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A chemist dissolves 777.mg of pure hydroiodic acid in enough water to make up 110.mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

Question

A chemist dissolves 777.mg of pure hydroiodic acid in enough water to make up 110.mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

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Solution

To calculate the pH of the solution, we first need to find the molarity (M) of the solution.

  1. Convert the mass of hydroiodic acid (HI) from milligrams to grams: 777 mg = 0.777 g

  2. Calculate the number of moles of HI. The molar mass of HI is approximately 128 g/mol, so: Moles of HI = 0.777 g / 128 g/mol = 0.00607 mol

  3. Calculate the volume of the solution in liters: 110 mL = 0.110 L

  4. Calculate the molarity (M) of the solution: M = moles / volume = 0.00607 mol / 0.110 L = 0.0552 M

Hydroiodic acid is a strong acid, so it will completely dissociate in water. Therefore, the concentration of H+ ions will be equal to the molarity of the solution, which is 0.0552 M.

The pH of a solution is calculated using the formula pH = -log[H+].

  1. Calculate the pH of the solution: pH = -log(0.0552) = 1.26

So, the pH of the solution is 1.26.

This problem has been solved

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