1
Q
pH titration curve
A
2
Q
what is the equivalence point?
A
the volume of one solution that exactly reacts with the volume of the other
3
Q
what is the end point of a titration?
A
when [HA] = [A-]
4
Q
how do you choose an indicator from a curve?
A
match the vertical section with the pH range of the indicator
Chemistry Module 5
flashcards
Decks in class (33)
# Cards
-
18.1 Orders and rate constants6
-
18.2 Concentration-time graphs10
-
18.3 Rate-concentration graphs8
-
18.4 Rate determining step4
-
18.5 Rate constants and temp13
-
chpt 18 graphs5
-
19.1 K꜀ constant3
-
19.2 Kₚ constant4
-
19.3 Controlling the position of the equilibrium10
-
20.1 Bronsted-Lowry acids and bases13
-
20.2 The pH scale and strong acids6
-
20.3 Kₐ constant12
-
20.4 The pH of weak acids6
-
20.5 pH and strong bases4
-
21.1 Buffer solutions16
-
21.2 Buffer solutions in the body7
-
21.3 Neutralisation4
-
22.1 Lattice enthalpy8
-
22.2 Enthalpy changes in solution9
-
22.3 Factors affecting lattice enthalpy8
-
22.4 Entropy9
-
22.5 Free energy11
-
23.2 Manganate (VII) redox titrations6
-
23.3 Iodine/thiosulfate redox titrations11
-
23.4 Electrode potentials28
-
23.5 Predictions from electrode potentials4
-
23.6 Fuel cells12
-
24.1 d-block elements25
-
24.2 complex ions11
-
24.3 stereoisomerism in complex ions9
-
24.4 ligand substitution and precipitation39
-
24.5 redox and qualitative analysis20
-
24.5 redox and qualitative analysis29
