Unit 12 – Acids and Bases PacketName:______

Station #1: Naming Acids and Bases

Name the following acids and bases:

1)NaOH ______

2)H2SO3 ______

3)H2S ______

4)H3PO4 ______

5)NH3 ______

6)HCN ______

7)Ca(OH)2 ______

8)Fe(OH)3 ______

9)H3P______

Write the formulas of the following acids and bases:

10)hydrofluoric acid ______

11)hydroselenic acid ______

12)carbonic acid ______

13)lithium hydroxide ______

14)nitrous acid ______

15)cobalt (II) hydroxide ______

16)sulfuric acid ______

17)beryllium hydroxide ______

18)hydrobromic acid ______

Station #2: Properties of Acids and Bases

First, watch the video on this page!!

  1. Acids have a ______taste.
  2. The word ‘acid’ comes from the latin word ______.
  3. Robert ______first classified substances as acids and bases.
  4. Acids turn litmus paper ______.
  5. Bases turn litmus paper ______.
  6. Acids dissolve in water releasing ______ions.
  7. Bases dissolve in water releasing ______ions.
  8. Hydrogen ions contain ______hydrogen atom.
  9. Acids have a pH greater than 0 but less than ____.
  10. Bases have a pH greater than 7 but less than ____.

Station #3: Strong vs Weak

Watch this video first!

Using the information from the video and your notes, answer the following questions.

  1. What makes acids and bases strong?
  1. Is hydrochloric acid, HCl, strong or weak? What is the dissociation reaction?
  1. Is sodium hydroxide, NaOH, strong or weak? What is the dissociation reaction?
  1. Is ammonia, NH3, strong or weak? What is the dissociation reaction?
  1. List the acids mentioned in the correct boxes…

Strong Acids: / Strong Bases:
Weak Acids: / Weak Bases:
  1. What are the three things you can see to determine whether an acid/base is strong or weak?
  1. How will strong acids/bases conduct electricity?
  1. Do strong acids/bases react slow or fast?
  1. Label on the pH scale where strong/weak acids/bases fall:
  1. Hydrochloric acid, HCl, is in your stomach. So the stomach has a ______acid in it.
  1. Phosphoric acid, H3PO4, is in most sodas, do you drink strong or weak acids when you drink sodas?
  1. The pH of most blood is 7.35-7.45, what is your blood?
  1. The pH of milk is about 6.5, what is milk?
  1. The pH of limes is about 1.5, what does that make limes?

Station #4: Electrical Conductivity

Use the electrolyte probes to determine whether the following acids and bases are strong or weak.

SubstanceBright lightbulb? Y/NStrong/Weak

Beaker #1 HCl solution______

Beaker #2 Acetic Acid solution______

Beaker #3 NaOH solution______

Beaker #4 NH3 solution______

Station #5: Acid/Base Theories

  1. The Arrhenius Theory of acids and bases is limited because it only applies to

______solutions, meaning dissolved in ______

  1. An Arrhenius acid is one that releases a ______in water and an Arrhenius base is one that

releases a ______in water

  1. Identify whether the following are Arrhenius acids or bases:
  2. HNO3(aq)  H+1(aq) + NO3-1(aq)
  1. Al(OH)3 (aq)  Al +3(aq) + 3OH-1(aq)
  1. Ca(OH)2(aq)  Ca+2(aq) + 2OH-1(aq)
  1. H2SO4(aq)  2H+1(aq) + SO4-2(aq)
  1. Bronsted-Lowry Theory of acids and bases includes acids and bases that do not have to be

dissolved in ______

  1. Bronsted-Lowry acids are proton (H+) ______while Bronsted-Lowry bases are proton

(H+1) ______

  1. Identify which of the following reactants are Bronsted-Lowry acids or bases:

NH3 + HI  NH4+1 + I-1

HCl + H2O <==> H3O+ + Cl¯

  1. An ______substance is one that acts as an acid or a base
  1. A hydrogen ion (H+1) is also known as a ______

Station #6: Ionization/Dissociation Reactions

Write the correct, balanced reaction the following acids and bases have when put into water.

  1. Nitrous acid + water
  1. Calcium hydroxide
  1. Hydroiodic acid + water
  1. Lithium hydroxide
  1. Chloric acid + water
  1. Aluminum hydroxide

Station #7: Types of Reactions (Demos)

Demos:

  1. Describe what happened in the demo: ______

______

  1. What kind of reaction did you observe? ______
  1. Write the balanced chemical equation.
  1. Describe what happened in the demo: ______

______

  1. What kind of reaction did you observe? ______
  1. Write the balanced chemical equation.
  1. Describe what happened in the demo: ______

______

  1. What kind of reaction did you observe? ______
  1. Write the balanced chemical equation.
  1. Describe what happened in the demo: ______

______

  1. What kind of reaction did you observe? ______
  1. Write the balanced chemical equation.

Station #7: Types of Reactions (Practice)

Write and balance the following chemical reactions as well as answer the questions:

  1. Hydrochloric acid reacts with sodium hydroxide to produce water and sodium chloride.
  1. What type of reaction?
  1. Cobalt (II) chloride reacts with sodium carbonate producing cobalt (II) carbonate plus sodium chloride.
  1. What type of reaction?
  1. Which of the products is the precipitate?
  1. How did you choose?
  1. Magnesium plus Bromine will combine to form magnesium bromide.
  1. What type of reaction?
  1. What element is reduced and why?
  1. What element is oxidized and why?
  1. Sulfuric acid plus ammonium hydroxide produce water plus ammonium sulfate.
  1. What type of reaction?
  1. Lead (II) Nitrate plus Sodium Iodide form Lead (II) Iodide plus Sodium Nitrate.
  1. What type of reaction?
  1. Which of the products is the precipitate?
  1. How did you choose?
  1. Lithium reacts with Sulfur to produce Lithium Sulfide.
  1. What type of reaction?
  1. What element is reduced and why?
  1. What element is oxidized and why?

Station #8: Calculations

What you will need:

pH = -log[H3O+][H3O+] x [OH-] = 1 x 10-14

pOH = -log[OH-]If [H3O+] > [OH-] = acidic

If [H3O+] x [OH-] = neutral

pH + pOH = 14If [H3O+] < [OH-] = basic

  1. If [H3O+] is 4.5 x 10-3 and [OH-] is 6.4 x 10-10, is the solution acidic/basic/neutral?
  1. If [H3O+] is 1.5 x 10-12 and [OH-] is 3.2 x 10-2, is the solution acidic/basic/neutral?
  1. If [H3O+] is 8.9 x 10-1 and [OH-] is 5.3 x 10-13, is the solution acidic/basic/neutral?
  1. If [H3O+] is 1.0 x 10-7 and [OH-] is 1.0 x 10-7, is the solution acidic/basic/neutral?
  1. If [H3O+] is 4.3 x 10-3, what is the [OH-]? Is the solution acidic/basic/neutral?
  1. If [H3O+] is 5.6 x 10-12, what is the [OH-]? Is the solution acidic/basic/neutral?
  1. If [H3O+] is 1.2 x 10-10, what is the [OH-]? Is the solution acidic/basic/neutral?
  1. Calculate the pH if [H3O+] = 3.2 x 10-10M. Is the solution acidic or basic?
  2. Calculate the pH if [H3O+] = 5.3 x 10-2M. Is the solution acidic or basic?
  1. Calculate the pH if [H3O+] = 2.3 x 10-5M. Is the solution acidic or basic?
  1. Calculate the pOH if [OH-] = 6.5 x 10-2M. Is the solution acidic or basic?
  1. Calculate the pOH if [OH-] = 2.3 x 10-8M. Is the solution acidic or basic?
  1. Calculate the pOH if [OH-] = 7.9 x 10-12M. Is the solution acidic or basic?
  1. Calculate pH if pOH is 1.2. Is the solution acidic or basic?
  1. Calculate pH if pOH is 13.2. Is the solution acidic or basic?