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rovide a test (including reagents needed and what to look for if it gives a positive result), and the net ionic equation for the test used, to distinguish berween the following compounds. NiCl, or BaCl, NaC,H,O, or KSCN: ZnS or CuS:

rovide a test (including reagents needed and what to look for if it gives a positive result), and the net ionic equation for the test used, to distinguish berween the following compounds. NiCl, or BaCl, NaC,H,O, or KSCN: ZnS or CuS:

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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### Educational Website Content: Chemical Compound Identification **Objective:** Provide a test (including reagents needed and what to look for if it gives a positive result), and the net ionic equation for the test used, to distinguish between the following compounds. **Compound Pairs:** 1. **NiCl₂ or BaCl₂:** - **Test:** Add sodium sulfate (Na₂SO₄) to the solution. - **Observation:** If a white precipitate forms, it indicates the presence of BaCl₂ due to the formation of barium sulfate (BaSO₄), which is insoluble in water. - **Net Ionic Equation:** \( \text{Ba}^{2+} (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{BaSO}_4 (s) \) 2. **NaC₂H₃O₂ or KSCN:** - **Test:** Add ferric chloride (FeCl₃) to the solution. - **Observation:** Formation of a blood-red solution indicates the presence of potassium thiocyanate (KSCN) due to the formation of iron(III) thiocyanate. - **Net Ionic Equation:** \( \text{Fe}^{3+} (aq) + \text{SCN}^- (aq) \rightarrow \text{Fe(SCN)}^{2+} (aq) \) 3. **ZnS or CuS:** - **Test:** Add hydrochloric acid (HCl). - **Observation:** If the sample dissolves to form a clear solution, it indicates the presence of ZnS. CuS will not dissolve in dilute HCl. - **Net Ionic Equation:** \( \text{ZnS} (s) + 2 \text{H}^+ (aq) \rightarrow \text{Zn}^{2+} (aq) + \text{H}_2\text{S} (g) \) 4. **AgCl or Ag₂O:** - **Test:** Add ammonia (NH₃) to the solution. - **Observation:** Silver chloride (AgCl) will dissolve in excess ammonia, forming a colorless complex. Ag₂O will not dissolve readily. - **Net Ionic Equation:** \( \text{AgCl} (s) +
Transcribed Image Text:### Educational Website Content: Chemical Compound Identification **Objective:** Provide a test (including reagents needed and what to look for if it gives a positive result), and the net ionic equation for the test used, to distinguish between the following compounds. **Compound Pairs:** 1. **NiCl₂ or BaCl₂:** - **Test:** Add sodium sulfate (Na₂SO₄) to the solution. - **Observation:** If a white precipitate forms, it indicates the presence of BaCl₂ due to the formation of barium sulfate (BaSO₄), which is insoluble in water. - **Net Ionic Equation:** \( \text{Ba}^{2+} (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{BaSO}_4 (s) \) 2. **NaC₂H₃O₂ or KSCN:** - **Test:** Add ferric chloride (FeCl₃) to the solution. - **Observation:** Formation of a blood-red solution indicates the presence of potassium thiocyanate (KSCN) due to the formation of iron(III) thiocyanate. - **Net Ionic Equation:** \( \text{Fe}^{3+} (aq) + \text{SCN}^- (aq) \rightarrow \text{Fe(SCN)}^{2+} (aq) \) 3. **ZnS or CuS:** - **Test:** Add hydrochloric acid (HCl). - **Observation:** If the sample dissolves to form a clear solution, it indicates the presence of ZnS. CuS will not dissolve in dilute HCl. - **Net Ionic Equation:** \( \text{ZnS} (s) + 2 \text{H}^+ (aq) \rightarrow \text{Zn}^{2+} (aq) + \text{H}_2\text{S} (g) \) 4. **AgCl or Ag₂O:** - **Test:** Add ammonia (NH₃) to the solution. - **Observation:** Silver chloride (AgCl) will dissolve in excess ammonia, forming a colorless complex. Ag₂O will not dissolve readily. - **Net Ionic Equation:** \( \text{AgCl} (s) +
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