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IV. Reactions involving Acids and Bases

IV. Reactions involving Acids and Bases. Reactions of Acids with Metals Any metal above hydrogen H in Table J will react with a hydrogen-containing acid to produce H 2 gas and a salt . Zn(s) + __ HCl(aq)  H 2 (g) + _______(aq)

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IV. Reactions involving Acids and Bases

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  1. IV. Reactions involving Acids and Bases • Reactions of Acids with Metals • Any metal above hydrogen H in Table J will • react with a hydrogen-containing acid to produce • H2 gas and a salt. • Zn(s) + __HCl(aq)  H2(g) + _______(aq) • Which of the following metals will react with HNO3 • to produce H2 gas? • Pb Li Cu Fe Ni Al Au • What type of reaction is the above equation? ZnCl2 2

  2. IV. Reactions involving Acids and Bases • Reactions of Acids with Metals • Any metal above hydrogen H in Table J will • react with a hydrogen-containing acid to produce • H2 gas and a salt. • Zn(s) + __HCl(aq)  H2(g) + _______(aq) • Which of the following metals will react with HNO3 • to produce H2 gas? • Pb Li Cu Fe Ni Al Au • What type of reaction is the above equation? ZnCl2 2

  3. metal + acid  H2 + salt ? Which metals ? The active metals can replace H The traditional coinage metals do not replace H!

  4. Neutralization Reactions • Arrhenius + Arrhenius  water + salt • acidbase • For example: • hydrochloric + sodium  water + salt • acid hydroxide • HCl (aq) + NaOH(aq)  H2O(l) + NaCl(aq) • Ex. Write the balanced equation for the neutralization • of nitric acid and potassium hydroxide: • acid + base  water + salt • ____(aq) + ____(aq)  H2O(l) + _____(aq)

  5. Neutralization Reactions • Arrhenius + Arrhenius  water + salt • acidbase • For example: • hydrochloric + sodium  water + salt • acid hydroxide • HCl (aq) + NaOH(aq)  H2O(l) + NaCl(aq) • Ex. Write the balanced equation for the neutralization • of nitric acid and potassium hydroxide: • acid + base  water + salt • ____(aq) + ____(aq)  H2O(l) + _____(aq) HNO3 KOH KNO3

  6. Ex. Write the balanced equation for the neutralization of sulfuric acid and calcium hydroxide: acid + base  water + salt _____(aq) + _____(aq)  __H2O(l) + ______(aq)

  7. Ex. Write the balanced equation for the neutralization of sulfuric acid and calcium hydroxide: acid + base  water + salt _____(aq) + ______(aq)  __H2O(l) + ______(aq) Ex. Write the balanced equation for the neutralization of hydrochloric acid and magnesium hydroxide: acid + base  water + salt ____(aq) + _____(aq)  __H2O(l) + ______(aq) H2SO4 Ca(OH)2 2 CaSO4

  8. Ex. Write the balanced equation for the neutralization of sulfuric acid and calcium hydroxide: acid + base  water + salt _____(aq) + ______(aq)  __H2O(l) + ______(aq) Ex. Write the balanced equation for the neutralization of hydrochloric acid and magnesium hydroxide: acid + base  water + salt ____(aq) + _____(aq)  __H2O(l) + ______(aq) H2SO4 Ca(OH)2 2 CaSO4 Mg(OH)2 2 HCl 2 MgCl2

  9. Adding acid to base is called a neutralization reaction because the H+ ions of the acid and the OH- ions of the base “cancel each other out” as they form H2O. acid + base  water + salt HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq) From acid: From base: H+ + OH-  H2O If the number of H+= number of OH- then the solution is neutral.

  10. C. Net Ionic Equations. HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq) Write out compounds as ions : ___(aq) + Cl-(aq) + Na+(aq) + ___(aq)  H2O(l) + ___(aq) + ____(aq) Note: Na+ and Cl- ions are on both sides of equation. They do NOT take part in the reaction. They are called spectator ions. Cross them out. What is left is called a net ionic equation: H+ (aq) + OH- (aq)  H2O(l) X X H+ OH- X X Na+ Cl-

  11. In reality, the hydrogen ion H+ exists in solution as hydronium ions H3O+, so this equation is often written: H3O+(aq) + OH-(aq)  2H2O(l) All neutralization reactions of acids and bases have the same net ionic equation as the one given above. Ex. Write the net ionic equation for H2SO4(aq) + Ca(OH)2(aq)  2H2O(l) + CaSO4(aq) What are the spectator ions in the above reaction? H3O+ + OH-  2H2O OR H+ + OH-  H2O SO42- Ca2+

  12. A salt is an ionic compound that has… • 1/ …positive ions other than H+, and… • 2/ …negative ions other than OH-. •  Aqueous solutions of salts are electrolytes. • They are named by saying “+” ion, then “-” ion • Ex. Circle the salts in the following list • NaCl NH4NO3 NH3 • HCl CO2 K2Cr2O7 • NaSO4 MnO2 MgCl2 • NaOH CaSO4 Ca(C2H3O2)2 • LiF H2CO3 KBr •  Put an A and B next to any acids or bases above.

  13. These All Form Ionic Compounds.

  14. A salt is an ionic compound that has… • 1/ …positive ions other than H+, and… • 2/ …negative ions other than OH-. •  Aqueous solutions of salts are electrolytes. • They are named by saying “+” ion, then “-” ion • Ex. Circle the salts in the following list • NaCl NH4NO3 NH3 • HCl CO2 K2Cr2O7 • NaSO4 MnO2 MgCl2 • NaOH CaSO4 Ca(C2H3O2)2 • LiF H2CO3 KBr •  Put an A and B next to any acids or bases above.

  15. A salt is an ionic compound that has… • 1/ …positive ions other than H+, and… • 2/ …negative ions other than OH-. •  Aqueous solutions of salts are electrolytes. • They are named by saying “+” ion, then “-” ion • Ex. Circle the salts in the following list • NaCl NH4NO3 NH3 • HCl CO2 K2Cr2O7 • NaSO4 MnO2 MgCl2 • NaOH CaSO4 Ca(C2H3O2)2 • LiF H2CO3 KBr •  Put an A and B next to any acids or bases above. B A B A

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