For 2.200 g of KHP, how many milliliters of 0.3 M sodium hydroxide \( (\mathrm{NaOH}) \) is needed to reach the endpoint of the titration? Report your answer to the nearest milliliter. Choose the single best answer. A. 28 mL B. 36 mL C. 10 mL D. 103 mL METHODS RESET MY NOTES LAB DATA SHOW LABELS

To find out how many milliliters of 0.3 M sodium hydroxide (NaOH) are needed to titrate 2.200 g of potassium hydrogen phthalate (KHP), it's important to know the molar mass of KHP, which is approximately 204.22 g/mol. First, convert the mass of KHP to moles: \[ \text{Moles of KHP} = \frac{2.200 \, g}{204.22 \, g/mol} \approx 0.01078 \, mol \] Since KHP is a monoprotic acid, it reacts with NaOH in a 1:1 ratio. Therefore, you will also need 0.01078 moles of NaOH for the titration. Now, using the concentration of NaOH (0.3 M), calculate the volume required: \[ \text{Volume of NaOH (in liters)} = \frac{0.01078 \, mol}{0.3 \, mol/L} \approx 0.03593 \, L \] Converting this to milliliters: \[ 0.03593 \, L \times 1000 \, mL/L \approx 35.93 \, mL \] Rounding to the nearest milliliter gives approximately 36 mL. So, the best answer is **B. 36 mL**. Titration has a rich history in the development of analytical chemistry. The concept was popularized in the late 18th century by Antoine Lavoisier, who demonstrated its utility in quantifying the concentration of acids and bases. This advancement was vital in furthering the understanding of chemical reactions and laid the groundwork for modern titrimetric methods. In real-world applications, titration is crucial in various industries, including pharmaceuticals, food and beverage, and environmental monitoring. For instance, titration helps ensure that the acidity of soft drinks is within desired levels, providing not only quality control but also compliance with health regulations. This technique can also be used to determine water quality by quantifying pollutants or determining hardness.