(a) Calculate the mass percentage of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in a solution containing 10.6 \(\mathrm{g}\) of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in 483 \(\mathrm{g}\) of water. (b) An ore contains 2.86 \(\mathrm{g}\) of silver per ton of ore. What is the concentration of silver in ppm?

Understanding solution concentration is essential in chemistry and various practical situations, including cooking, and medicine. Concentration indicates how much of a substance, known as the solute, is contained within a certain volume or mass of another substance, called the solvent. When we refer to the mass percentage of a solute in a solution, we are indicating the fraction of the solution's total mass that is composed of the solute.

For instance, if you dissolve a small amount of salt in water, the salt is the solute, and the water is the solvent. By calculating the mass percentage, you can determine the strength of the solution. A higher mass percentage means a stronger solution, while a lower mass percentage means a more diluted one. This is essential for ensuring correct dosages in pharmaceuticals or the desired taste in food preparations. To calculate the mass percentage, you divide the mass of the solute by the total mass of the solution (which includes both the solute and the solvent) and then multiply by 100.

The term 'parts per million' (ppm) is another way to express very dilute concentrations of substances. One ppm signifies that one unit of the solute is present in one million units of the total solution. This unit is very convenient for measuring extremely low concentrations, such as impurities in water, air quality, or, as in this exercise's context, the amount of a precious metal within an ore.

Calculating ppm is straightforward when you have the mass of the solute and the mass of the solution. You simply divide the mass of the solute by the total mass of the solution and then multiply the result by one million. This conversion is especially useful when dealing with environmental regulations, where maximum permissible levels of contaminants are often defined in ppm, thus requiring precision and an understanding of how very small amounts relate to larger quantities.

In different regions and for various applications, certain mass units may be preferred. For example, the gram is frequently used in scientific contexts, while the pound may be more common in everyday life in the United States. Converting between these units is essential for accurate communication of measurements. The process of converting units requires an understanding of the equivalent values between units. For instance, understanding that one kilogram is equivalent to 1000 grams is necessary for such conversions.

In chemistry and physics problems, you often need to convert between mass units to carry out calculations correctly. A ton, commonly used in measuring large quantities of raw materials like ore, equals 1000 kilograms or 1 million grams. Therefore, knowing how to convert tons to grams is critical when calculating ppm for substances, such as the concentration of silver in ore, as seen in the provided exercise. This conversion ensures that all measurements are in the same units, which is a fundamental step in performing accurate calculations.