5. How many grams of potassium sulfate would be recovered by evaporating 623 mL of 22.5 % potassium sulfate solution to dryness (d= 1.23 g/mL)? 6. How many grams of hydrobromic acid are in 100.0 mL of 11.0 M hydrobromic acid solution? 7. A 525.0 mL sample of 5.50 M sulfuric acid has a density of 1.49 g/mL. Express the concentration of the solution in mass percent.

5. How many grams of potassium sulfate would be recovered by evaporating 623 mL of 22.5 % potassium sulfate solution to dryness (d= 1.23 g/mL)? 6. How many grams of hydrobromic acid are in 100.0 mL of 11.0 M hydrobromic acid solution? 7. A 525.0 mL sample of 5.50 M sulfuric acid has a density of 1.49 g/mL. Express the concentration of the solution in mass percent.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 27QAP

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Similar questions

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A large beaker contains 1.50 L of a 2.00 M iron(III) chloride solution. How many moles of iron ions are in the solution? How many moles of chloride ions are in the solution? You now add 0.500 L of a 4.00 M lead(II) nitrate solution to the beaker. Determine the mass of solid product formed (in grams).
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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.