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Review of Acids, Bases, & Salts

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Presentation on theme: "Review of Acids, Bases, & Salts"— Presentation transcript:

1 Review of Acids, Bases, & Salts

2 Has H in the formula Produces H+ as the only positive ion in solution
Arrhenius Acid

3 Inorganic – formula starts with H (except H2O & H2O2)
Organic – formula ends with COOH Formula of an Acid

4 Properties of Acids Sour Taste Electrolytes
React with bases to form a salt + H2O Turn litmus RED React with most metals to produce H2(g) Properties of Acids

5 Ionization of an Acid: Why is it so weird?
Because acids are covalent! Ionization of an Acid: Why is it so weird?

6 HCl  H+ + Cl- HCl + H2O  H3O+ + Cl- Ionization of an Acid or
Arrhenius format or HCl + H2O  H3O+ + Cl- Bronsted-Lowry format Ionization of an Acid

7 HCl HNO3 HBr HClO4 HI H2SO4 Six strong acids?

8 Ionization of a weak base: Why is it so weird?
Because weak bases are covalent! Ionization of a weak base: Why is it so weird?

9 Autoionization of water
H2O  H+ + OH- Autoionization of water

10 Arrhenius Base (Strong bases)
Has OH in the formula Produces OH- as the only negative ion in solution Arrhenius Base (Strong bases)

11 LiOH Ca(OH)2 NaOH Sr(OH)2 KOH Ba(OH)2
Six strong bases?

12 Formula of a Strong Base
Has format M(OH)x M is a metal X can be 1, 2, or 3 Formula of a Strong Base

13 Properties of Bases Bitter Taste Slippery Feel Electrolytes
React with acids to form a salt + H2O Turn litmus BLUE Properties of Bases

14 Ionization of a strong base
NaOH  Na+ + OH- Ionization of a strong base

15 Ionization of NH3, a weak base
NH3 + H2O  NH4+ + OH- Ionization of NH3, a weak base

16 Metal + Nonmetal Formula of a Salt

17 Write the formula of potassium sulfate
K+ & (SO4)2- K2SO4 Write the formula of potassium sulfate

18 Electrolytes Solutions conduct – they contain ions
Acids (HX), bases (MOH), & salts (MX) are electrolytes Electrolytes

19 Solutions of covalent compounds (all nonmetals), excepting the acids and the weak bases.
They do NOT conduct. NONelectrolytes

20 Identify the electrolytes
Yes - B Yes - B LiOH CH3COOH C6H12O6 NaNO3 H2SO4 CH3OH Ca(OH)2 HCl C8H18 Al(OH)3 HNO3 CH3CH2COOH K2SO4 CH3CHOHCH3 CH3OCH3 H3PO4 Mg(OH)2 CH3CH2OH Yes - A Yes - A Yes - A No Yes - S Yes - S Yes - A No No No Yes - A Yes - B Yes - A Yes - B No No

21 0-14 Acidic: 0 to 7, Neutral: 7 Basic: 7-14
pH scale

22 pH = -log[H+] pH = ?

23 How do you get [H+] from pH?
[H+] = 10-pH How do you get [H+] from pH?

24 pOH = -log[OH-] pOH = ?

25 pK = -log[K] pK = ?

26 pH = 0 Most acidic on pH scale

27 pH = 14 Most basic on pH scale

28 Hydroxide ion OH-

29 Hydrogen ion or Proton H+

30 Hydronium ion. Bronsted-Lowry form of H+. Used interchangeably with H+ .
H3O+

31 [H+]  [OH-] Acidic Solution

32 [OH-]  [H+] Basic Solution

33 14, at 25C pH + pOH = ?

34 If the pH changes from 3 to 5, how does the [H+] change?
The pH changes by 2, so the [H+] changes by 102 or 100X. Since the pH went up, it became LESS acidic. The new solution has a [H+] 100 times less than the original solution. It is 1/100 of the original [H+]. If the pH changes from 3 to 5, how does the [H+] change?

35 How can pH be safely tested?
Instrumental – use pH meter Indicators – use a series of indicators to narrow down the pH range Test acids with metals (NOT Cu, Ag, or Au) How can pH be safely tested?

36 Proton Donor Bronsted-Lowry Acid

37 Proton Acceptor Bronsted-Lowry Base

38 Bronsted-Lowry Acids & Bases
HCl + H2O  H3O+ + Cl- Acid Base c. acid c. base Bronsted-Lowry Acids & Bases

39 Complete or almost complete ionization.
Strong Acids & Bases

40 Concentration of ions in .4 M HCl
Strong acid HCl  H+ + Cl- Concentration of H+ = 0.4 M Concentration of Cl- = 0.4 M Concentration of ions in .4 M HCl

41 Ionization occurs only to a slight extent, a few percent.
Weak Acids & Bases

42 Reactions of Acids with Metals
Metal + Acid  H2(g) + salt Reactions of Acids with Metals

43 Zn(s) + 2HCl  H2(g) + ZnCl2 Zn(s) + HCl  ?

44 2Al(s) + 6HCl  3H2(g) + 2AlCl3 Al(s) + HCl  ?

45 Neutralization Reactions
Acid + Base  Salt + H2O Neutralization Reactions

46 H+ + OH-  H2O Net Ionic Equation for strong acid/strong base Neutralization Reactions

47 Moles H+ = Moles OH- At equivalence point

48 Molarity = Moles solute
Liters of soln Molarity (M)

49 NYS Titration Equation
MaVa = MbVb This equation only works when the number of H’s on the acid EQUALS the number of OH’s on the base! NYS Titration Equation

50 naMaVa = nbMbVb Titration Equation
This equation works when the number of H’s on the acid does NOT equal the number of OH’s on the base! na = number of acidic H’s in acid. nb = number of OH’s in base. Titration Equation

51 -log[H+] or –log[H3O+] pH

52 -log[OH-] pOH

53 Equilibrium Constant Expression for aA(aq) + bB(aq)  cC(aq) + D(aq)
[C]c[D]d [A]a[B]b K = Equilibrium Constant Expression for aA(aq) + bB(aq)  cC(aq) + D(aq)

54 Equilibrium Constant Expression for aA(s) + bB(aq)  cC(s) + D(aq)
[D]d [B]b K = Equilibrium Constant Expression for aA(s) + bB(aq)  cC(s) + D(aq)

55 -logK pK

56 14 pOH + pH =

57 1.0 X 10-14 [OH-] X [H+] =

58 The pH = The pOH = The [OH-] =
3 11 1 X 10-11 If the [H+] = 1 X 10-3

59 Substance that changes color over a narrow pH range.
Indicator

60 Molarity H2SO4 Vs. Molarity H+
H2SO4  2H+ + SO42- [H+] = 2[H2SO4] 2M H2SO4  4M H+ Molarity H2SO4 Vs. Molarity H+

61 naMaVa = nbMbVb (1)X(20.0 mls) = (1).250M(50.0mls)
What is the concentration of a hydrochloric acid solution if 50.0 mL of a M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration?

62 (1.50 M)(10.62 mls) = X(20.20 mls) Acid 1.50 M Base ? M Final Volume
16.07 24.25 Initial Volume 5.45 4.05 Amount Used 10.62 20.20 (1.50 M)(10.62 mls) = X(20.20 mls)

63 Why do different salts produce solutions with different pHs?
Hydrolysis of the ions! Why do different salts produce solutions with different pHs?

64 Reaction of ions with water to produce H+ or OH-
Hydrolysis

65 Which anions undergo hydrolysis?
Anions of weak acids: they produce basic solutions. C2H3O H2O  HC2H3O2 + OH- Which anions undergo hydrolysis?

66 Which cations undergo hydrolysis?
Cations of weak bases: They produce acidic solutions. NH H2O  H3O+ + NH3 Which cations undergo hydrolysis?


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