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ACIDS , BASES , & SALTS

ACIDS , BASES , & SALTS. Properties of Acids. Sour taste Electrolytes: - aq solns that conduct electric current React with bases to form water and salt (Neutralization Reaction) React with most metals to produce H 2 (g) Aci d s turn litmus re d. Electrolyte.

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ACIDS , BASES , & SALTS

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  1. ACIDS,BASES, & SALTS

  2. Properties of Acids • Sour taste • Electrolytes: - aq solns that conduct electric current • React with bases to form water and salt (Neutralization Reaction) • React with most metals to produce H2(g) • Acids turn litmus red

  3. Electrolyte • Substance when dissolved in H2O produces soln that conducts electric current • Separate into ions in aq soln • Acids, bases, & salts are electrolytes MgCl2(s)  Mg+2(aq) + 2Cl-1(aq)

  4. Can metals react with acids? • SeeTable J • All metals above H2 react with acids • SR reactions • Cu, Ag, and Audonotreact with acids

  5. 2HCl + Mg  MgCl2 + H2 • Mg above H2 so reaction proceeds • Single replacement reaction

  6. Properties ofBases • Bitter taste • Slippery or soapy feeling • Electrolytes • React with acids to produce water and salt • Bases turn litmusblue

  7. Formulas of Acids • Format:HX where X = nonmetal (F, Cl, Br, I) or X = negative polyatomic ion Exception: H2O2 • Some acids have 2 or 3H’s • Ex:HF,H2S,H3PO4

  8. Formulas ofBases • Format: MOH where M is metal • Ex: NaOH, Ca(OH)2 • Exception: NH3 and NH4+1 • CH3OH isNOTa base.WHY?

  9. CCl4 HNO3 C5H12 K3PO4 CH3OCH3 LiOH HI (NH4)2SO4 C12H22O11 NO Yes - S Yes - A NO NO Yes - A Yes - B Yes - S NO NO Yes - S Yes - B Yes - A Yes - A Yes - B Yes - B NO NO Identify the Electrolytes • NaCl • C2H5OH • H2SO4 • NaOH • C6H12O6 • CaI2 • HF • Mg(OH)2 • C3H7OH

  10. Acid, Base, or Neutral? • all H2O contains some H+1 & some OH-1 ions • pure H2O: concentrations very low • Neutral solution: [H+1] = [OH-1] • Acidic solution: H+1 > OH-1 • Basic solution: OH-1 > H+1

  11. Water & self-ionization • H2O(l) + H2O(l)  H3O+1(aq) + OH-1(aq) H3O+1 = hydronium ion OH-1 = hydroxide ion • H2O(l)  H+1(aq) + OH-1(aq) H+1 and H3O+1 used interchangeably H+1 called proton or hydrogen ion

  12. Self-ionization of water

  13. Arrhenius Acid • Substance that contains hydrogen & ionizes to produce H+1 ions in aqueous solution HCl(g) + H2O(l) H+1(aq) + Cl-1(aq) HNO3 + H2O(l) H+1(aq) + NO3-1(aq)

  14. Arrhenius Base • substance that contains hydroxide group & ionizes to produce OH-1 ions in aqueous solution NaOH(s)  Na+1(aq) +OH-1(aq)

  15. Arrhenius Salt • Electrolytes where H+1not only positive ion and OH-1not only negative ion formed in aqueous solution Ex: NaCl, CaBr2,KNO3, NH4I

  16. Salts in Water (ionic compounds) • NaCl(s) + H2O(l)  Na+1(aq) + Cl-1(aq) • CaBr2(s) + H2O(l)  Ca+2(aq) + 2Br-1(aq) • Al(NO3)3(s) + H2O(l)  Al+3(aq) + 3NO3-1(aq)

  17. Arrhenius Model has limitations • Don’t always useH2O as solvent • Arrhenius modelonly applies whenH2O is solvent • Doesn’t explain all cases: • NH3 (base) doesn’t contain OH-1 but it produces OH-1

  18. Alternate Theory: Bronsted-Lowry • Acid = a proton donor • All Arrhenius acids = Bronsted-Lowry Acids HX(g) + H2O(l)  H3O+1 + X-1 H+1forms molecule-ion bond with water molecule H3O+1(hydronium ion)

  19. Bronsted-Lowry Acids • HCl + H2O  H3O+1 + Cl-1 • HNO3 + H2O  H3O+1 + NO3-1 • H2SO4 + H2O  H3O+1 + HSO4-1 • H2O + HSO4-1 H3O+1 + SO4-2

  20. Bronsted-Lowry Base • Base = proton acceptor OH-1 is base • Not restricted to aqueous solution NH3 + H2O  NH4+1 + OH-1 NH3 is a base!

  21. Bronsted-Lowry Acids & Bases

  22. Amphoteric • Substance that acts as both acid & base

  23. Water is amphoteric!

  24. HX(g) +H2O(l)  H3O+1 + X-1 (base) NH3 +H2O NH4+1 + OH-1 (acid)

  25. Naming Acids & Bases

  26. Naming Binary Acids • Hydro + stem of nonmetal + ic HF = ? HCl = ? H2S = ? Hydrofluoric acid Hydrochloric acid Hydrosulfic acid

  27. Naming Ternary Acids • Name derived frompolyatomicanion(see Table E) • Replace –itewith–ous, add acid HNO2 • Replace–atewith–ic, addacid HNO3 nitrous acid nitric acid

  28. Ternary Acids polyatomics with S and P, make stem long again • H3PO4 = phosphoric acid, not phosphic acid • H2SO4 = sulfuric acid, not sulfic acid • H2SO3 = sulfurous acid, not sulfous acid • SEE TABLE K

  29. NamingBases • Name the metal + hydroxide NaOH = ? Ca(OH)2 = ? Mg(OH)2 = ? Sodium hydroxide Calcium hydroxide Magnesium hydroxide

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