Final answer:
The question inquires about dissolving sucrose in water to make a solution. It is a chemistry question related to the preparation and concentration calculation of solutions. The calculation involves determining the mass/volume percentage or molarity if moles are given.
Step-by-step explanation:
The question involves dissolving 1.50g of sucrose in enough deionized water to prepare a 10.00 ml solution. This is a topic from Chemistry, specifically from a section dealing with solutions and their concentration calculations. The solvent in this solution is deionized water, and the solute is sucrose (C12H22O11). To determine the concentration of the solution, one could calculate the mass/volume percentage, which would be the mass of the sucrose divided by the total volume of the solution, then multiplied by 100%.
For example, a similar problem would be if a 1.00 g of sucrose solution was prepared in 100.0 g of liquid water, one would identify water as the solvent and sucrose as the solute. If expressed in molarity, for instance, a teaspoon of table sugar (approximately 0.01 mol sucrose) dissolved in a 200 mL cup of tea, one would calculate the molarity by dividing the number of moles of sucrose by the volume of the solution in liters.