Thallium (Tl) is a heavy element used in the electronic industry. The reduction reaction for Tl is Tl+ + e- ® Tl and its exchange current is j0 = 103´[Tl+]1/2 A/m2 when [Tl+] is measured in mol/dm3.

1) explain why the exchange current has the functional form shown above (hint: look up the derivation of the exchange current in the notes and introduce a necessary modification).

2) Calculate and plot the redox current density for this reaction using (a) the Butler-Volmer equation, (b) the linear and (c) the Tafel approximations at overvoltages h between 0 and - 0.2 V for Tl+ concentrations of 1 mM and 1M. Determine the potential ranges where one of the two approximations provide the actual current

What do you mean by related question?

An 18.0 g ice cube initially at -10 Celsius is dropped into 120g of water initiallly at 25 Celsius. What is the final temperature of the system after all of the ice has melted? Assume that no heat is lost to the container or the surroundings

Make a list of the anions of the six strong monoprotic acids discussed in lecture. These anions are said to have no effect on the pH of an aqueous solution. The same is true for solutions of strong bases - their conjugate acids (which are Group 1 or Group 2 cations) are very weak acids, and therefore, have virtually no effect on the pH of the solution.

4. Make a list Group 1 and Group 2 cations, and note that these ions are said to have no effect on the pH of an aqueous solution with the exception of Be2+. The situation is different, however, for the conjugate acid of a weak base, or the conjugate base of a weak acid.

5. A weak base: Write a balanced equation for the protonation of ammonia, using water as a reactant.______________________________________________ a. What species is the conjugate acid of ammonia? ________________ b. The Kb of ammonia is 1.8 x 10-5 . What is the Ka of its conjugate acid? Show work.

6. Hypoiodous acid (HIO) has Ka = 2.3 x 10-11. Which is a stronger acid, HIO or NH4 +? Explain your reasoning. Acids, Bases, Salts and Buffers Prelab Assignment revised by Bruce E. Wilcox, Fall 2017 Name _____________________________ Assignment: Complete this assignment (and the reproduction in your manual) and hand this form in at the beginning of lab. Also copy the work from pages 3 – 4 into your notebook. 2 Now you have seen that the conjugate acid of a weak base can exhibit significant acid behavior. What about the conjugate base of a weak acid?

7. Write the balanced equation for the ionization of nitrous acid in water. _____________________________________________________ a. The Ka of HNO2 is 4.3 x 10-4 . What is the Kb of its conjugate base? Show work.

1. For the compounds present, list all intermolecular forces present and then rank the compounds in order of increasing boiling point (lowest to highest). Hint: draw the structures to make this easier.
   1. Ethane (C₂H₆)
   2. Ethanol (C₂H₅OH)
   3. Acetic acid (CH₃COOH)
   4. Dimethyl ether (C₂H₆O)

For the diprotic weak acid H2A, Ka1 = 3.1 × 10-6 and Ka2 = 5.4 × 10-9. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?

pH of Aqueous Sulfuric Acid Calculate the pH of a 2.07×10-3 M solution of H2SO4. (Ka = 0.0120 for HSO4-)

What is the probability of finding the particle in the region a/4 < x < a/2? show your work.

For molecule NF3-

a) draw a full MO diagram. All F 2pz LGO are non-bonding. The 2s orbitals are to far from 2p to interact. The e LGO derived from F 2px and 2py orbitals (depends on central atom with e symmetry exist, then the 2py LGO wil either be bonding or not)

b) what are the symmetries of valance orbitals on central N atom

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HF(g) NH4F(s) at 25 °C is 10.2. (a) If the partial pressure of ammonia is PNH3 = 0.553 atm (at equilibrium) and solid ammonium fluoride is present, what is the equilibrium partial pressure in atm of hydrogen fluoride at 25 °C? An excess of solid NH4F is added to a container filled with NH3 at 25 °C and a pressure of 1.09 atm. Calculate the pressures of NH3(g) and HF(g) reached at equilibrium in atm.

At 1 atm, how much energy in kJ is required to heat 85.0 g H 2 O ( s ) at − 10.0 ∘ C to H 2 O ( g ) at 167.0 ∘ C? Use the heat transfer constants found in this table.

a.) What is the order of this reaction?

b.) What is the value of the rate constant for this reaction?

Express your answer to three significant figures and include the appropriate units.

Consider the titration of a 22.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH. What is the pH after adding 4.00 mL of base beyond the equivalence point?

2)

A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M HCl.

Determine the following quantities:

a)

The initial pH of the KOH solution before any acid is added.

b)

The pH of the solution after 3.00 mL of HCl is added.

c)

The quantity of HCl solution required to reach the equivalence

point.

d)

The pH of the solution at the equivalence point.

e)

The pH of the solution after20.0 mL of HCl is added.