Unit 10B Review Reg Chem

11 When a solution sits out over a long period of time and water evaporates the concentration of the solution __________. Increases. As the volume of solution decreases, the molarity (concentration) increases

12 List an example of a solution that would naturally dilute. Ice in pop

13 What does solution concentration describe? Molarity: amount of solute dissolved in a given amount of solvent

14 What do we use to describe solution concentration in chemistry? Molarity

15 If a solution is “strong” it is If a solution is “weak” it is concentrated dilute

16 What does it mean to dilute a solution? What equation do we use for dilutions? To lower its concentration “water it down” Yet keep the number of moles the same M 1 V 1 = M 2 V 2

17 What is the molarity of a sodium chloride solution that contains 1.73 moles in 3.94 L of solution?

18 What is the molarity of sodium hydroxide solution that contains 23.5 g NaOH in mL of solution?

19 How many grams of potassium nitrate are in 275 mL of 1.25 M solution?

20 How many mL of 3.25 M hydrochloric acid would contain 16.0 grams of solute?

21 You have 12.0 M HCl in your stock room, how would you prepare mL of 2.50 M HCl solution? (12.0 M)(x) = (2.50 M)(600.0 mL) X=125 mL Measure out 125 mL of stock solution. Add 475 mL of distilled water.

22 How would you correctly prepare mL of a 3.0 M solution of NaOH from solid solute? NaOH Measure out 60 g of NaOH (s) Add water to the mL line

23 How would you prepare 500 mL of 3.0 M NaOH from 12.0 M concentrated stock solution? (12.0 M)(X) = (3.0 M)(500 mL) X=125 mL Measure out 125 mL of stock solution. Add it to 375 mL of distilled water

26 An excess of zinc is added to 125 mL of M HCl solution. What mass of zinc chloride is formed? Zn + 2HCl  ZnCl 2 + H 2