We can check our predictions by using other materials for solubility experiments. a. Make a table for the Lewis structures, polarity and expected intermolecular forces for all of the following: water, I2, CH2Cla, CH;OH, and CsH14 b. Do you expect la to be more soluble in CsHza or H2O? Why?

Rank the species from most to least soluble in water. Ba(103)2, Ksp = 4.0×10-9 FeF2, Ksp = 2.4x10-6 CslO4, Ksp = 5.2×10-6 I. I. I. Periodic Table and Datasheet O I> || > III O II >I> II O I> III >|| O III > || > I

Which of the following has the highest ionic strength? Why? A.  0.025 mol/L Na2SO4 B.  0.025 mol/L CaSO4 C.  0.050 mol/L NaCl D.  0.005 mol/L NH4Cl

A pharmacist adds 3 mL of 8 mmol/L NaF to 197 mL of 2.5 mmol/L NaCl. What is the total mEq of the sodium (Na) ion in the mixture? Report your answer with 2 decimal places. DO NOT include units.

What is the equilibrium concentration of N₂ in water that is in contact with air at 25 °C and air pressure 1 atm? The mole fraction of N2₂ in the air is 80 %, and Henry's law constant for N₂ is 6 x 10-4 mol L-1 atm-1. Select the nearest value. O 4.8x 10-3 mg L-1 4.8 x 10-4 mmol L-1 0.6 x 10-4 mol L-1 6 x 10-3 g L-1 6 x 10-4 mol L-1

2.00 mol of NOBr dissociates 9.4 % in a 1.0 L vessel.  Calculate Kc.               2NOBr (g)  ↔ 2NO(g)  +  Br2(g)

3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small.   D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.

4. Why do you determine a mass by difference? You use this because it's typically more accurate. 5. What are equivalence points and end points? How do they differ? equivalence point- the point @ which stoichiometric quantities are brought together, end point- the the equivalence point is theoretical, when end poi 6. Why should the standardized NaOH solution be kept in a stoppered bottle? pr 7. What is parallax? Why should you avoid it? Parallax is the upperent displacement or the di da in direction of an object as seen from two diffe points. са It should be colded because it ca errors in volume measurements. Copyright © 2018 Pearson Education, Inc.

I. List all the IMFS that are present in a pure sample of substance A below. The Lewis structure of a molecule is shown. H -C C-H | | H II. Draw one example of substance A acting as a H-bond donor with water. Make sure your H- bond starts and ends in the right places. If the molecule can't act as a H-bond donor, write "not possible." II. Draw one example of substance A acting as a H-bond acceptor with water. Make sure your H-bond starts and ends in the right places. If the molecule can't act as a H-bond acceptor, write "not possible." IV. List all the IMF that are present in a pure sample of substance B below. The Lewis structure of a molecule is shown. H H. C N. H H. H V. Compare substance A and substance B. Which would you expect to have the highest boiling point? Briefly explain why (in about 1 sentence). IIC- :O:

9. Consider the molecule of palmitic acid that is shown below. Draw a figure to show the behaviour of this molecule when it is added to an aqueous solution in high concentration. In your answer, describe what motivates the behaviour of palmitic acid in aqueous solution. HO,