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Ch.13 - Properties of Solutions
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.13 - Properties of SolutionsProblema 54a
Capitolo 13, Problema 54a

Describe how you would prepare each of the following aqueous solutions from water and the solid solute: a. 1.50 L of 0.110 M (NH4)2SO4 solution;

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1
Determine the molar mass of \((NH_4)_2SO_4\) by adding the atomic masses of all atoms in the formula.
Calculate the number of moles of \((NH_4)_2SO_4\) needed using the formula: \(\text{moles} = \text{molarity} \times \text{volume in liters}\).
Convert the moles of \((NH_4)_2SO_4\) to grams using the molar mass calculated in step 1.
Weigh the calculated mass of \((NH_4)_2SO_4\) using a balance.
Dissolve the weighed \((NH_4)_2SO_4\) in a volume of water less than 1.50 L, then dilute the solution to a final volume of 1.50 L in a volumetric flask.

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Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for preparing solutions, as it allows chemists to quantify how much solute is needed to achieve a desired concentration in a given volume of solvent. For example, a 0.110 M solution of (NH4)2SO4 means there are 0.110 moles of ammonium sulfate in every liter of solution.
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01:13
Molarity

Dilution

Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. Understanding dilution is essential when preparing solutions, as it helps in calculating the amount of solute needed to achieve a specific molarity. The dilution formula, M1V1 = M2V2, relates the initial and final concentrations and volumes, guiding the preparation process.
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00:58
Dilution Equation

Solubility

Solubility refers to the maximum amount of solute that can dissolve in a solvent at a given temperature and pressure. It is important to know the solubility of (NH4)2SO4 when preparing the solution to ensure that the solute can fully dissolve in the solvent without forming a precipitate. This concept helps in determining whether the desired concentration can be achieved with the available solute.
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00:28
Solubility Rules
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