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Acids, Bases, and SALTS

Acids, Bases, and SALTS. According to Arrhenius theory, Acid + base  salt + water Examples: HCl + NaOH  NaCl + H 2 O H 2 SO 4 + Sr(OH) 2  SrSO 4 + 2H 2 O. SALTS ~ Defined. The relationship between salts and pH. There are six strong acids~

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Acids, Bases, and SALTS

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  1. Acids, Bases, and SALTS According to Arrhenius theory, Acid + base  salt + water Examples: HCl + NaOH  NaCl + H2O H2SO4 + Sr(OH)2 SrSO4 + 2H2O

  2. SALTS ~ Defined

  3. The relationship between salts and pH There are six strong acids~ HCl, HBr, HI, H2SO4, HNO3 HClO4 There are six strong bases~ LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2,Ba(OH)2 All other acids and bases are considered weak and do NOT dissociate completely.

  4. Therefore when an acid and base are combined the final pH will depend on which of the reactants is strong or weak. • Strong acid + strong base  neutral salt + H2O • The acid and base will neutralize each other and create a solution with pH 7. • Strong acid + weak base  salt and water (pH < 7)‏ • Because the weak base doesn’t completely dissociate, the H1+ ions will prevail in determining pH. • Weak acid and strong base  salt and water (pH> 7)‏ • Because the weak acid doesn’t completely dissociate, the OH1- ions will prevail in determining pH.

  5. What happens when you put a salt in water? You would think that putting a salt in water would have nothing to do with acids or bases and pH, but that is NOT the case. NaCl + H2O  H1+(aq) + Cl1-(aq) + Na1+(aq) + OH1-(aq) The hydrogen from the strong acid and the hydroxide from the strong base neutralize each other. Here the pH is 7.

  6. Look at what happens with this salt and water combination. NH4Cl +H2O NH4OH(aq) + H1+(aq) + Cl1-(aq)‏ Notice that the product is a strong acid (which completely dissociates) and a weak base (which does NOT completely dissociate). Therefore, the strong acid is the prevailing ionic species and influences the pH. The pH will < pH7. The opposite will be true when the salt is derived from a weak acid and a weak base. The pH will be > pH7. If a salt derived from both a weak acid and weak base (Ex. FeC2O4) is put in water the pH will depend on which was weaker.

  7. Acidic Salts and Basic Salts There is also another class of salts called acidic salts and basic salts. They will also affect pH values. These salts occur when there is NOT complete neutralization of the acid or base. Acidic salt ~ NaHSO4(sodium hydrogen sulfate) (incomplete neutralization of sulfuric acid)‏ Basic salt ~ BaOHCl (barium hydroxide chloride) (incomplete neutralization of barium hydroxide)‏

  8. Acidic and Basic Anhydrides • There is a class of compounds that are neither acids nor bases nor salts, but produce either an acid or base when put in water. • (Basic) Metallic oxides (ex. CaO, Fe2O3, K2O, etc.) are solids that will make a base when put in water (Ca(OH)2, Fe(OH)3, KOH). These anhydrides are all solids. • (Acidic) Non-metallic oxides (ex. CO2, SO2, NO2, etc.) are gasses that will make an acid when put in water (H2CO3, H2SO3, HNO3). These anhydrides are all gasses.

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