Question

The density of concentrated sulfuric acid is \(1.85 \mathrm{~g} / \mathrm{ml}\). What volume of the acid would weigh \(74.0 \mathrm{~g}\) ?

Short answer

The volume of the concentrated sulfuric acid that would weigh 74.0 g is approximately \(40.0 \mathrm{ml}\).

Step-by-step solution

Identify the given information

We are given the following information: - Density of concentrated sulfuric acid: \(1.85 \mathrm{~g} / \mathrm{ml}\) - Mass of concentrated sulfuric acid: \(74.0 \mathrm{~g}\)

Use the density formula to find the volume

We can use the formula: Density = mass/volume Rearrange the formula to find the volume: Volume = mass/density

Substitute the given values and solve for the volume

Now, we will substitute the given values into the formula and solve for the volume: Volume = \(\frac{74.0 \mathrm{~g}}{1.85 \mathrm{~g} / \mathrm{ml}}\) Volume ≈ \(40.0 \mathrm{ml}\) So, the volume of the concentrated sulfuric acid that would weigh 74.0 g is approximately 40.0 mL.

Key concepts

Understanding Sulfuric Acid

Sulfuric acid (H2SO4) is a highly corrosive strong mineral acid with a wide range of applications in industry and laboratories. Being colorless to slightly yellow, it is a viscous liquid which is soluble in water at all concentrations. It's used in battery acid, as a dehydrating agent, in fertilizer production, oil refining, wastewater processing, and chemical synthesis. Its significant role in various reactions, including acid-base reactions, synthesis, and decomposition, makes it essential in chemistry problem solving.

When dealing with sulfuric acid, it's crucial to understand its density, which is notably higher than that of water due to its molecular structure, with two hydrogen atoms, one sulfur atom, and four oxygen atoms resulting in a dense molecular framework. The density becomes an important factor to consider in calculations for preparatory procedures or when specific volumes need to be measured for reactions or processes.

Chemistry Problem Solving with Density

Solving chemistry problems often involves understanding and applying the concepts of density. The density of a substance is a measure of how much mass is contained in a given volume. Being able to calculate the density or use it to find volume or mass is an essential skill in chemistry.

In particular, for concentrated sulfuric acid or other chemical solutions, density calculations become important in laboratory preparations, where precise amounts of a substance are required for a reaction. Knowing the density enables chemists to correctly calculate the volume needed for a given mass of substance or vice versa. Problem solving in chemistry requires careful identification of what is known and what needs to be discovered, methodical use of formulas, and accurate manipulation of units throughout the calculation. This stepwise approach ensures that the results are reliable and applicable to practical situations in the laboratory.

The Density Formula in Practice

The density formula is a key tool in scientific calculations and is defined as the ratio of mass to volume. It is usually expressed in grams per cubic centimeter (g/cm³) or grams per milliliter (g/mL) for liquids. This formula is crucial for converting between the mass of a substance and the volume that it occupies.

In the given exercise, we used the density formula to determine the volume of a mass of sulfuric acid. By rearranging the formula to express volume as mass divided by density (\( Volume = \frac{mass}{density} \)), we're able to find the volume occupied by a known mass of the acid. It's important to always keep track of units when solving such problems, as consistent units across mass and volume are essential for the correct application of the formula. This basic yet extremely useful equation underpins many complex calculations in the field of chemistry, underscoring the concept that even the most advanced scientific problems often rely on a foundation of fundamental principles.