Problem PageQuestionA chemist dissolves 263.mg of pure hydroiodic acid in enough water to make up 210.mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places

To solve this problem, we need to follow these steps:

1. Convert the mass of hydroiodic acid (HI) to moles. Hydroiodic acid has a molar mass of approximately 128 g/mol. So, 263 mg is equal to 0.263 g. Therefore, the number of moles of HI is 0.263 g / 128 g/mol = 0.00205 mol.

2. Calculate the molarity of the solution. Molarity is defined as the number of moles of solute per liter of solution. So, the molarity of the HI solution is 0.00205 mol / 0.210 L = 0.00976 M.

3. Hydroiodic acid is a strong acid, which means it completely dissociates in water. Therefore, the concentration of H+ ions in the solution is equal to the molarity of the HI solution, which is 0.00976 M.

4. Calculate the pH of the solution. The pH is defined as the negative logarithm (base 10) of the H+ ion concentration. So, the pH of the solution is -log(0.00976) = 2.010.

Therefore, the pH of the solution is approximately 2.010.