Question 22 of 27 A student needs to prepare 250 mL of a 0.850 M aqueous solution of sucrose, C,,H„0,, (aq), which is used frequently in biological experiments. 200 mL 250 mL 150 100 200 150 50 2:0 m 100 A Which type of glassware should be used to make this How should the correct amount of solute be obtained? solution (assuming that the accuracy of the concentration is important)? Measure out x mol of solid sucrose on a molemeter. Measure out xg of solid sucrose on a balance. O A Measure out x cm of sucrose with a ruler.

Question 22 of 27 A student needs to prepare 250 mL of a 0.850 M aqueous solution of sucrose, C,,H„0,, (aq), which is used frequently in biological experiments. 200 mL 250 mL 150 100 200 150 50 2:0 m 100 A Which type of glassware should be used to make this How should the correct amount of solute be obtained? solution (assuming that the accuracy of the concentration is important)? Measure out x mol of solid sucrose on a molemeter. Measure out xg of solid sucrose on a balance. O A Measure out x cm of sucrose with a ruler.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section: Chapter Questions

Problem 82AP: Which of the following statements is/are true regarding solutions? l type='a'> If a solute is...

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When a solution is diluted by adding additional solvent, the concentration of solute changes hut the amount of solute present does not change. Explain. Suppose 250. mL of water is added to 125 mL of 0.55 1 M NaCl solution. Explain how you would calculate the concentration of the solution after dilution.
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
60. Suppose 325 in L of 0.150 M NaOH is needed for your experiment. How would you prepare this if all that is available is a 1.01 M NaOH solution?
What volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4? Phosphoric acid contains three acidic hydrogens.
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
Which of the following statements is/are true regarding solutions? l type='a'> If a solute is dissolved in water, then the resulting solution is considered aqueous. i>If two solutions are mixed and no chemical reaction occurs, then a net ionic equation cannot be written. i>If two clear solutions are mixed and then cloudiness results, this indicates that a precipitate formed.

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