Question

1) a. Write the balanced molecular equation that occurs for the complete reaction of sulfuric acid with sodium hydroxide.

b. To determine the molarity of your final sulfuric acid solution, you titrate the final solution with a standardized sodium hydroxide solution to the second equivalence point. If 26.32 mL of 0.1000 M sodium hydroxide was required for complete reaction with 10.00 mL of the final sulfuric acid solution, determine the molarity of the final sulfuric acid solution precisely to four significant figures.

c. If the same dilution factors used in lab were also used to prepare this final sulfuric acid solution, determine the molarity of both the stock solution and initial solution of sulfuric acid.

2. A 0.158–gram sample of a salt, comprised of barium and one of the halide ions (BaX2), was dissolved in water, and an excess of sulfuric acid was added to form barium sulfate, BaSO4. After filtering and drying, the solid BaSO4 weighed 0.124 grams. Determine the identity of the halide ion (X) and the formula of the barium halide salt.

Answer 1