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Unit 6: Acids and Bases
Guiding Questions:
- What is an acid?
- What makes acids dangerous?
- Is acid rain an issue for us?
- What does pH balanced mean?
What you should learn:
- Acids are essential for life, are commonly found in the home, and have a myriad of uses outside the home.
- The strength of an acid is determined by its electron structure
- Acids can cause chemical changes by breaking or weakening chemical bonds.
More Specifically...:
IB Objectives: SL
Option (A.5)
HL
- Properties and Theory
- List general properties of acids and bases (Including bases which are not hydroxides such as ammonia, soluble carbonates and hydrogen carbonates)
- a. Effect on indicators
- b. Reaction of acids w/ bases, metals and carbonates
- Compare Arrhenius and Brönsted-Lowry theories of acids
- Classify acids and bases as Arrhenius or Brönsted-Lowry
- Identify acid base conjugate pairs
- Convert between chemical formula and name using acid naming rules
- State the expression for the ionic product constant of water (Kw)
- Deduce [H+] and [OH-] for water at different temperatures given Kw
- Define pH, pOH, and pKw
- Distinguish between strong and weak acids in terms of
- a. degree of ionization/dissociation
- b. conductivity
- c. Ka
- d. pH
- e. pKa
- State whether a given acid/base is strong or weak
- a. Strong: hydrochloric acid, nitric acid, sulfuric acid, all group 1 hydroxides and barium hydroxide
- b. Weak: Ethanoic acid, carbonic acid, ammonia and ethylamine
- State the equation for the reaction of any weak acid or waek base with water and hence derive the ionization constant expression
- State and explain the relationship between Ka and pKa
- Write and balance neutralization reaction an acid and base react to form a salt and water
- Describe and explain data from experiments to distinguish between strong and weak acids and bases, and to determine the relative acidities and basicities of substances
- Sketch titration curves and be able to suggest a suitable indicator for a particular titration using a table of indicators
- Distinguish between 'equivalence point' and 'end point'
- Describe a buffer solution in terms of its composition and behavior IBH 9.4.1
- a. Ammonium chloride/ammonia
- b. Ethanoic acid/sodium ethanoate
- c. Blood
- Describe ways of preparing buffer solutions
- Math
- State that each change of one pH unit represents a tenfold change in the hydrogen ion concentration [H+]
- Deduce changes in [H+] when pH of a solution changes by more than one unit
- Calculate pH and pOH, hydrogen and hydroxide ion concentration from specified concentrations
- Apply Ka or pKa in calculations
- Calculate unknown concentration using titration data
- Calculate the pH of a specified buffer system
Lecture Notes:
Assignments:
Labs:
- Titrations using pH probes
- Titration using indicator
- Design a buffer
- Buffer Make-up Lab
- Standardize a base
- Calculate Ka of a weak acid
- Investigate acids/bases/buffers
Resources:
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