2 1. A clear solution of silver nitrate is mixed with a solution of sodium chloride and a white precipitate forms.Write a balanced equation for this reaction.Write a complete ionic equation.Write a net-ionic equation
3 2. Define the following: a. Hydrogen bonds b. Hygroscopic c 2. Define the following: a. Hydrogen bonds b. Hygroscopic c. Desiccant d. Deliquescent e. efflorescent
4 3. Water is a polar solvent; gasoline is a nonpolar solvent 3. Water is a polar solvent; gasoline is a nonpolar solvent. Decide which compounds are more likely to dissolve in water and which are more likely to dissolve in gasoline? a. Sucrose (C12H22O11) b. Na2SO4 c. Methane (CH4) d. KCl
5 4. Match each term with the following descriptions 4. Match each term with the following descriptions. A description may apply to more than one term.a. True solution b. Colloid c. SuspensionDoes not settle out on standingHeterogeneous mixtureParticle size less than 1.0nmParticles can be filtered outDemonstrates the Tyndall EffectParticles are invisible to the unaided eyeHomogeneous milkSalt waterjelly
6 5. Name and distinguish between the town components of a solution.
7 6. Explain the difference between miscible and immiscible 6. Explain the difference between miscible and immiscible. Provide examples of each.
8 7. Explain the difference between an unsaturated, saturated and supersaturated solution.
9 8. What mass of KNO3 can be dissolved into100 g of water at 20oC 8. What mass of KNO3 can be dissolved into100 g of water at 20oC. (use Figure 18.4 on page 504)
10 9. The solubility of methane, the major component of natural gas, in water at 20oC and 1.00 atm of pressure is g / L. If the temperature remains constant, what will be the solubility of this gas at the following pressure?a atmb atm
11 10. Calculate the molarity (M) of each solution: 1.0 mol KCl in 750 mL of solution0.50 mol MgCl2 in 1.5 L of solution
12 11. Calculate the moles and grams of solute in each solution: 1.0 L of 0.50M NaCl5.0 x 102 mL of 2.0M KNO3
13 12. What is the concentration (in % m/v) of the following solutions: a g KCl in 0.60 L of solution32 g NaNO3 in 2.0 L of solutionHINT: (m / v) = mass / vol(g / mL)
14 13. What is the freezing point of each solution? a mol Na2SO4 in 1750 g H2Ob mol MgSO4 in 100 g H2O
15 14. Determine the freezing points of each 0. 20m aqueous solutions 14. Determine the freezing points of each 0.20m aqueous solutions. (use the Kf for water)K2SO4CsNO3Al(NO3)3