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Understanding Acids, Bases, and Salts: Properties and Reactions

Explore the properties, ionization, and dissociation of acids and bases, along with the preparation of salts through neutralization reactions. Learn about conducting solutions, pH scales, and the importance of buffers in maintaining pH balance.

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Understanding Acids, Bases, and Salts: Properties and Reactions

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  1. Ch # 6 Acids, Bases and Salts

  2. ACIDS • An acid “is a hydrogen-containing substance that produces hydrogen ions” in water.(Hydronium ion: H3O+) • An aqueous solution that contains more H+ ions than OH- ions is ‘acidic’

  3. ACID PROPERTIES • Sour taste (think lemons and sour candies) • Change the color of litmus from blue to red.

  4. Acid Properties (cont.) • React with a base to produce water and salt in a double displacement neutralization reaction. • React with metals such as zinc and magnesium to produce hydrogen gas in a single replacement reaction.

  5. BASES • An base is a hydroxide-containing substance that dissociates to produce hydroxide ions in aqueous solution. • An aqueous solution that contains more OH- ions than H+ ions is ‘basic’

  6. BASE PROPERTIES • Bitter or caustic taste. • A slippery, soapy feeling. • The ability to change litmus red to blue. • The ability to interact with acids in a neutralization reaction to produce water and salt.

  7. Ionization/Dissociation. • Ionization: A process in which ions are produced from a molecular compound when dissolved in a solvent. ACIDS • Dissociation: A process in which already existing ions in an ionic compound separate when an ionic compound is dissolved in a solvent. BASES

  8. Amphoteric substances • Glycine • Hydrogen carbonate

  9. Other kinds of acids and bases • FeCl3A metal ion that is acidic • CO32- An anion that is basic • NH4+A cation that is acidic

  10. Salts • A salt is an ionic compound containing a metal cation and a nonmetal anion • Produced in a neutralization reaction: HCl + NaOH H2O + NaCl

  11. 6.3 Conductance of A, B, S Solutions • Strong electrolyte • Weak electrolyte • Non-electrolyte

  12. 6.4 Dissociation of A & B • Strong acids & bases – strong electrolyte • Weak acids & bases – weak electrolyte

  13. 6.5 Buffers • A solution that resists major changes in pH when small amounts of acid or base is added to it.1) A substance to react with and remove added base. • 2) A substance to react with and remove added acid. • 3) weak acid-salt.

  14. 6.6 pH and Acidic / Basic Solutions

  15. Self ionization of water: • Ion product constant for water: • Kw = [H3O+] [OH-] = 1.00 x 10-14 • If [H3O+] = 7.50 x 10-5 M What is the [OH-] in this solution?

  16. pH = -log [H3O+] = -log [H+]

  17. H3O+

  18. Acidic solution: [H3O+]> [OH-] pH= 0-6 • Basic solution: [H3O+]< [OH-] pH =8-14 • Neutral solution: [H3O+]= [OH-] pH =7 • pH scale: Scale that is used to specify molar hydronium ion concentration in an aqueous solution.

  19. Problems Calculate pH for the following and identify as acidic or basic: [H3O+] = 1 X 10-3 [H3O+] = 1 X 10-9 [OH-] = 1 X 10-4 [H3O+] = 3.9 X 10-5 [H3O+] = 7.9 X 10-11 The number of decimal places of a logarithm is equal to the number of significant figures in the original number.

  20. Problem The pH of a solution is 5.70. What is the molar hydronium ion concentration for this solution? [H3O+] = 10-pH

  21. 6.7 Preparation of Acids • H2(g) + Cl2(g) 2HCl(g) • 2NaCl + H2SO4 2HCl(g) + Na2SO4 • SO2(g) + H2O  H2SO3

  22. 6.8 Preparation of bases: • Alkali metal and water to produce hydrogen and a hydroxide salt. • Ammonia in water • Carbonate in water

  23. 6.9 Preparation of Salts • The reaction of an acid with a base is called a neutralization reaction. In an aqueous solution the products are a salt and water. • Solvay process for making NaHCO3 and Na2CO3 (p226)

  24. Reactions of salts: Reaction with metals: Single replacement reaction according to activity series. • Reaction with acids: Double displacement reaction. A new weaker acid, new insoluble salt, gaseous compound is one of the products. • Reaction with bases: Insoluble precipitate forms, or weaker base. • Reaction of salts with each other: Double displacement reaction. Insoluble salt is formed.

  25. 6.10 Acidic and Basic Salts • Ions that contain H+ • Bases: See Page 213 • Hydroxyapatite Ca5OH(PO4)3 • Reactions: NaHCO3 + NaOH Na2CO3 + H2O

  26. 6.11 Water of Hydration • Water binds to some salts: • These are hydrates. They are used as desiccants (drying agents). • A desiccant is a hygroscopic substance that induces or sustains a state of dryness (desiccation) in its vicinity. • Anhydrous (without water of hydration)

  27. Examples and names CaSO4▪2H2O calcium sulfate dihydrate (gypsum-dry wall, plaster of paris, Dri-rite) CuSO4▪5H2O copper(II) sulfate pentahydrate

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