An analytical chemist weighs out 0.163g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1300M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 16.5mL of NaOH solution.Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
Question
An analytical chemist weighs out 0.163g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1300M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 16.5mL of NaOH solution.Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
Solution
To calculate the molar mass of the unknown acid, we need to follow these steps:
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First, we need to calculate the moles of NaOH used in the titration. We can do this using the formula: moles = Molarity * Volume(L). The molarity of NaOH is given as 0.1300M and the volume is 16.5mL which is equal to 0.0165L. So, moles of NaOH = 0.1300 * 0.0165 = 0.002145 moles.
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Since the unknown acid is monoprotic, it means that one mole of the acid reacts with one mole of NaOH. Therefore, the moles of the unknown acid is also 0.002145 moles.
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Now, we can calculate the molar mass of the unknown acid using the formula: Molar mass = mass(g) / moles. The mass of the unknown acid is given as 0.163g and we have calculated the moles as 0.002145. So, Molar mass = 0.163 / 0.002145 = 75.988 g/mol.
Therefore, the molar mass of the unknown acid is approximately 76.0 g/mol when rounded to three significant digits.
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