ICE Charts: Acid and Base
Redox reaction questions
Balancing half reactions
Galvanic cells
Standard potential
100
To 1.00 L of 0.200 M HClO(aq), add 0.125 mole NaOH(s), which completely dissolves.
(a) Write the balanced net ionic equation for this process at 25°C.
HClO(aq) + OH-(aq) --> ClO-(aq) + H2O(l)
100
Which is the reducing agent and oxidizing agent:
2 Na(s) + Cl2(g) → 2 NaCl(s)
Na is the reducing agent
Cl2 is the oxidizing agent
100
Cu + NO3- --> Cu2+ + NO
3Cu + 2NO3- + 8H+ --> 3Cu2+ + 2NO +4H2O
100
Which component contains electrolytes which are required to complete the circuit in a galvanic cell?
what are salt bridge
100
Find the standard cell potential for an electrochemical cell with the following cell reaction.
Zn(s) + Cu2+(aq) 
Zn2+(aq) + Cu(s)
- Eoreduction of Cu2+ = + 0.339 V
Eoreduction of Zn2+ = - 0.762 V
Eocell = + 1.101 V
200
To 1.00 L of 0.200 M HClO(aq), add 0.125 mole NaOH(s), which completely dissolves. For the chemical process,
HClO(aq) + OH-(aq) --> ClO-(aq) + H2O(l)
Determine the value of the equilibrium constant K. (Kw = 1.00 × 10-14) Ka(HClO) = 3.00 × 10-8.
K= 3.0 x 106
200
what is the oxidation number for Na3Co(NO2)6
Na= +1, Co= +3, N=+3, O= -2
200
Mn2+(aq) + BiO3–(s) → Bi3+(aq) + MnO4− (aq)
14H+ + 5BiO3- + 2Mn2+ --> 5Bi3+ + 7H2O + 2MnO4-
200
In galvanic cell in which electrode reduction occurs?
cathode
200
Rank the following from the weakest to the strongest oxidizing agent.
Cl2,I2, Zn2+,Na+, Ni2+
Na+,Zn2+,Ni2+, I2, Cl2
300
Estimate the pH of a 0.200 M HClO(aq) solution at 25°C. At 25°C, Ka(HClO) = 3.00 × 10-8.
Identify the approximation(s) (assumption(s)) you make.
pH= 4.11
300
Identify the species being oxidized and reduced in each of the following reaction:
Cr+ + Sn4+ 
Cr3+ + Sn2+
oxidized: Cr+
reduced: Sn4+
300
Al(s) + 2H+(aq)+ 2Cl- ---> Al3+(aq) + H2(g) + 2Cl- (aq)
2 Al(s) + 6H+(aq) --> 2Al3+(aq) + 3H2(g)
300
Which kind of reaction occurs at anode?
oxidation
300
Rank the following from weakest to strongest reducing agent: Cl2,I2, Zn2+,Na+, Ni2+
Cl2, I2, Ni2+, Zn2+, Na+
400
To 1.00 L of 0.200 M HClO(aq), add 0.125 mole NaOH(s), which completely dissolves. Estimate the pH of this solution at 25°C.
pH= 7.75
400
Balance the equation, Identify the reactant oxidized and the reactant reduced.
____ AlCl3 (aq) + ____ Mg (s) → ____ Al (s) + ____ MgCl2 (aq)
2 AlCl3 (aq) + 3 Mg (s) → 2 Al (s) + 3 MgCl2 (aq)
Al3+ in AlCl3(aq) is the reactant reduced.
Mg(s) is the reactant oxidized.
400
As2O2 + NO3- --> H3AsO4 + N2O3
As2O2 + 2NO3- + 2H2O + 2H+ --> 2H3AsO4 + N2O3
400
Consider a galvanic cell consisting of Cr(s)/Cr3+(aq) (E°red = −0.74 V) and Cu(s)/Cu2+(aq)(E°red = +0.34 V. Which is the cathode?
Cu/Cu2+
400
Co(s) + Fe2+(aq) --> Co2+(aq) + Fe(s)
is the process spontaneous?
EoCo2+/Co = -0.28V
EoFe2+/Fe= -0.447V
Not spontaneous
500
Aniline is an amine that is used to manufacture dyes. It is isolated as anilinium chloride (C6H5NH3)Cl, a salt prepared by the reaction of the weak base aniline and hydrochloric acid. What is the pH of a 0.233 M solution of anilinium chloride. Ka= 2.3 x 10-5
C6H5NH3+(aq) +H2O(l) <--> H3O+(aq)+C6H5NH2(aq)
pH= 2.64
500
Identify which is undergoing reduction and oxidation, and identify the oxidizing and reducing agents.
Cr2O72-(aq) + HNO2(aq) --> Cr3+(aq) + NO3-
reduction: Cr2O72- --> Cr3+
Cr is the oxidizing agent
Oxidation: HNO2 --> NO3-
reducing agent
500
MnO4-(aq) + Cl-(aq) --> Mn2+(aq) + HClO(aq)
11 H+(aq) +2MnO4-(aq) + 5Cl-(aq) --> 2Mn2+(aq)+ 5HClO(aq) + 3H2O(l)
500
For the following voltaic cell: Fe(s)/Fe2+(aq) (E°red= -0.440) and Cu2+(aq)/Cu(s) (E°red=0.337)
Draw a cell including the salt bridge
Label oxidation and reduction, anode and cathode. Label the e- flow.
Write the overall cell reaction and determine the standard emf (V).
emf= 0.777V
500
What is the standard potential for the following reaction at 25 °C? Is it spontaneous?
2Ag+(aq)+Fe(s)⇋2Ag(s)+Fe2+(aq)
+1.247 V, spontaneous