Final answer:
After calculating the molarity of the NaOH solution, we find that the pH of the solution is approximately 13, which is not one of the options provided in the question.
Step-by-step explanation:
The student has asked about the pH of a solution prepared by dissolving 0.8 g NaOH in 200 mL of water. NaOH is a strong base and dissociates completely in water. To calculate the pH, first we need to calculate the molarity of the solution. The molar mass of NaOH is approximately 40 g/mol.
Therefore, the number of moles of NaOH is:
Number of moles = mass (g) / molar mass (g/mol) = 0.8 g / 40 g/mol = 0.02 mol
Next, we calculate the molarity (M), which is moles of solute per liter of solution:
Molarity = moles / volume (L) = 0.02 mol / 0.2 L = 0.1 M
Since NaOH is a strong base, it contributes one OH- ion per NaOH molecule to the solution, so the pOH of the solution is equal to 1 when rounded to the nearest whole number (pOH = -log[OH-] = -log[0.1]). Finally, we use the relation pH + pOH = 14 at 25 °C to find the pH:
pH = 14 - pOH = 14 - 1 = 13
Thus, the pH of the solution is 13, which makes option d) 14.0 incorrect. The correct choice is not listed among the provided options.