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(b) Potassium nitrate was synthesized in an experiment using 10 mL of nitric acid and excess potassium hydroxide. The mass data obtained from the experiment is shown in Table 1 below. Given that the percentage yield of potassium nitrate was 88.3 %, calculate the concentration (% m/v) of the nitric acid used in the experiment. Table 1: Mass data for the synthesis of potassium nitrate from nitric acid and potassium hydroxide Mass of clock glass and crystallized potassium nitrate/ 45.55 Mass of empty clock glass/ g 39.18

Which piece of equipment would you use to measure 7.10 mL of CuSO4 (aq)?

A company is making table salt by using a dryer to remove water from wet salt crystals. Wet salt crystals are fed to the dryer at a rate of 4900 pounds per hour. The wet salt crystals have a water content of 63%. The water that is removed by the dryer does not contain any salt. The dryer removes 3,000 pounds per hour of water. What is the water concentration (%) in the product table salt that is being produced by the drier?

Oнtres OH CH3 HBr CH3CN (solvent) E1 H₂C

A 15000 L tailings pond at a mine site was analyzed for cadmium contamination. First, a 25.0 mL sample of water was removed from the pond. Then the solution was evaporated to dryness, and 56.1 mg of cadmium was recovered (the identity of the metal was confirmed through other methods). Assuming the water is homogeneously distributed throughout the pond, what is the concentration of cadmium in the tailings pond?

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl3(aq) + 3 AgNO3(aq) 3 AgCl(s) + Fe(NO3),(a9) The chemist adds 56.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 2.8 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. mg L Submit Assignment Continue Accessibility Privacy O 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use 888 %23 5 6 2 3 E R. G…

Please consider significant figures.

Please consider significant figures.

In preparing a zinc oxide ointment, 28.35 g of zinc oxide was used rather than the correct quantity, 31.1 g. What percentage error was incurred?