A chemist dissolves 790.mg of pure perchloric acid in enough water to make up 320.mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.
Question
A chemist dissolves 790.mg of pure perchloric acid in enough water to make up 320.mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.
Solution
To calculate the pH of the solution, we first need to find the molarity (M) of the solution.
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Convert the mass of perchloric acid (HClO4) from milligrams to grams: 790 mg = 0.790 g
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Calculate the number of moles of HClO4. The molar mass of HClO4 is approximately 100.46 g/mol. Number of moles = mass (g) / molar mass (g/mol) Number of moles = 0.790 g / 100.46 g/mol = 0.00787 mol
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Calculate the molarity of the solution. Molarity (M) = moles of solute / liters of solution. Convert the volume of the solution from milliliters to liters: 320 mL = 0.320 L Molarity = 0.00787 mol / 0.320 L = 0.0246 M
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Perchloric 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 acid.
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Calculate the pH of the solution. pH = -log[H+] pH = -log(0.0246) = 1.61
So, the pH of the solution is 1.61.
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