a. What is the molar solublity of lead(II) chloride in water?

b. Should we be concerned about the chloride ion acting as a base? Why or why not?

A student mixes 50.0 mL of 1.00 M Ba(OH)₂ with 81.2 mL of 0.450 M H₂SO₄.

Calculate the mass of BaSO₄ formed.

Calculate the pH of the mixed solution.

340.0  gallons of 15.0 M nitric acid were added to a lake. The initial pH of the lake was 6.40 and the final pH was 4.50 . If none of the acid was consumed in chemical reactions, determine the volume of the lake. (IN LITERS)

When trying to purify fluorene, why does a NaOH extraction work best with Benzoic Acid, succinimide, and fluorenone but a HCl extraction works best with ethyl-4-aminobenzoate? Also, draw the acid/base reaction for each of the reactions.

1.Please describe how hybridization tells you about chemical structures? What is a good rule of thumb about where groups are arranged around any central atom? Provide a reaction mechanism (i.e. movement of electrons shown) for an organic reaction to illustrate the answer from 1 , and explain how the shape of the molecule changes during a chemical reaction

The pH change around the equivalence point for strong-base/weak-acid titration is usually not as great as that for strong-base/strong-acid. The statement is true or not. Explain.

What is the percent yield of dibenzalacetone when 0.212 g of benzaldehyde and 0.058 g of acetone was used in the experiment? I got a 0.885 g of product in the end.

Show an organic reaction mechanism which relies on bond polarity in order to occur. How does electronegativity participate in this reaction.

The equilibrium vapor pressure of mercury at room temperature is about 1.6x10-6 atm. Imagine an old chemistry lab that over the years has experienced enough liquid mercury spills and thereby accumulated enough mercury in cracks in the floor, etc. that mercury liquid-vapor equilibrium has been established. What is the concentration, in the units of milligrams per cubic meter, of Hg0 in the air of the room? Does this value exceed the limit of 0.05 mg m-3 established by the American Conference of Governmental Industrial Hygienists (ACGIH) for safe exposure based upon a 40-hour work week?

Consider the titration of a 26.0-mL sample of 0.180 M CH3NH2 with 0.145 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.)

Already found:

volume of added acid required to reach the equivalence point.=32.3 ml

pH at 6.0 mL of added acid=11.28

pH at one-half of the equivalence point.= 10.64

Part A

Determine the initial pH

Part B

Determine the pH at the equivalence point.

Part C

Determine the pH after adding 5.0 mL of acid beyond the equivalence point.

For each of the following pairs of molecules, identify the dominate intermolecular force, and answer any associated questions.

a. KNO2, CH3NO2

Which compound do you expect to have the highest melting point?

b. CH3CH2OH, CH3OCH3

Which compound do you expect to have the highest boiling point?

c. KF, BrF

Which compound do you expect to have the greatest vapor pressure?

List the dominant IMF for each molecule:

d. NH3, N2

e. CF4, CCl4

f. HCN, KCN

g. LiCl, CH3CH3

h. CH3OH, CH3F

Please explain each step.

• Draw products for the following addition reactions:
  • Hydrogenation (H₂ / Pt)
  • Halogenation (X₂)
  • Hydrohalogenation (HX)
  • Hydration (H₂O, H⁺)

1a. What happens to the pressure of an ideal gas if you double its temperature in a closed volume? And what happens to the pressure of an ideal gas if you double its volume at a fixed temperature?Please explain your answer using the combine gas law.

1b. Based upon the standard molar volume, what volume would 0.500 moles of an ideal gas occupy at STP? And based upon the standard molar volume, what volume would be occupied by 1.00 mol of an ideal gas at a temperature of 819.45 K and a pressure of 760.0 mmHg?Please explain your answer.