Describe how you would prepare each of the following aqueous solutions: (a) 1.50 L of 0.110 M 1NH422SO4 solution, starting with solid 1NH422SO4;

Verified step by step guidance

1. insert step 1> Calculate the number of moles of (NH_4)_2SO_4 needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume} \). Here, the molarity is 0.110 M and the volume is 1.50 L.
2. insert step 2> Determine the molar mass of (NH_4)_2SO_4 by adding the atomic masses of all the atoms in the formula: 2(N) + 8(H) + 1(S) + 4(O).
3. insert step 3> Convert the moles of (NH_4)_2SO_4 to grams using the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \).
4. insert step 4> Weigh the calculated mass of solid (NH_4)_2SO_4 using a balance.
5. insert step 5> Dissolve the weighed (NH_4)_2SO_4 in a small amount of distilled water, then transfer the solution to a 1.50 L volumetric flask and fill it with distilled water up to the mark to ensure the final volume is 1.50 L.

Key Concepts

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) and is crucial for preparing solutions accurately. To prepare a solution of a specific molarity, one must calculate the amount of solute needed based on the desired volume and concentration.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions. In the context of preparing solutions, it helps determine the mass of the solute required to achieve a specific molarity. Understanding stoichiometric relationships is essential for accurately measuring and mixing chemicals to create desired concentrations.

Dissolution Process

The dissolution process refers to how a solute interacts with a solvent to form a solution. When solid ammonium sulfate (1NH4)2SO4 is added to water, it dissociates into its constituent ions, which then become evenly distributed throughout the solvent. This process is important to understand to ensure complete solvation and uniform concentration in the final solution.