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a. H3PO4 (aq) + Fe(NO3)2 (aq) → HNO3(aq) + Fe3(PO4)2 (8) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. O2H3PO4 (aq) + 3Fe(NO3)2 (aq) →6HNO3(aq) + Fes (PO4)2 (aq) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. O2H3PO4 (aq) + 3Fe(NO3)2 (aq) →6HNO3(aq) + Fe3(PO4)2 (8) Rule 2: Most phosphate (PO4³) salts are only slightly soluble. 2H3PO4 (aq) + 3Fe(NO3)2 (aq) → 6HNO3(aq) + Fes (PO4)2 (8) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. H₂S (aq) + Ca(NO3)2 (aq) → b. H₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(s) Rule 6: Most sulfide salts are only slightly soluble. OH₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(8) Rule 2: Most sulfide salts are only slightly soluble. O H₂S(aq) + Ca(NO3)2 (aq) → HNO3(aq) + Cas(8) Rule 6: Most sulfide salts are only slightly soluble. H₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(aq) Rule 6: Most sulfide salts are only slightly soluble. MnCl₂ (aq) + NaOH(aq) → c. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (8) Rule 2: Most hydroxide compounds are only slightly soluble. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (8) Rule 5: Most hydroxide compounds are only slightly soluble. O MnCl₂ (aq) + NaOH(aq) → NaCl(aq) + Mn(OH)2 (8) Rule 5: Most hydroxide compounds are only slightly soluble. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (aq) Rule 5: Most hydroxide compounds are only slightly soluble.

a. H3PO4 (aq) + Fe(NO3)2 (aq) → HNO3(aq) + Fe3(PO4)2 (8) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. O2H3PO4 (aq) + 3Fe(NO3)2 (aq) →6HNO3(aq) + Fes (PO4)2 (aq) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. O2H3PO4 (aq) + 3Fe(NO3)2 (aq) →6HNO3(aq) + Fe3(PO4)2 (8) Rule 2: Most phosphate (PO4³) salts are only slightly soluble. 2H3PO4 (aq) + 3Fe(NO3)2 (aq) → 6HNO3(aq) + Fes (PO4)2 (8) Rule 6: Most phosphate (PO4³) salts are only slightly soluble. H₂S (aq) + Ca(NO3)2 (aq) → b. H₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(s) Rule 6: Most sulfide salts are only slightly soluble. OH₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(8) Rule 2: Most sulfide salts are only slightly soluble. O H₂S(aq) + Ca(NO3)2 (aq) → HNO3(aq) + Cas(8) Rule 6: Most sulfide salts are only slightly soluble. H₂S(aq) + Ca(NO3)2 (aq) → 2HNO3(aq) + Cas(aq) Rule 6: Most sulfide salts are only slightly soluble. MnCl₂ (aq) + NaOH(aq) → c. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (8) Rule 2: Most hydroxide compounds are only slightly soluble. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (8) Rule 5: Most hydroxide compounds are only slightly soluble. O MnCl₂ (aq) + NaOH(aq) → NaCl(aq) + Mn(OH)2 (8) Rule 5: Most hydroxide compounds are only slightly soluble. MnCl₂ (aq) + 2NaOH(aq) → 2NaCl(aq) + Mn(OH)2 (aq) Rule 5: Most hydroxide compounds are only slightly soluble.

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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For each of the following precipitation reactions, choose the right variant for completing and balancing the equation, indicating clearly which product is the precipitate. If no reaction would be expected, so indicate. [Review Topics] 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 + NHA 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. NaOH and KOH. [References] 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( CO32), 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
Transcribed Image Text:For each of the following precipitation reactions, choose the right variant for completing and balancing the equation, indicating clearly which product is the precipitate. If no reaction would be expected, so indicate. [Review Topics] 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 + NHA 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. NaOH and KOH. [References] 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( CO32), 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
For each of the following precipitation reactions, choose the right variant for completing and balancing the equation, indicating clearly which product is the precipitate. If no reaction would be expected, so indicate. [Review Topics] 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 + NHA 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. NaOH and KOH. [References] 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( CO32), 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
Transcribed Image Text:For each of the following precipitation reactions, choose the right variant for completing and balancing the equation, indicating clearly which product is the precipitate. If no reaction would be expected, so indicate. [Review Topics] 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 + NHA 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. NaOH and KOH. [References] 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide ( S²-), carbonate ( CO32), 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
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