How would you prepare each of the following solutions? (a) A 0.150 M solution of glucose in water

Verified step by step guidance

1. Determine the molar mass of glucose (C_6H_{12}O_6) by adding the atomic masses of all the atoms in the formula.
2. Calculate the number of moles of glucose needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume of solution in liters} \).
3. Convert the moles of glucose to grams using the molar mass calculated in step 1.
4. Measure the calculated mass of glucose using a balance.
5. Dissolve the measured glucose in a volume of water that is less than the desired final volume, then dilute to the final volume with water to ensure the solution is homogeneous.

Key Concepts

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is a crucial concept in chemistry for preparing solutions, as it allows chemists to quantify how much solute is present in a given volume of solvent. For example, a 0.150 M solution means there are 0.150 moles of solute (glucose) in every liter of solution.

Dissolving Solutes

Dissolving a solute involves the process of mixing a solid, liquid, or gas into a solvent to form a homogeneous solution. In the case of glucose, it is a solid that must be added to water, where it will interact with water molecules, breaking apart into individual glucose molecules. This process is essential for achieving the desired concentration in the final solution.

Preparation of Solutions

Preparing a solution involves accurately measuring the solute and solvent to achieve the desired concentration. For a 0.150 M glucose solution, one would calculate the mass of glucose needed for a specific volume of water, dissolve it completely, and then adjust the final volume to ensure the correct molarity. This process ensures that the solution is uniform and meets the required specifications for experiments or applications.