22. When the following solutions are mixed, which will NOT form a precipitate? A. FeSO4(aq) + KCl(aq) B. Al(NO3)3(aq) + Ba(OH)2(aq) C. CaCl₂(aq) + Na₂SO4(aq) D. K₂S(aq) + Ni(NO3)2(aq) 23. A solution containing NH4Cl and NH3 has a hydroxide-ion concentration of 10-6 M. Which of the following hydroxides may be precipitated when this solution is added to an equal volume of a 0.1 M solution of a metal ion? B. A. Ba(OH)2 (Ksp = 1.0 × 10-4) Ca(OH)2 (Ksp = 2.2 x 10-5) C. Mg(OH)2 (Ksp = 3.0 × 10-12) D. Fe(OH)2 (Ksp = 8.0 × 10-16)

22. When the following solutions are mixed, which will NOT form a precipitate? A. FeSO4(aq) + KCl(aq) B. Al(NO3)3(aq) + Ba(OH)2(aq) C. CaCl₂(aq) + Na₂SO4(aq) D. K₂S(aq) + Ni(NO3)2(aq) 23. A solution containing NH4Cl and NH3 has a hydroxide-ion concentration of 10-6 M. Which of the following hydroxides may be precipitated when this solution is added to an equal volume of a 0.1 M solution of a metal ion? B. A. Ba(OH)2 (Ksp = 1.0 × 10-4) Ca(OH)2 (Ksp = 2.2 x 10-5) C. Mg(OH)2 (Ksp = 3.0 × 10-12) D. Fe(OH)2 (Ksp = 8.0 × 10-16)

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 116AP

See similar textbooks

Similar questions

One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H+ or OH ions left in solution.
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?
Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.
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?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
A noncarbonated soft drink contains an unknown amount of citric acid, H3C6H5O7. lf 100. mL of the soft drink requires 33.51 mL of 0.0102 M NaOH to neutralize the citric add completely, what mass of citric acid does the soft drink contain per 100. mL? The reaction of citric acid and NaOH is H3C6H5O7(aq) + 3 NaOH(aq) Na3C6H5O7(aq) + 3 H2O()
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?