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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblema 59
Capitolo 4, Problema 59

A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

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1
Calculate the number of moles of NaNO_3 needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume in liters} \). Convert 400.0 mL to liters by dividing by 1000.
Use the molarity (1.1 M) and the volume in liters from Step 1 to find the moles of NaNO_3.
Determine the molar mass of NaNO_3 by adding the atomic masses of Na, N, and O (Na: 22.99 g/mol, N: 14.01 g/mol, O: 16.00 g/mol).
Calculate the mass of NaNO_3 needed using the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \).
Use the moles from Step 2 and the molar mass from Step 3 to find the mass of NaNO_3 in grams.

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Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L). In this question, a 1.1 M NaNO3 solution means there are 1.1 moles of sodium nitrate in every liter of the solution.
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Molarity Concept

Calculating Moles from Volume and Molarity

To find the number of moles of solute needed for a specific volume of solution, you can use the formula: moles = molarity × volume (in liters). For a 400.0 mL solution, you must convert the volume to liters (0.400 L) before applying this formula to determine the moles of NaNO3 required.
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Molar Mass Calculation Example

Molar Mass

The molar mass of a compound is the mass of one mole of that substance, typically expressed in grams per mole (g/mol). For NaNO3, the molar mass can be calculated by summing the atomic masses of sodium (Na), nitrogen (N), and three oxygen (O) atoms. This value is essential for converting moles of NaNO3 into grams.
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02:11
Molar Mass Concept
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