Net Ionic Reactions. The reaction between strong acids and strong bases is one example:
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1 Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you focus on the chemical reactions that are occurring, and can emphasize general chemical trends. The reaction between strong acids and strong bases is one example: Reaction: HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) Complete: H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq) Na + (aq) + Cl - (aq) + H2O (l) Net: H + (aq) + OH - (aq) H2O (l) The formation of a precipitate from solutions of strong electrolytes is another: Reaction: 2Na3PO4 (aq) + 3Ba(NO3)2 (aq) 6NaNO3 (aq) + Ba3(PO4)2 (s) Complete: 6Na + (aq) + 2PO4 3- (aq) + 3Ba 2+ (aq) + 6NO3 - (aq) Ba3(PO4)2 (s) + 6Na + (aq) +6 NO3 - (aq) Net: 3Ba 2+ (aq) + 2PO4 3- (aq) Ba3(PO4)2 (s) Critical Thinking Questions 1. Verify that all of the reactions in Model 1 are balanced. 2. Is the following statement true or false? Explain. If the same chemical shows up on both sides of a chemical reaction, it doesn t react. 3. Do the coefficients of the chemical species that are crossed out in the reactions match when comparing the reagent and product coefficients?
2 Information: The net ionic reaction for a strong acid reacting with a strong base containing hydroxide is: H + (aq) + OH - (aq) H2O (l) Critical Thinking Question 4. Write balanced reactions for the following strong acid-strong base reactions. Verify that the net ionic equation given above is correct. a) Hydrochloric acid and barium hydroxide b) Sulfuric acid (1 st proton) and potassium hydroxide c) Hydrobromic acid and sodium hydroxide 5. Do the concentrations of the spectator ions in these reactions increase, decrease, or stay the same? Information Solubility Rules in Water The solubility rules for ionic compounds are given in Table 10.9 (pg. 329) of McQuarrie, etal. 1. Most alkali metal (Group 1) and ammonium salts are soluble. 2. Most nitrates, perchlorates, and acetates are soluble. 3. Most halides (Group 17) are soluble, except silver, lead, and mercury (I) halides. 4. Most sulfates are soluble, except sulfates of calcium, barium, and strontium. 5. Most carbonates, chromates, sulfides, oxides, phosphates, and hydroxides are insoluble, except hydroxides of Group 2.
3 Insoluble compounds will form precipitates from the ions in solution. For example, when potassium iodide is mixed with lead(ii) nitrate, solid lead(ii) iodide forms: Molecular Reaction: 2KI (aq) + Pb(NO3)2 (aq) 2KNO3 (aq) + PbI2 (s) Complete Ionic Reaction: 2K + (aq) + 2I - (aq) + Pb 2+ (aq) + 2NO3 - (aq) PbI2 (s) + 2K + (aq) + 2NO3 - (aq) Net Ionic Reaction: Pb 2+ (aq) + 2I - (aq) PbI2 (s) Critical Thinking Questions 6. Precipitates form when the following aqueous solutions are mixed. Write the balanced chemical and net ionic reactions for each. Label all phases. a) Sodium chloride and silver chloride: b) Ammonium chromate and iron(iii) nitrate: c) Potassium phosphate and copper(ii) nitrate d) Copper(II) iodide and ammonium carbonate
4 Model 2 Putting it all together. When ml of M sodium chloride is mixed with ml of M lead(ii) nitrate, solid lead(ii) chloride forms a precipitate. 2NaCl (aq) + Pb(NO3)2(aq) 2NaNO3 (aq) + PbCl2 (s) Before mixing: After mixing: moles Na moles Na moles Cl - 0 moles Cl moles Pb = moles Pb moles NO moles NO moles PbCl2 or g Critical Thinking Questions. 7. Write the net ionic equation for this reaction. 8. Verify the moles of each reactant before mixing. 9. Verify the moles of all the species, and the mass of solid, after mixing. 10. What are the molar concentrations of the ions remaining in solution after mixing?
5 Exercises 1. Complete and balance each of the following acid-base neutralization reactions. Name the products, and write the net ionic equations. a) HBr (aq) + KOH (aq) b) HNO3 (aq) + Ba(OH)2 (aq) 2. Determine if a precipitate forms for the following. If one does, write balanced chemical and net ionic reactions: a) NiCl2 (aq) + NH4NO3 (aq) b) FeCl2 (aq) + Na2S (aq) c) MgSO4 (aq) + AgNO3 (aq) 3. How many milliliters of M HNO3 are needed to neutralize each of the following solutions? a) 45.0 ml M KOH b) 58.5 ml M Al(OH)3 c) 34.7 ml M NaOH 4. Calculate the mass of MgCO3 precipitated by mixing 10.0 ml of a M Na2CO3 solution with 5.00 ml of M Mg(NO3)2 solution. Problems 1. The solubility of magnesium hydroxide (Mg(OH)2) in water is g/100.0 ml. What volume of M HCl is needed to neutralize 1.00 L of a saturated Mg(OH)2 solution? 2. Phosphate can be removed from drinking water supplies by treating the water with Ca(OH)2. How much Ca(OH)2 is required to remove 90% of the PO4 3- from L of drinking water containing 25 mg/l PO4 3-? 5 Ca(OH)2 (aq) + 3 PO4 3- (aq) Ca5(PO4)3OH (s) + 9 OH - (aq)
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