Final answer:
To calculate the pH of the nitric acid solution, the molarity of HNO₃ was found to be 0.001 M by dividing the number of moles of HNO₃ by the volume of the solution. Since HNO₃ is a strong acid, the pH was then calculated using the pH formula, yielding a value of 3.0.
Step-by-step explanation:
To calculate the pH of a solution prepared by dissolving 0.63 g of nitric acid (HNO₃) in 10 L of the solution, we must first determine the molar concentration of HNO₃. Nitric acid is a strong acid, so it completely dissociates in water. Knowing the molar mass of HNO₃ (~63 g/mol), we can find the number of moles of acid using the formula:
moles of HNO₃ = 0.63 g / 63 g/mol = 0.01 moles
With this, the concentration [HNO3] is:
[HNO₃] = moles / volume = 0.01 moles / 10 L = 0.001 M
Since HNO₃ is a strong acid, its concentration equals the hydronium ion concentration [H₃O+]. Hence, the pH can be calculated using the formula:
pH = -log [H₃O+] = -log(0.001) = 3.0
Therefore, the pH of the solution is 3.0.