A chemistry student weighs out 0.134g of hypobromous acid HBrO into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NaOH solution.Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.
Question
A chemistry student weighs out 0.134g of hypobromous acid HBrO into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NaOH solution.Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.
Solution
To solve this problem, we need to follow these steps:
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First, we need to find the number of moles of HBrO. We can do this by dividing the mass of HBrO by its molar mass. The molar mass of HBrO (1.01 g/mol for H, 79.90 g/mol for Br, and 16.00 g/mol for O) is approximately 96.91 g/mol. So, the number of moles of HBrO is 0.134 g / 96.91 g/mol = 0.00138 mol.
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In a titration to the equivalence point, the number of moles of acid is equal to the number of moles of base. So, we need 0.00138 mol of NaOH to neutralize the HBrO.
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Finally, we can find the volume of NaOH solution needed by dividing the number of moles of NaOH by its concentration. The volume is therefore 0.00138 mol / 0.2000 M = 0.00690 L, or 6.90 mL.
So, the student will need to add approximately 6.90 mL of NaOH solution to reach the equivalence point.
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