Chem200HWChap13 - diluted acid. The stoichiometric point...

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Chapter 13 1. A 10.0-mL sample of 3.0 M KOH (aq) is transferred to a 250.0-mL volumetric flask and diluted to the mark. It was found that 38.5 mL of this diluted solution was needed to reach the stoichiometric point in a titration of 10.0 mL of a phosphoric acid solution. a) Write the balanced chemical equation for the titration. b) Calculate the molarity of H 3 PO 4 solution. c) What mass of H 3 PO 4 is in solution? 2. A solution of hydrochloric acid was prepared by measuring 10.00 mL of the concentrated acid into a 1 L volumetric flask and adding water up to the mark. Another solution was prepared by adding 0.530 g of anhydrous sodium carbonate to a 100 mL volumetric flask and adding water up to the mark. Then 25.00 mL of the latter solution was pipetted into a flask and titrated with the
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Unformatted text preview: diluted acid. The stoichiometric point was reached after 26.50 mL of acid had been added. a) Write the balanced equation for the reaction of HCl(aq) with Na 2 CO 3 (aq). b) What is the molarity of the original hydrochloric acid? 3. A vitamin C tablet was analyzed to determine whether it did in fact contain, as the manufacturer claimed, 1.0 g of the vitamin. A tablet was dissolved in water to form a 100.0 mL solution, and a 10.0-mL sample was titrated with iodine (as potassium triodide). It required 10.1 mL of 0.0521 M I 3-to reach the stoichiometric point in the titration. Given that 1 mol I 3-2245 1 mol vitamin C in the reaction, is the manufacturers claim correct? The molar mass of vitamin C is 176 g.mol-1 . 1...
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This note was uploaded on 09/09/2011 for the course CHEM 200 taught by Professor Saidane during the Spring '11 term at Mesa CC.

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