Hydrazine, N₂H₄(aq), is used in the preparation of polymers, pharmaceuticals and rocket fuel.  Hydrazine has alkaline properties similar to ammonia and will act as a weak base.  Given that a 100 mL sample of 0.10 mol/L hydrazine solution has a pH of 10.55 at 25.0 ^oC, write the formula for the conjugate acid and calculate the Ka of the conjugate acid.

1. For test tubes 1-5, list the entities initially present. Also, identify the SOA and SRA and predict the spontaneity of the reaction. 

test tube 1: Iron placed in distilled water

Test tube 2: Iron is placed in hydrochloric acid

Test tube 3: Iron is placed in magnesium

Test tube 4: Iron is placed in saltwater

Test tube 5: Iron is placed in de-aerated water

Test tube 6: Iron alone (controlled)

2. Using the SOA and SRA identified in Question 17, write the oxidation and reduction half-reactions and the net reaction for systems 2 and 4.

3. Explain why there was accelarated corrosion in test tube 3

4. Explain why the nails did not corrode in test tubes 4 and 5.

3Cl2 + 6NaOH ‹ 5NaCl + NaClO3 + 3H2O,

Cl2 undergoes

 6 CH₃COOH_(l)  +  11 O_2(g)  →  10 CO_2(g)  +  2 CO_(g)  +  12 H₂O_(g) + 694 kJ

Consider: Cl 2 (g) + PCl (g) ↔ PCl 5 (g)

Initial [ ]’s of Cl 2 and PCl 3 are shown in the following data table and the concentration changes

are recorded at various time periods after the reaction progresses towards equilibrium.

Reaction time (sec) [Cl 2 ] mol/L [PCl 3 ] mol/L [PCl 5 ] mol/L

0 1.00 1.00 0.00

20 0.90 0.90 0.10

40 0.80 0.80 0.20

60 0.75 0.75 0.25

80 0.71 0.71 0.29

100 0.71 0.71 0.29

120 0.71 0.71 0.29

From observing this data table:

C. At 40 seconds which reaction is faster, forward or reverse? ____________________

2ClF3(s) <--> Cl2(g) + 3F2(g)

In order to establish the equilibrium, 5.45g of ClF3(s) was placed into a 500mL flask. When the equilibrium was established the Cl2(g) was measured at 0.0280 mol/L. 

The equilibrium contant for the equilibrium above is a.bc*10-d. The values of a,b,c and d are.

A sample of pure tin metal is dissolved in nitric acid to produce a solution containing Sn²⁺.  This tin solution is  then titrated with a solution of KMnO₄

a.    Complete and balance the overall redox reaction.

How do you comapare the theoretical and expirimental values for decomposatioin of ammonium nitrate

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How would the net cell potential for the following cell be affected if the reduction of tin(II) ions had been selected as the reference half-cell? 

    Mg(s) | Mg(NO3)2(aq) || Cd(NO3)2(aq) | Cd(s)