Name: Reaction in Aqueous Solutions Review Worksheet 1) Define the following and give one example for each: a) Strong electrolytes: b) Weak electrolytes:

c) Non-electrolytes:

2) Why are electrolytes conductors of electricity?

3) What is a precipitate? 4) What is the driving force in the following reactions? a) Precipitation reactions – b) Acid-Base reactions – c) Redox reactions – d) Gas forming reactions – 5) Write the molecular, ionic, and net ionic equations for the following. Indicate the spectator ions as well. a) An aqueous solution of Iron (II) sulfate is mixed with an aqueous solution of sodium phosphate.

b) An aqueous solution of sulfuric acid is mixed with an aqueous solution of aluminum hydroxide.

c) An aqueous solution of methyl amine (CH3NH2) is mixed with an aqueous solution of hydrobromic acid.

6) Define an acid according to: a) Arrheneius theory:

b) Bronsted-Lowry theory:

c) Lewis theory:

7) What acid and base should be mixed to produce the following salts? Write the balanced equations for these reactions: a) Na2CO3 b) KCl c) CaSO4 8) Identify the acid, base, and their conjugate pairs in the following acid base reactions. a) HCl + OH- ßà H2O + Clb) C2H3O2H + OH- ßà C2H3O2- + H2O 9) Give one example each of a Lewis acid and Lewis base.

10) What is the pH scale? What information does it give us?

11) Calculate the pH and pOH of the solutions with following concentrations:a) [OH-] = 4.51 x 10-10 M b) [H3O+] = 3.25 x 10-5 M 12) Calculate the [H+] and [OH-] for the following: a) pH = 4.4

b) pOH = 12.43 13) a) What are buffers? What is their function?

b) Explain the buffer action using one buffer example.

c) What is buffer capacity? What information does it give?

14) How would you prepare a 400 mL solution of 0.50 M NaNO3 from the solid reagent? Show the calculations involved and describe the process.

15) How would you prepare 250 mL of 0.10 M HCl if you have 500 mL of 0.25 M HCl solution? Show the calculations involved and describe the process.

16) What is titration? What is this technique useful for?

17) What is an indicator? 18) What is the end point? What is the equivalence point? Explain the difference.

19) Titration indicates that 12.7 mL of 4.5 M sulfuric acid are required to neutralize 25.00 mL of NaOH solution. What is the molarity of the NaOH solution?

20) Define the following: a) Oxidation:

b) Reduction:

c) Oxidizing agent:

d) Reducing agent:

21) Write the oxidation numbers on each element and figure out which species is oxidized and which species is reduced. Then balance the following reaction in acid medium: IO3 -(aq) + I -(aq) à I3 -(aq) How many electrons are transferred in this redox process?

22) Write the oxidation numbers on each element and figure out which species is oxidized and which species is reduced. Then balance the following reaction in basic medium: ClO3 -(aq) + I2(aq) à Cl -(aq) + IO3 -(aq) How many electrons are transferred in this redox process?

23) A compound has been isolated that can have either of two possible formulas: a) K[Fe(C2O4)2(H2O)2] or (b) K3[Fe(C2O4)3. To find which is correct, you dissolve a weighed sample of the compound in acid and then titrate the oxalate ion (C2O4-2) with potassium permanganate, KMnO4 (the source of the MnO4- ion). The balanced net ionic equation for the titration is 5 C2O4-2 + 2 MnO4- + 16 H+ à 2 Mn +2 + 10 CO2 + 8 H2O Titration of 1.356 g of the compound requires 34.50 mL of 0.108 M KMnO4. Which is the correct formula of the iron containing compound (a) or (b)?

24) Vitamin C, ascorbic acid (C6H8O6), is a reducing agent. One way to determine the ascorbic acid content of a sample is to mix the acid with an excess of iodine, C6H8O6 + I2 à C6H6O6 + 2 H+ + 2 Iand then titrate the iodine that did not react with the ascorbic acid with sodium thiosulfate. The balanced, net ionic equation for the reaction occuring in the course of this titration is I2 + 2 S2O3-2 à 2 I- + S4O6-2 Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. After the ascorbic acid/I2 reaction was complete, the I2 not used in the reaction required 20.30 mL of 0.196 M Na2S2O3 for titration to the equivalence point. Calculate the mass of ascorbic acid in the unknown sample.