ (b) To what volume must you dilute this volume of $\mathrm{HNO}_{3}$ from part (a) to prepare a $0.20 \mathrm{M}$ solution?

Name: Problem 87, Chapter 9: Fundamentals of General, Organic, and Biological Chemistry
Uploaded: 2022-01-13T18:35:55-08:00
Duration: 2 min 24 s
Channel: John Nicolle
Description: Nitric acid, HNO3, is available commercially at a concentration of 16 M. (a) What volume would you need to obtain 0.150 mol HNO3 ? (b) To what volume must you dilute this volume of HNO3 from part (a) to prepare a 0.20 M solution?

   Nitric acid, $\mathrm{HNO}_{3},$ is available commercially at a concentration of $16 M$.
(a) What volume would you need to obtain $0.150 \mathrm{~mol}$ $\mathrm{HNO}_{3} ?$
(b) To what volume must you dilute this volume of $\mathrm{HNO}_{3}$ from part (a) to prepare a $0.20 \mathrm{M}$ solution?

Fundamentals of General, Organic, and Biological Chemistry

John McMurry, David… 1st Edition

Chapter 9, Problem 87

Instant Answer

Solved by Expert John Nicolle

01/13/2022

Step 1

We need to find the volume that contains $0.150 \mathrm{~mol}$ of $\mathrm{HNO}_{3}$. We can use the formula for molarity which is moles of solute divided by liters of solution. Rearranging this formula to find the volume, we get: \[ V = \frac{n}{M} \] where: - Show more…

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Nitric acid, $\mathrm{HNO}_{3},$ is available commercially at a concentration of $16 M$. (a) What volume would you need to obtain $0.150 \mathrm{~mol}$ $\mathrm{HNO}_{3} ?$ (b) To what volume must you dilute this volume of $\mathrm{HNO}_{3}$ from part (a) to prepare a $0.20 \mathrm{M}$ solution?

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Key Concepts

Dilution Calculations

Dilution calculations use the principle that the number of moles of solute remains constant when a solution is diluted. This is represented by the equation C1V1 = C2V2, which allows one to find the new volume needed to achieve a desired lower concentration by adding solvent.

Molarity

Molarity is defined as the number of moles of solute per liter of solution. This concept is crucial in chemistry for quantifying how concentrated a solution is and is used to determine the volume needed to achieve a desired amount of solute.

Moles-to-Volume Conversion

This concept involves rearranging the molarity formula (moles = molarity × volume) to calculate the volume required to get a specific number of moles of solute. It is essential for accurate solution preparation from a concentrated stock solution.

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