Titration
Which of the following statements is true of titrations? Select ALL correct answers.
A. The equivalence point of the titration is where the moles of acid (or base) in the sample have been completely reacted by the moles of added base (or acid)
B. A strong base can be titrated by a strong acid
C. A weak acid can be titrated by a weak base
D. Equivalence point of titrations are often estimated using color indicators
A,B,D
What are the 3 types of titrations?
1. strong acid/strong base
2. weak acid/ strong base
3. weak base/ strong acid
Smaller Ksp = less soluble
Consider a reaction that has a negative ΔH and a negative ΔS. Which of the following statements is true?
A. The reaction will be spontaneous at all high temperatures
B. The reaction will be spontaneous at high temperatures
C. The reaction will be spontaneous at low temperatures
D. The reaction will be nonspontaneous at all temperatures
C
In the balanced reaction below, which element is the reducing agent?
Au3+ + MnO2 + 2H2O → Au + MnO4- + 4H+
Mn
50.0 mL of an HCl solution required 50.0 mL of 0.100 M NaOH to reach the equivalence point of a titration. What was the pH of the solution at the equivalence point?
7
What is Ksp?
solubility product constant
Which solution (basic or acidic) does solubility increase?
Acidic
Place the following compounds in order of decreasing standard molar entropy.
Ar (g), F2 (g), Ne (g), H2O2 (g)
H2O2 > F2 > Ar > Ne
In the balanced reaction below, which species is oxidized?
F2 + 2MnO42- → 2F- + 2MnO4-
Mn
50 mL of NaOH solution required 30 mL of 0.30 M HCl to reach the equivalence point of a titration.
Find initial pH
13.26
What is the common ion effect?
the solubility decreases if the solution contains a common ion
What is the Ksp expression for PbI2?
Ksp = [Pb2+] [I-]2
Calculate ΔGrxn° for the first reaction below, given values of ΔGrxn° for two other reactions.
2KClO3 (s) + 5H2 (g) → 2K (s) + Cl2O (g) + 5H2O (l) ΔGrxn° = ??
K (s) + 3H2O (l) + ½ Cl2 (g) → KClO3 (s) + 3H2 (g) ΔGrxn°=+415.0 kJ
H2 (g) + Cl2O (g) → H2O (l) + Cl2 (g) ΔGrxn°= - 335.0 kJ
-495 kJ
-255 kJ
80 kJ
-750 kJ
-495 kJ
Balance the redox reaction below in a basic solution.
BrO3- + I- → Br - + I3-
9I- + 3 H2O + BrO3- -- >Br- + 6OH- + 3I3-
45.0 mL of 0.100 M acetic acid was titrated using 0.150 M NaOH. What was the pH of the solution after adding 15.0 mL of NaOH?
4.74
Which law of thermodynamics states that entropy can have a true value of zero?
Third
The Ksp of PbI2 is 2.00. Determine the molar solubility.
0.79 M
60 mL of 0.15 M NaOH solution required 30 mL of 0.30 M HCl to reach the equivalence point of a titration. What was the pH of the solution after adding 40.0 mL of HCl?
1.52
Which of the 3 delta G rxn formulas can ONLY be used at 25 C?
delta G rxn = products - reactants
The solubility of BaCO3 is 5.00 M. Determine Ksp.
25