Chapter 7 – Practice Problems (Definitions)

1. Define solute and solvent.

2. Define saturated, unsaturated, and supersaturated.

3. A solution is prepared by combining 2.09 g of CO₂ and 35.5 g of H₂O. Identify the solute and solvent.

4. A solution is prepared by combining 10.3 g of Hg(ℓ) and 45.0 g of Ag(s). Identify the solute and solvent.

5. Use the associated table to determine the following: decide if a solution containing 45.0 g of NaCl per 100 g of H₂O is unsaturated, saturated, or supersaturated.
   

   Solute	Solubility (g per 100 g of H2O at 25°C)
   AgCl	0.00019
   CaCO3	0.0006
   KBr	70.7
   NaCl	36.1
   NaNO3	94.6

6. Use the table in question 5 to determine the following: decide if a solution containing 0.000092 g of AgCl per 100 g of H₂O is unsaturated , saturated, or supersaturated.
7. Would the solution in Exercise 5 be described as dilute or concentrated? Explain your answer.
8. Would the solution in Exercise 6 be described as dilute or concentrated? Explain your answer.
9. Identify a solute from the table in question 5 – Solubilities of Some Ionic Compounds, whose saturated solution can be described as dilute.
10. Identify a solute from the table in question 5 – Solubilities of Some Ionic Compounds, whose saturated solution can be described as concentrated.
11. Which solvent is Br₂ more likely soluble in—CH₃OH or C₆H₆?
12. Which solvent is NaOH more likely soluble in—CH₃OH or C₆H₆?
13. Compounds with the formula C_nH_{2n + 1}OH are soluble in H₂O when n is small but not when n is large. Suggest an explanation for this phenomenon.
14. Glucose has the following structure:

What parts of the molecule indicate that this substance is soluble in water?