I'm trying to study for my General Chemistry II Exam, but I want to make sure that I don't miss anything important! If you could provide your input on the following concepts, that would be greatly appreciated! Thank you so much!(:

Chapter 17 – Chemical Equilibrium

I. Chemical Equilibria

            A. Equilibrium constant

            B. Homogeneous equilibria

            C. Heterogeneous equilibria

            D. Molar concentrations

            E. Contribution of a pure liquid or a pure solid to the equilibrium constant

            F. Gaseous equilibria

                        1. Relationship between concentration and partial pressure

                        2. Relationship between K_c and K_p

II. Comparing Q and K

            A. Le Chatelier’s Principle

1. Predicting the effects of pressure, volume, concentration changes on equilibrium composition

1(a). Consider the compound with molecular formula C₄H₈O₂. Draw the structures of three isomers that match the following ¹H NMR information.

Isomer A: 1H singlet at 8.2 ppm, 2H triplet at 4.2 ppm, 2H sextet at 1.8 ppm, 3H triplet at 0.9 ppm

Isomer B: 2H quartet at 4.2 ppm, 3H singlet at 2.4 PPM, 3H triplet at 1.2 ppm

Isomer C: 3H singlet at 3.8 ppm, 2H quartet at 2.4 ppm, 3H triplet 1.2 ppm

(b) The mass spectrum of compound A shows molecular ion peak at m/z 88. The IR spectrum of this compound has a broad peak between 3200 and 3550 cm-1. The ¹H NMR spectrum of A shows the following peaks: a triplet at d 0.9, a singlet at d 1.1, one more singlet at d 1.15, and a quartet at d 1.6. The area ratio of these peaks is 3:6:1:2. The ¹³C NMR contains 4 signals. In the space below, propose a structure for A and justify your claim using the data provided.

Determine the pH of a 0.45M solution of Na₂SO₃.

usign the literature value of the acetic acid aand answer the following questions

pKa for acetic acid=4.74 , pH=4.35

Group#1: Buffer pH = 4.00

Group#2: Buffer pH = 4.35

Group#3: Buffer pH = 4.70

Group#4: Buffer pH = 5.00

Group#5: Buffer pH = 5.30

Group#6: Buffer pH = 5.60

1. Explain which group should havethe BEST OPTIMAL BUFFER (see choices above).

2. Explain which group has a buffer that has the HIGHEST BUFFERING CAPACITY AGAINST NaOH.

3. Explain which group has a buffer that has the HIGHEST BUFFERING CAPACITY AGAINST HCl.

4. Is the best optimal buffer the same as the buffer that has the HIGHEST buffer capacity againstNaOH? Explain your reasoning.

5. Is the best optimal buffer the same as the buffer that has the HIGHEST buffer capacity against HCl? Explain your reasoning.

Use the Heisenberg uncertainty principle to explain why does the harmonic oscillator have a zero point energy, but the rigid rotor does not?

In transcription what is the open complex?

Which pair of atoms will likely form a polar covalent bond?

Question 5 options:

Use bond-energy data to calculate the enthalpy of formation for eah of the following compounds at 25 C

a) n-Octane, C8H18(g)

b) Napthalene, C10H8(g)

c) Formaldehyde, H2CO(g)

d) Formic acid, HCOOH(g)

Give the most likely reason for the largest discrepancies between your calculated values and the ones in the tables.

Treatment of a 0.2496-g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.2852 g of AgCl. Calculate the percentage of KCl in the sample?

%?

What is “hardness” and how is it measured?

1. If you have 10.0g of each reactant, determine the limiting reagent and the amount of H₂O produced.

MnO₂ (s) + H₂SO₄ (l) ---> Mn(SO₄)₂ (s) + H₂O (l)

Can you go over each step?

Describe the procedure you would follow to determine the concentration of Vitamin C in a sample if the volume of DCPIP required to reach the endpoint was more than the 25-mL flask could hold. Note the titration must still be carried out in the flask. Be sure to include any calculations you would need to perform.

What role does structure play in the ductility of a material? Discuss the way bonding influences ductility.

A beaker with 130 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 6.20 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.

Express answer numerically to two decimal places. Use a minus (-) sign if the pH has decreased.