Determine the mass/volume percent of a solution made by dissolving: (a) \(175.2 \mathrm{~g}\) of table sugar, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\), in water to make \(275.5 \mathrm{~mL}\) of solution (b) \(35.5 \mathrm{~g}\) of \(\mathrm{CH}_{3} \mathrm{OH}\) (methanol) in water to make \(75.0 \mathrm{~mL}\) of solution

When trying to understand a solution's composition, concentration measurement becomes a fundamental tool in chemistry. It quantifies the proportion of one substance, known as the solute, within another, known as the solvent. Mass/Volume percent, often shown as m/v%, is one of the simplest concentration measurements. To get the mass/volume percent, we use the following formula:
\[ \text{m/v\%} = \left(\frac{\text{mass of solute in grams}}{\text{volume of solution in mL}}\right) \times 100 \]
This formula tells us how many grams of solute can be found in 100 milliliters of a solution. It is particularly useful in day-to-day applications, like pharmacy or culinary recipes, where quantities are typically discussed in terms of volume.

In any solution, the solute and solvent play critical roles. The solute is the substance that gets dissolved, while the solvent is the medium that does the dissolving. Understanding the distinction is key to grasping various chemistry topics, including concentration.

It's easy to recall the roles by thinking of a common example: when making saltwater, the salt is the solute and the water is the solvent. When discussing solutions, the majority substance is often the solvent, and the minority substance is the solute. The solubility of the solute in the solvent defines how well a substance can become part of the solution and at what degree—information that's particularly important when preparing solutions in the lab or in industry.

Accurate chemistry calculations are the heart of many scientific studies and industrial processes. In the realm of concentration, precise calculations ensure the correct proportions of solute and solvent, which can affect the properties and effectiveness of a solution. When tackling mass/volume percent problems, following a step-by-step approach eliminates errors and provides clarity:

• Identify the solute and its mass.
• Determine the total volume of the solution.
• Apply the appropriate formula, in this case for m/v%, without forgetting to multiply by 100 to get the percentage.
• Ensure the units are consistent for accurate results—a common hurdle in chemistry calculations.

With practice, these calculations become second-nature, enabling not only academic success but also practical applications in fields ranging from medicine to engineering.