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Understanding Electrolytes, Solubility, and Net Ionic Equations in Aqueous Solutions

This comprehensive guide covers the essential concepts of electrolytes, solubility of electrolytes, and the writing of net ionic equations in chemistry. It explains the dissociation of ionic compounds in water, provides solubility guidelines for various compounds, and outlines how to identify soluble and insoluble substances. Additionally, you'll learn the procedure for writing net ionic equations, highlighting the importance of spectator ions. This resource is ideal for students needing to grasp fundamental topics in aqueous chemistry.

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Understanding Electrolytes, Solubility, and Net Ionic Equations in Aqueous Solutions

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  1. Drill – 4/8/08 1. What is an electrolyte? 2. Is a precipitate soluble or insoluble?

  2. Ions in Aqueous SolutionChapter 13, Section 1

  3. Dissociation • The separation of ions that occurs when an ionic compound dissolves. • NaCl (s)  Na+ (aq) + Cl- (aq) • CaCl2 (s)  Ca+2 (aq) + 2Cl- (aq) H2O H2O

  4. H2O • NaCl (s)  Na+ (aq) + Cl- (aq) • 1 mol 1 mol 1 mol • CaCl2 (s)  Ca+2 (aq) + 2Cl- (aq) • 1 mol 1 mol 2 mol • Al2(SO4)3 (s)  2Al3+ (aq) + 3SO42- (aq) • 1 mol 2 mol 3 mol H2O H2O

  5. How many solute ions in each case?

  6. Solubility Guidelines – Use these to determine if an ionic compound is soluble • Na+, K+, and NH4+ compounds are soluble in H2O2 • Nitrates, acetates, and chlorates are soluble. • Chlorides are soluble, except those with Ag+, Hg+, and lead. • Most sulfates are soluble, except those with Ba2+, Sr2+, Pb2+, Ca2+, and Hg+

  7. Solubility Guidelines – Use these to determine if an ionic compound is soluble 5. Most carbonates, phosphates, and silicates are insoluble, except those of Na+, K+, and NH4+ 6. Most sulfides are insoluble, except those of Sr2+, Ca2+, Na+ , K+, and NH4+

  8. Is calcium phosphate soluble or insoluble? • Ca3(PO4)2 • Most carbonates, phosphates, and silicates are insoluble, except those of Na+, K+, and NH4+

  9. We can use this information to predict states of matter. We can determine if a product is either soluble (aq) or insoluble (s).

  10. Net Ionic Equations • Include only those compounds and ions that undergo a chemical change in a reaction in aqueous solution.

  11. How to write net ionic equations 1. Write the chemical equation. 2. Write the state of matter, making sure to identify precipitates (use solubility rules). 3. Convert chemical equations to ionic equations (do not dissociate precipitates). 3. Cancel spectator ions from both sides of the equation. Spectator ions do not take part in the chemical reaction and are found in solution both before and after the reaction.

  12. CdSO4 and H2S • CdSO4 + H2S  CdS + H2SO4 • CdSO4 (aq) + H2S (aq)  CdS (s) + H2SO4 (aq) • Cd2+(aq) + SO42-(aq) + 2H+(aq) + S2-(aq)  CdS(s) + SO42-(aq) + 2H+(aq) • Cd2+(aq) + S2-(aq)  CdS(s)

  13. Practice Problems • Pg. 586 in Blue Chemistry Book # 30, 41, 44, 45

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