When a solution of hydrogen bromide is prepared, \(1.283 \mathrm{~L}\) of \(\mathrm{HBr}\) gas at \(25^{\circ} \mathrm{C}\) and \(0.974\) atm is bubbled into \(250.0 \mathrm{~mL}\) of water. Assuming all the HBr dissolves with no volume change, what is the molarity of the hydrobromic acid solution produced?

The Ideal Gas Law is a fundamental equation bridging the properties of gases, showing how pressure (P), volume (V), temperature (T), and number of moles (n) of a gas are interrelated. Represented by the equation PV = nRT, where R is the ideal gas constant, this law allows us to calculate any one of these variables if the others are known. In the context of the problem, we used the Ideal Gas Law to find the number of moles of hydrobromic gas, based on its pressure, volume, and temperature. Understanding how to manipulate this equation is crucial for various applications in chemistry, such as calculating gas densities, molar masses, and as seen here, solution molarity.

When dealing with the Ideal Gas Law, one must always be mindful to convert all values into the correct units. For instance, temperature should be in Kelvin (K) and volume may need to be converted to liters (L) if not already provided in such units. This meticulous approach ensures accuracy in your mole calculations, playing a pivotal role in deducing the correct molarity of a solution, as demonstrated in our example.

The mole is a basic unit in chemistry that quantifies amount of substance. One mole equals approximately 6.022 \(\times\) 10^23 (Avogadro's number) of entities, whether they are atoms, molecules, ions, or other particulates. Calculating moles can be made simple by applying the correct formulas, such as the Ideal Gas Law in gas scenarios, or mass divided by molar mass for substances with known quantities.

In our exercise, we calculated the moles of hydrobromic acid by arranging the Ideal Gas Law. This calculation was a two-step process: first rearranging the equation to solve for n, and then substituting in the known values. It's important for students to familiarize themselves with these steps in order to calculate moles swiftly in differing contexts—whether it's a reaction proceeding in a lab, or when analyzing a gaseous sample in an environmental study.

Hydrobromic acid (HBr) is a strong acid that completely dissociates in water. The concentration of such a solution can be expressed in molarity (M), which is the number of moles of solute per liter of solution. To ensure a deep understanding, it is essential to recognize that the concentration reflects the ratio of the number of moles of hydrobromic acid to the volume of solution—in this case, the water into which the HBr gas is dissolved.

Calculating the molarity involves dividing the moles of solute by the volume of solvent (converted to liters), as we did in our problem. This gives a clear indication of the strength of the hydrobromic acid solution created. These concepts are not only important in academic exercises but also in practical applications such as making standard solutions in a laboratory setting or adjusting concentrations for industrial processes.