1. Chapter 10 Acids, Bases, and Salts

2. Electrolytes
Any substance that conducts electricity in a solution is an electrolyte
Ions are electrolytes
ACIDS, BASES, and SALTS are all good electrolytes.

3. Properties of Acids Aqueous solutions conduct an electric current
They are good electrolytes
Sour taste.
So, lemon juice is an ____.
Formula usually begins with an “H” and the name ends in the word “acid.”
HCl or Hydrochloric Acid
pH of 0-6
We will talk more about pH later
Reacts with certain metals to produce hydrogen gas.
Table J, but we will go over it later
Reacts with bases to form a salt and water.
Called neutralization
Cause indicators to change colors
Table M
Common acids are on Table K

4. Table J- Reactivity
The higher up the element is, the MORE reactive it is.
Any metals ABOVE **H2 react with acids to produce hydrogen gas.
Zn + 2HCl => ZnCl2 + H2
Metals BELOW **H2 do NOT react with acids!

5. Properties of Bases Aqueous solutions conduct an electric current
They are good electrolytes
Bitter taste.
So, coffee is a ____.
Have a slippery or soapy feeling
So, dish soap is a ___.
Formula usually ends in -OH and the name ends in the word “hydroxide.”
NaOH or Sodium Hydroxide
pH of 8-14
We will talk more about pH later
Reacts with acids to form a salt and water.
Called neutralization
Cause indicators to change colors
Table M
Common acids are on Table L

6. Defining an Acid and a Base
There are 2 main theories that define an acid and a base
Arrhenius Theory
Bronsted-Lowry Theory

7. Arrhenius Theory
Acids in a water solution will release H+ HYDROGEN IONS as the only positive ions in solution.
Sometimes written as H3O+ Hydronium ions
HCl(aq) => H+ + Cl-
HCl + H2O => H3O+ + Cl-
Bases in a water solution will release OH- HYDROXIDE IONS as the only negative ions in solution.
NaOH(aq) => Na+ + OH-

8. Bronsted-Lowry Theory
Acids are PROTON DONORS
Bases are PROTON ACCEPTORS
Think about it….
What is the charge on a proton?
So, acids DONATE an H+
And, bases ACCEPT an H+

9. Conjugate Acid/Base Pairs
Whichever compound in an equation DONATES the proton must be the ACID
Whichever compound in an equation ACCEPTS the proton must be the BASE
HNO3 + H2O => H3O+ + NO3-
acid base acid base

10. Amphoteric Solutions
A substance that can act as EITHER an acid or a base.
H2O
H2SO4

11. Neutralization Reaction
Occurs when [H+] = [OH-]
Do you remember what brackets mean?
So, for complete neutralization, it must have the same concentrations and the same strength of pH
Weak acid + strong base = weak base
Strong acid + weak base = weak acid
Strong acid + strong base = neutral
Acid + Base => Salt + Water
BY salt, I mean compounds that do NOT contain an H+ or an OH- ions.
Net Ionic Equation for Neutralization
H+ + OH- => H2O

12. Examples Finish the following equations: HCl + NaOH =>
HCl + KOH =>
Mg(OH)2 + HCl =>

13. Acid/ Base Indicators Indicates the presence of an acid or base
Changes color when pH changes
Table M

14. Table M
pH of 5.4?
pH of 3?
Why is litmus not a good indicator of something that has a pH of 13?

15. pH Scale 0 – 7 – 14 0 = strong acid 6 = weak acid 7 = neutral
8 = weakest base
14 = strongest base

16. pH Scale
A negative log scale that demonstrates the strength of an acid or a base
1 x 10-4 = pH 4
1 x = pH 10
pH is the number of the exponent
It is how many H+ ions are present
Each change of 1 position on the pH scale is a change of 10x
As you change from a 4 pH to a 5 pH, there are ___ times (more/less) H+ ions
pH of 6 to pH of 8 ?
pH of 10 to a pH of 7 ?
As the concentration of the hydrogen ion increases, the concentration of the hydroxide ion decreases

17. Titration Used to find the unknown Molarity of an acid or a base
The KNOWN variable is placed in a buret and the UNKNOWN variable is placed in a flask with a indicator (usually phenolphthalein)
When the color changes, you have the volume of the KNOWN variable and can now find the molarity using a formula

18. Titration
Color change indicates end point of titration
Table T

19. Examples
50mL of an acid with a molarity of 10M completely neutralizes 100mL of a base. What is the molarity of the base?
A 9.0mL sample of HCl solution is exactly neutralized by 6.0mL of a 3.0M NaOH solution. What is the concentration of the HCl solution?
How many milliliters of 0.20M HCl are needed to exactly neutralize 40.mL of 0.40M KOH?
Write the balanced equation for the reaction between HCl and KOH