1. Chapter 7 Solutions Scavenger Hunt

2. Big Idea 1: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions.
Big Idea 2: Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them.
By the end of this chapter, you should be able to do the following:
Distinguish between a solution and a pure substance
Predict the relative solubility of a solute in a solvent, based on its polarity
Relate ion formation to electrical conductivity in aqueous solutions
Calculate the concentration of ions in solution
By the end of this chapter you should know the meaning of these key terms: acid-base neutralization mole
dissociation equation non-polar
electrical conductivity polar
ion charge solute
ionization equation solution
molarity solvent
molar solution

3. Give two examples of: Pure Substance Mixture

4. Define homogeneous, heterogeneous, pure substance, and mixture
Define homogeneous, heterogeneous, pure substance, and mixture. Give an example for each.

5. Complete the following sentences using the terms solute, solvent, miscible, and immiscible.
A solution is composed of a __________ and __________. The ____________ is the substance that makes up the larger part of the solution. If two components can be mixed in any proportions to make a homogeneous mixture, they are _______________.

6. What is the difference between soluble and insoluble?

7. How do you calculate molar solubility?

8. Salts containing which cations are always soluble?
Salts containing which anion are always soluble?
Salts containing which anions have a low solubility most often?

9. For the following salts, use the solubility table (Table 7. 1
For the following salts, use the solubility table (Table 7.1.1) to predict whether they are soluble (S), or have a low solubility (LS):
NaCl
CaCO3
Zinc Sulfite
Ammonium Hydroxide

10. When the solubility of a substance is given, what information must be specified?

11. The molar solubility of lead(II) bromide is 2. 6 × 10–3M
The molar solubility of lead(II) bromide is 2.6 × 10–3M. What is its solubility in g/ml?

12. Describe unsaturated, saturated and supersaturated in your own words.

13. What are the three important criteria for a substance to dissolve?

14. What is “like” between NaCl and H2O? Why do they interact as they do?

15. Explain why water molecules will not surround I2 molecules
Explain why water molecules will not surround I2 molecules? What forces must be overcome between each water molecule?

16. What are the three types of “forces” described in 7. 2
What are the three types of “forces” described in 7.2? Describe these three types of “forces”.

17. Which is more soluble in water: C2H6 or CH3OH? Explain.

18. Octanol has the formula C8H17OH
Octanol has the formula C8H17OH. Explain why octanol does not dissolve in water.

19. Complete Activity 7.2: Determining the Bond Type of a Solute

20. A student dissolved 0.25 g of calcium nitrate in mL water. A 50.0 mL sample of this solution was diluted to 75.0 mL. What was the final concentration?

21. Explain how the terms “solvation” and “hydration” are different.

22. Explain why the cation in a solute will be attracted to a solvent water molecule.

23. Write balanced dissociation equations to represent the dissolving of the following solutes in water:
FeCl3
MnHPO4

24. List the acids that are strong electrolytes
List the acids that are strong electrolytes. Explain why they are considered strong.

25. What are the differences between a strong electrolyte, weak electrolyte and a nonelectrolyte? Give an example of each.

26. You are given two beakers, one containing 3
You are given two beakers, one containing 3.0 M HNO3 and one containing 6.0 M C12H22O11. Explain how you could use a light bulb apparatus to distinguish between the two solutions.

27. What is titration?

28. Write the balanced equation for the reaction between aluminum hydroxide and hydrobromic acid to form aluminum bromide and water.

29. Write the formulas for the acid and base that will react to give the salt K2CO3 and water.

30. A student titrated 25. 00 mL of HCl with 15. 62 mL of 0. 30M NaOH
A student titrated mL of HCl with mL of 0.30M NaOH. Calculate the [HCl].

31. Define the terms “standardized,”“equivalence point,” and “endpoint.”

32. A 25. 00 mL sample of 0. 20 M H2CO3 was titrated with 0. 50 M NaOH
A mL sample of 0.20 M H2CO3 was titrated with 0.50 M NaOH. What volume of NaOH was required to reach the equivalence point?