The document discusses different definitions of acids and bases, including:
1) Arrhenius definitions - acids produce H+ ions in water, bases produce OH- ions. Limited to aqueous solutions.
2) Bronsted-Lowry definitions - acids are H+ donors, bases are H+ acceptors. Acids and bases always come in pairs when reacting.
3) pH scale is used to express acidity because [H+] is usually very small. pH decreases as [H+] increases exponentially. Common substances are classified as acidic, basic, or neutral based on their pH.
Application of Statistical and mathematical equations in Chemistry Part 5Awad Albalwi
Application of Statistical and mathematical equations in Chemistry
Part 5
Strong Acids and Bases
Ph theory
Weak Acids and Weak Bases
Salts of Weak Acids and Bases theory
A buffer solution theory
POLYPROTIC ACID IONIZATION
Application of Statistical and mathematical equations in Chemistry Part 5Awad Albalwi
Application of Statistical and mathematical equations in Chemistry
Part 5
Strong Acids and Bases
Ph theory
Weak Acids and Weak Bases
Salts of Weak Acids and Bases theory
A buffer solution theory
POLYPROTIC ACID IONIZATION
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Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
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Z5e 14.1 658 The Nature of Acids and Bases Alternative link if can’t get through to YouTube: http://dailycackle.com/2007/01/20/science-experiment-gone-wrong/
Z53 Fig. 14.1 659: reaction of HCl and H20
Z5e 660 SE 14.1 a, c, e
Z5e fig. 14.5 p. 661
Z5e 661 14.2 Acid Strength; see Table 14.1
For SE 14.2 -- you need to “remember” that HCl is a strong acid, so Cl - is a weak base (since id does not easily accept a proton (or a H + ). That is, acid strength is inversely proportional to its conjugate base strength.
Z5e 663 SE 14.2
Z5e 663 SE 14.2
Z5e 663 SE 14.2
Rf. Z5e 664 Note: in =m expression, H 2 O (l) is a pure liquid, so constant and drops out of the expression. K w called the ion-product constant (or the dissociation constant)
Rf. Z5e 664 Note: in =m expression, H 2 O (l) is a pure liquid, so constant and drops out of the expression. K w called the ion-product constant (or the dissociation constant)
Z5e 666 SE 14.4
Z5e 664 Fig. 14.7
Z5e 14.3 The pH Scale
Z5e Fig. 14.8 667
Z5e 668. SE 14.6
Z5e 669 Section 14.4: Calculating the pH of Strong Acid Solutions
Z5e 670 SE 14.7b
Z5e 671 Section 14.5: Calculating the pH of Weak Acid Solutions
[H + ] = .0060, so pH = 2.22 pOH = 11.78; [OH - ] = 1.7 x 10 -12 & [H + ] = 6.0 x 10 -3
Z5e 675 Major species: HF, HOC 6 H 5 , H 2 O Since HF is dominant producer of H + , use its Ka Set up “RICE” table, use approximations and 5% rule [H + ] = .030 & pH = 1.53
Z5e 675 Major species: HF, HOC 6 H 5 , H 2 O Since HF is dominant producer of H + , use its Ka Set up “RICE” table, use approximations and 5% rule [H + ] = .030 & pH = 1.53
Rf. Z5e 675 SE 14.9
Z5e 677 [H] = 4.24 x 10 -3 vs. 1.34 x 10 -4 So % dissociation (aka % ionization) = 0.42% vs. 1.3%
Rf. Z5e 680 SE 14.11 Since (X/0.100)(100%) = 8.1%, x = 8.1 x 10 -3 = [H + ] = [A - ], then plug into =m to solve for Ka. Ans. = 6.6 x 10 -4
Z5e 680 fig. 14.10
Z5e 681 Section 14.6 Bases
See next slide for explanation
[hydroxide] = 1.2 x 10 -10
Z5e 688 Section 14.7 Polyprotic Acids
[H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
[H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
[H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
[H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
[H + ] = 7.1 x 10 -2 [H 2 AsO 4 2- ] = 7.1 x 10 -2 also [HAsO 4 3- ] = 8.0 x 10 -8 = Ka 2 [AsO 4 3- ] = 6.8 x 10 -16 Remember: Must consider [H + ] from all sources
Both [H + ] and [HSO4 - ] are 2 M , since completely dissociated.
Both [H + ] and [HSO4 - ] are 2 M , since completely dissociated.
Z5e 694 Section 14.8 Acid-Base properties of Salts
Z5e 695 Write major species Set up =m between anion and water Since product includes hydroxide ion, must use K b so need to convert from K a Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
Z5e 695 Write major species Set up =m between anion and water Since product includes hydroxide ion, must use K b so need to convert from K a Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
Z5e 697
Z5e 697
Z5e 699 Table 14.5
Z5e 701 Section 14.9 The Effect of Structure on Acid-Base Properties
Z5e 702 Figure 14.11
Z5e Section 14.10 Acid-Base Properties of Oxides
Z5e 704 Section 14.11 The Lewis Acid-Base Model
Al ion is Lewis acid and water is Lewis base
Z5e 707 Section 14.12 Strategy for Solving Acid-Base Problems: A Summary
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