1. Introduction to Acids & Bases
Thursday, May 4th, 2017

2. How Do you Characterize Acids and Bases?
pH scale – a measure used to report the acidity of a solution
Range 0 to 14

3. Indicators - chemical substances that change color based on pH

4. Indicators - chemical substances that change color based on pH

5. Use the handout to complete the Venn Diagram in your notes.
Acid/Base Venn Diagram
Use the handout to complete the Venn Diagram in your notes.

6. Three Acid/Base Theories
complete the chart and put in your notebook
Arrhenius - H+ and OH- production in water
Acid – produces H+ in water
HCl + H2O → H3O + + Cl-
or dissociation equation: HCl (aq) → H + (aq) + Cl- (aq)
Base – produces OH- in water
dissociation equation: NaOH (aq) → Na + (aq) + OH- (aq)

7. Bronsted – Lowry – proton transfer between reactants
Acid – donates a proton
Base – accepts a proton   
HF  + NH3  →   NH4 +  +  F-
    acid           base

8. Lewis – electron pair transfer between reactants
Acid – accepts electron pair
Base – shares electron pair
H+  + :NH3  →   NH4 +          
acid           base

9. Common Acids and Bases to Memorize
HCl – hydrochloric acid [hydrogen chloride]
H2SO4 – sulfuric acid [hydrogen sulfate]
HNO3 – nitric acid [hydrogen nitrate]
H2CO3 – carbonic acid [hydrogen carbonate]
NaOH – sodium hydroxide
Ca(OH)2 – calcium hydroxide
NH3 – ammonia

10. Why are these called acids and bases? Why do they cause a color change?
They deviate from the natural water ion concentration
            Salt in water:    NaCl (aq)   Na+ (aq)   +  Cl- (aq)
Water forms ions – self ionization! H2O  H + + OH-
Hydrogen ion [H +]      vs        hydronium ion [H3O +]
      (proton)
Transferred in Exists in aq solutions
A/B rxn         

11. Which of the following substances are acidic, basic or neutral?
H2O   H +  +  OH-
Water is neutral because for Water [H+]=[OH-] 
both = 1.0 x 10-7M
Acid  or acidic solution – [H+] > [OH-] 
[H+] > 1.0 x 10-7M
Base or alkaline solution (basic) - [H+] < [OH-] 
[H+] < 1.0 x 10-7M
Which of the following substances are acidic, basic or neutral?
a) A solution with  [H+] = 1.0 x 10-3M
b) A solution with  [H+] = 1.9 x 10-8M
c) A solution of salt and water

12. pH = -log [H+1] pOH = -log [OH-1] [H+1][OH-1] = 1 x 10-14
pH Formulas:
[H+1] = 10-pH [OH-1] = 10-pOH
pH = -log [H+1] pOH = -log [OH-1]
[H+1][OH-1] = 1 x 10-14
pH + pOH = 14

13. Calculate the pH of the following:
pH can be determined mathematically from the concentration!
[H+] = hydrogen ion molar concentration
Working with log and antilog is easy all you do is find the key on your calculator!:
pH = -log [H+]
[H+ ] = 10-pH
Calculate the pH of the following:
a) What is the pH of a solution with [H+] = 1.0 x 10-3M
b) What is the pH of a solution with [H+] = 1.9 x 10-8M
c) What is the [H+] of a solution with a pH of 5
d) What is the [H+] of a solution with a pH of 3.7

14. a) What is the pOH of a solution with [OH-] = 1.0 x 10-3M
OK so pH is related to how acidic something is....but what about the other ion???
[OH-] = hydroxide ion molar concentration
This focus on how basic something is
pOH = -log [OH-]
[OH- ] = 10-pOH
a) What is the pOH of a solution with [OH-] = 1.0 x 10-3M
b) What is the [OH-] of a solution with a pOH of 10.7

15. a) What is the pOH of a solution with pH = 5.75?
Oh and YES there is a relationship between the two!!!!
pH + pOH = 14  
[H+] [OH-] = 1.0 x 10-14               
a) What is the pOH of a solution with pH = 5.75?
b) What is the [OH-] of a solution with a pH of 4.5?

16. Complete the Intro to Acid/Base Review Worksheet