NaOH: Calculate Mass From Moles

To determine the mass of sodium hydroxide ($NaOH$) from a given number of moles, we need to utilize the concept of molar mass. Sodium hydroxide is a strong base, known for its corrosive properties, and understanding its chemical properties is crucial in various laboratory and industrial applications. The molar mass of a compound is the mass of one mole of that substance, expressed in grams per mole (g/mol). To find the molar mass of $NaOH$, we sum the atomic masses of its constituent elements: sodium (Na), oxygen (O), and hydrogen (H). The atomic mass of sodium is approximately 22.99 g/mol, oxygen is approximately 16.00 g/mol, and hydrogen is approximately 1.01 g/mol. Therefore, the molar mass of $NaOH$ is $22.99 + 16.00 + 1.01 = 40.00$ g/mol.

Now, we are given that we have $2.75 imes 10^{-4}$ moles of $NaOH$. The relationship between mass, moles, and molar mass is given by the formula: Mass = Moles $ imes$ Molar Mass Substituting the given values into the formula, we get: Mass = $(2.75 imes 10^{-4} ext{ mol}) imes (40.00 ext{ g/mol})$ Mass = $11.0 imes 10^{-3}$ g This can also be expressed in scientific notation as $1.10 imes 10^{-2}$ g.

It's important to handle sodium hydroxide with care due to its corrosive nature. Always use appropriate personal protective equipment, such as gloves and eye protection, when working with this chemical. Understanding these calculations is fundamental in stoichiometry, a branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. This allows chemists to predict the amount of product that can be formed or the amount of reactant needed for a specific reaction, which is vital for efficiency and safety in chemical synthesis and analysis.

The precision of the atomic masses used can influence the final answer. For most general chemistry calculations, using atomic masses rounded to two decimal places is sufficient. However, in more advanced or specialized applications, more precise atomic masses might be required. The molar mass is a fundamental property that bridges the macroscopic world (mass we can measure) with the microscopic world (number of atoms or molecules). This calculation is a basic yet essential skill for anyone involved in chemistry, whether it's for academic study, research, or industrial processes. The corrosive nature of NaOH also highlights the importance of understanding chemical safety protocols. Proper storage, handling, and disposal are critical to prevent accidents and protect both individuals and the environment.

In summary, calculating the mass of a substance from its moles involves knowing its molar mass. For $NaOH$, this molar mass is derived from the atomic masses of sodium, oxygen, and hydrogen. By multiplying the given moles by the calculated molar mass, we can accurately determine the mass of the sample. This process is a cornerstone of quantitative chemistry, enabling precise control and measurement in chemical experiments. The ability to perform such calculations is indispensable for students and professionals alike, ensuring accurate results and safe laboratory practices when dealing with chemicals like sodium hydroxide. The practical applications of these calculations range from pharmaceutical compounding to industrial chemical production, underscoring their significance.