Acids and Bases
Arrhenius: H+ and OH-
Bronsted: Proton acceptors/donors
Lowry: Electron pair acceptors/donors
[Ar]3d5
Determine the anode and cathode reactions for the electrolysis of molten NaCl
Cathode: Na+ (aq) +e- --> Na(s)
Anode: 2Cl- (aq) --> Cl2 (g) +2e-
What is the standard free energy of CaCO3(s) → CaO (s) + CO2(g). Is the reaction spontaneous?
ΔG° = 130.41 kJ not spontaneous
Consider the following reaction:
2 AgNO3 (aq)+Cu (s)2 Ag (s)+Cu(NO3)2 (aq).
What is being oxidized and what is being reduced?
Cu is being oxidized and Ag is being reduced
Is NH4CN acidic basic or neutral?
Basic
How many atoms does a face-centered unit cell contain? Assume there's only face centered atoms
3
Determine the anode and cathode reactions for the electrolysis of a molten mixture of NaCl and CsI
Cathode: Cu+(aq) + e- → Cu(s)
Anode: 2I-(aq) → I2(s) + 2e-
What is the standard change in entropy for 2CO (g) + O2 (g) ⇌ 2CO2 (g)?
ΔS° = -173.27 J/mol K
Balance the following redox reaction in basic solution:
MnO4 - (aq)+I - (aq)I2 (aq)+Mn 2+ (aq)
2 MnO4 -+8 H2O+10 I -2 Mn 2++5 I2 +16 OH -
A 0.054 M solution of a weak base has a pH of 8.63. What is the Kb value for the unknown weak base?
3.38x10-10
A solution of [CrF6]3- is orange. What is a likely color for a solution of [Cr(NH3)6]3+?
Yellow
Determine the anode and cathode for the electrolysis of a molten mixture of KBr and LiF
Cathode: K+(aq) + e- → K(s)
Anode: 2Br-(aq) → Br2(l) + 2e-
Consider the following reaction: CH4 (g) + 8O2 (g) → CO2 (g) +2H2O (g) + 4O3 (g). At what temperature does its spontaneity switch from what is observed at standard conditions?
-827 ℃
What is the standard cell potential for a galvanic cell that consists of Au3+/Au and Ni2+/Ni half cells?
E cell= 1.77V
What is the pH of a solution where 3.33g of potassium acetate (C2H3O2K) is dissolved in 3.50L of water?
pH = 8.37
An X-ray beam with a λ =154pm incident on the surface of a crystal produced a maximum reflection angle of θ =28.3. Assuming n=1 calculate the separation between layers of atoms in the crystal.
d=162pm
Determine the anode and cathode for the electrolysis of a aqueous mixture of PbCl2
Cathode: Pb2+(aq) + 2e- → Pb(s)
Anode: 2H2O(l) → O2(g) + 4H+(aq) + 4e-
Calculate the gibbs free energy change for: glutamate + NH3 → glutamine + H2O if the reaction occurs at 68 °C, has a change in heat of 4103 kJ/mol, and a change in entropy of 273 J/mol K
ΔG = 4009.907 kJ
Consider the following reaction:
2 AgNO3 (aq)+Cu (s)2 Ag (s)+Cu(NO3)2 (aq)
What is the standard voltaic cell voltage?
E cell= 0.460 V
What mass of HCOONa (68.0069 g/mol) do you need to add to 400. mL of 1.00 M formic acid for a pH 3.50 buffer. (Ka=1.77x10-4)
15.2g
An X-ray beam of an unknown wavelength is diffracted from an NaCl surface. If the interplanar distance in the crystal is 286pm and the angle of maximum refraction is found to be 7.23, what is the wavelength of the X-ray beam if we assume n=1?
wavelength = 72pm
Determine the anode and cathode reactions for the electrolysis of aqueous K2SO4
Cathode: SO42-(aq) + 4H+ + 2e- → H2SO3(aq) + H2O(l)
Anode: O2(g) + 4H+(aq) + 4e- → 2H2O(l)
In the following reaction: 2KClO3(s) → 2KCl(s) + 3O2(g), ΔG° = -226 kJ/mol. The standard free energy of formation for KCl = -409 kJ/mol. What is the standard free energy of formation for KClO3(s)?
ΔG°KClO3 = -296 kJ
Find the cell potential of a galvanic cell based on the following half reactions at 25 C with [Cd2+]=0.050M and [Sn2+]=0.200M
Cd2+ +2e- --> Cd E=-0.403V
Sn2+ +2e- --> Sn E=-0.137V
Will the reaction occur spontaneously?
Reaction will be spontaneous