<p> Unit 12 WATER and SOLUTIONS!!! Let’s talk about solutions a bit more in depth 1) A solution is made of two parts, name them and define each (pg. 482)</p><p>2) Describe the solvation process (pg. 483)</p><p>3) What kind of things dissolve in water (sometimes called the universal solvent)?</p><p>4) What does “like dissolves like” mean?</p><p>5) What are some things that determine how fast a solute will dissolve in a solvent (pg. 501,502)</p><p>6) Solubility (pg. 502-507) a. What are the three levels of solubility and describe each.</p><p> b. What is the most common factor that changes solubility? i. How does this factor usually effect how solids dissolve in water?</p><p> ii. How does this factor usually effect how gases dissolve in water?</p><p> iii. Solubility curves</p><p>Typical solubility curve questions: - What is the solubility of KBr at 70o?</p><p>- How much KNO3 will dissolve in 100 g of water at 20o, at 80o?</p><p>- What happens when 100 g of NaNO3 is added to 100 mL of boiling water, what happens when this is cooled to 50o, what happens when it is cooled to 0o? Concentration Units: 1) Molarity (M) = moles of solute/ L of solution (pg.509-513) a. From a solid: What is the M of a solution of 10 g of NaCl in enough water to make 250 mL of solution?</p><p> b. Dilution: (M1V1 = M2V2) I take 25.0 mL of 12M HCl and dilute it to 500 mL with water, what is the solutions new M?</p><p>How do I make 250.0 mL of 1.0M nitric acid from a stock solution (15M)?</p><p>2) Percentages: (pg. 513-514) a. Percent by mass = mass solute/ total mass</p><p> b. Percent by volume = volume of solute/ total volume of solution</p><p> c. Percent mass/volume = mass of solute (g) / total volume of solution (mL)</p><p>Summary Problem: I dissolved 25.0 mL of C2H5OH (D = 0.82 g/mL) in 75.0 mL of water. The resulting solution had a volume of 97.0 mL. Give the concentration of this solution in all 4 units we’ve learned.</p><p> solute solvent solution mass volume moles</p>