Concept explainers
In the qualitative cation analysis procedure,
Calculate the pH of a saturated aqueous solution of BiOOH.
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
- Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?arrow_forwardSolubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forwardThe solubility product for silver chloride is 1.6 x 10−10. What is the molar solubility of silver chloride in a 6.5 x 10−3 M AgNO3 aqueous solution at 298 K?arrow_forward
- The Ksp of calcium hydroxide, Ca(OH)2, is 1.3 × 10–6. Calculate the molar solubility of calcium hydroxide.arrow_forwardThe solubility of silver chromate (Ag2CrO4) in 500 mL of water at 25°C is 0.0129 g. Calculate its solubility product constant.arrow_forwardThe ionic compound magnesium hydroxide, which is found in the over-the-counter consumer product Milk of Magnesia™,has the formula Mg(OH)2. Magnesium hydroxide dissolves in water according to the following equation:Mg(OH)2(s) ←→ Mg2+(aq) + 2OH–(aq)Write the solubility product expression for magnesium hydroxidearrow_forward
- = 1.6 x 10-10 Given the reactions below, calculate the molar solubility of AgCl (s) in 0.566 M NH3 (aq) at 25 degrees C. AgCl (s) →> Ag+ (aq) + Cl¯ (aq) K sp Ag+ (aq) + 2 NH3 (aq) →> Ag (NH3) + (aq) K = 1.7 x 107 f 2 Report your answer rounded to two significant figures and do NOT include units. Use "e" for scientific notation. For example, 1.0 x 10-14 is 1.0e-14.arrow_forwardWrite the general equilibrium constant for 2 NaBr(aq) + Pb(ClO4)2(aq) → PbBr2(s) + 2 NaClO4(aq). K = 1 / [Pb^2+][Br^−] 2 K = [NaClO4]^2 / [NaBr]^2 [Pb(ClO4)2] K = [Pb^2+][Br−]^2 K = [PbBr2] / [Pb^2+][Br−]^2 K = 1 / [Pb(ClO4)2][NaBr]^2arrow_forwardAnswer the following questions about the solubility of AgCl(s). The value of Ksp for AgCl(s) is 1.8 × 10−10. Calculate the value of [Ag+] in a saturated solution of AgCl in distilled water. The concentration of Cl−(aq) in seawater is 0.54 M. Calculate the molar solubility of AgCl(s) in seawater. Explain why AgCl(s) is less soluble in seawater than in distilled water.arrow_forward
- The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?arrow_forwardThe solubility product of aluminum hydroxide (Al(OH)3) is 1.9x10–33. Derive an equation for the concentration of Al3+ in water as a function of pH if the water is saturated with Al(OH)3. If the concentration of Al3+ in water cannot exceed 10 micromolar (because all the aluminum has dissolved), at what pH would you expect the product of the Al3+ concentration and the PO43− concentration to be a maximum? Explain your reasoning.arrow_forwardThe drinking water standard for lead is 0.05 mg/L total soluble lead. One method for removing heavy metals such as lead is pH adjustment to precipitate the metal hydroxide. Consider the reactions governing the solubility of lead hydroxide in pure water: Pb(OH)2(s) Pb²+ + 2OH- Pb²+ + OH →PbOH+ 2+ Pb²+ + 2OH™↔Pb(OH)₂⁰ Pb²+ + 3OH Pb(OH)3¯ Kso=10-15.6 B₁-106.3 B2-1010.9 B3-1013.9 Construct a logC-pH diagram for the Pb(OH)2(s) system. Indicate the region of Pb(OH)2 supersaturation by shading the appropriate portion of the diagram.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning