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a. Magnesium chloride and sodium hydroxide. OMagnesium hydroxide, Mg(OH)2. Rule 5: Most hydroxide salts are only slightly soluble. OMagnesium hydroxide, Mg(OH)2. Rule 5: Exception. OMagnesium hydroxide, Mg(OH)2. Rule 3: Most hydroxide salts are only slightly soluble. ONo precipitate. b. Copper(II) nitrate and ammonium sulfide. Copper(II) sulfide, CuS. Rule 6: Most sulfide salts are only slightly soluble. Copper(II) sulfide, CuS. Rule 6: Exception. OCopper(II) sulfide, CuS. Rule 3: Most sulfide salts are only slightly soluble. ONo precipitate. c. Potassium phosphate and magnesium nitrate. OMagnesium phosphate, Mg3 (PO4)2. Rule 3: Most phosphate salts are only slightly soluble. Magnesium phosphate, Mg, (PO4)2. Rule 6: Exception. OMagnesium phosphate, Mg, (PO4)2. Rule 6: Most phosphate salts are only slightly soluble. ONo precipitate. d. Sodium carbonate and calcium nitrate. OCalcium carbonate, CaCO3. Rule 3: Most carbonate salts are only slightly soluble. OCalcium carbonate, CaCO3. Rule 6: Exception. OCalcium carbonate, CaCO3. Rule 6: Most carbonate salts are only slightly soluble. ONo precipitate.

a. Magnesium chloride and sodium hydroxide. OMagnesium hydroxide, Mg(OH)2. Rule 5: Most hydroxide salts are only slightly soluble. OMagnesium hydroxide, Mg(OH)2. Rule 5: Exception. OMagnesium hydroxide, Mg(OH)2. Rule 3: Most hydroxide salts are only slightly soluble. ONo precipitate. b. Copper(II) nitrate and ammonium sulfide. Copper(II) sulfide, CuS. Rule 6: Most sulfide salts are only slightly soluble. Copper(II) sulfide, CuS. Rule 6: Exception. OCopper(II) sulfide, CuS. Rule 3: Most sulfide salts are only slightly soluble. ONo precipitate. c. Potassium phosphate and magnesium nitrate. OMagnesium phosphate, Mg3 (PO4)2. Rule 3: Most phosphate salts are only slightly soluble. Magnesium phosphate, Mg, (PO4)2. Rule 6: Exception. OMagnesium phosphate, Mg, (PO4)2. Rule 6: Most phosphate salts are only slightly soluble. ONo precipitate. d. Sodium carbonate and calcium nitrate. OCalcium carbonate, CaCO3. Rule 3: Most carbonate salts are only slightly soluble. OCalcium carbonate, CaCO3. Rule 6: Exception. OCalcium carbonate, CaCO3. Rule 6: Most carbonate salts are only slightly soluble. ONo precipitate.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3) salts are soluble. 2. Most salts of Na+, K+, and + NH4 are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( 2- CO3), and phosphate ( 3- PO4³) salts are only slightly soluble. * *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. Show Hint Previous Next Save and
Transcribed Image Text:On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3) salts are soluble. 2. Most salts of Na+, K+, and + NH4 are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( 2- CO3), and phosphate ( 3- PO4³) salts are only slightly soluble. * *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. Show Hint Previous Next Save and
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3) salts are soluble. 2. Most salts of Na+, K+, and + NH4 are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( 2- CO3), and phosphate ( 3- PO4³) salts are only slightly soluble. * *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. Show Hint Previous Next Save and
Transcribed Image Text:On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3) salts are soluble. 2. Most salts of Na+, K+, and + NH4 are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( 2- CO3), and phosphate ( 3- PO4³) salts are only slightly soluble. * *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. Show Hint Previous Next Save and
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