1. Acid/Base Review

2. List the properties of Acids
Sour, H3O+ ions, strong acids conduct, react with metals to form H2 gas, neutralize bases to form salt + water. Acids Ionize with water to form H3O+, litmus red

3. List the properties of bases
Bitter, slippery, OH- ions, strong bases conduct, , neutralize acids to form salt + water. Strong bases dissociate (water on arrow), litmus blue

4. List the 6 strong acids HBr HI HCl HNO3 H2SO4 HClO4
Remember these acids ionize completely in water creating a strong electrolyte!

5. Explain the difference between an oxyacid and a binary acid and give an example of each
Oxyacid has oxygen in the compound
H2SO4
Binary acid means that there are two compounds present
HCl

6. List common acids that we have talked about
Phosphoric Acid-found in soda/used to make fertilizer
HCl-found in the stomach
Acetic Acid-vinegar

7. Give two examples of weak acids and one example of a weak base
H2S-Hydrosulfuric Acid
HCH3COO-acetic acid
NH3 – ammonia (weak base)

8. List the strong bases
Anything in column 1 & 2 bonded with an OH-

9. Explain the Arrhenius Acid Definition
Acids produce H+ in solution
Acid – produces H+ in water
HCl + H2O  H3O+ + Cl-
H2SO4 + H2O  2H3O+ + SO42-
Remember H+ can also mean H3O+ (Hydronium Ion)

10. Explain the Arrhenius Base Definition
Base – produces OH- in water
NaOH  Na+ + OH-
NH3 + H2O  NH OH-

11. Explain the Bronsted-Lowrey Definition of Acids/Bases
Acids are H+ donors,
bases are proton (H+ ) acceptors.
HCl + H2O  Cl + H3O+
acid base
Bronsted-Lowry is a way to study proton transfer!!

12. Explain conjugate Acid/Base
Conjugate Acid – formed when BL base gains a proton
Conjugate Base – formed when BL acid looses a proton
HCl + NH3  NH Cl-
a b ca cb
H2SO4 + 2H2O  2 H3O+ + SO42-
a b ca cb

13. If I have a strong acid what is the strength of the conjugate base?
The stronger the acid, the weaker its conjugate base; the stronger the base, the weaker its conjugate acid

14. Study your conjugate acid/base worksheet as there are a few questions on recognizing a/cb and b/ca pairs

15. What is an amphoteric substance and give an example
Water:
can react as either an acid or base
HCl + Water  H3O Cl -
proton acceptor(water)
Water + NH  NH OH -
Water(proton donor)

16. Complete the following Reactions
3KOH + H3PO4 →
K3PO H2O
Mg(OH) HCl →
2H2O MgCl2

17. Are strong acids/bases strong or weak electrolytes?
Strong because they will completely ionize or dissociate creating many ions…….
Weak acids/bases do not ionize completely thus there are fewer electrons, thus they are not very strong electrolytes

18. How many moles of Nitric acid are in 500 ml of a 10 M HNO3 solution?

19. What does pH measure?
pH – related to the concentration of H3O + ions in solutions. The more H3O+ ions, the lower the pH.

20. Given the H3O+ concentration find the pH / pOH…A/N/B
[H3O+]=7.3x10-13
pH=12.13
pOH=1.86
Basic
[H3O+]=5x10-2
pH=1.3
pOH=12.2
Acidic

21. Given the pH find the Hydronium or hydroxide ion concentration
[H3O+]= 7.9x10-4
pH= 10.5
[H3O+]=3.2x10-11

22. Draw a strong acid/strong base titration curve

23. Draw a weak base strong acid titration curve

24. Summary of titration curves

25. During a titration curve why do we have to titrate so slowly when we get close to the equivalence point/end point?
When the hydronium ions and hydroxide ions are nearly equal (the equivalence point) the curve of graph is very steep and thus happens very quickly.

26. Explain the End Point
When the indicator changes color which should be close to the equivalence point if chosen correctly.
Ex. Strong acid/strong base should be litmus
Ex. Strong base/weak acid should be phenolphthalein

27. What is the pH of a .036M LiOH solution
First find the pOH by finding the normality
Remember normality = molarity x equivalence
Then you take the
–log (normality concentration)
-log (.036)=1.44 but that equals the pOH
Then you take =12.56 which gives you the pH
pH=12.56

28. To neutralize 20 ml of aqueous sulfuric acid, you use 32. 5 ml of a 0
To neutralize 20 ml of aqueous sulfuric acid, you use 32.5 ml of a 0.2 M NaOH solution. Calculate the Molarity
Molarity of H2SO4 =0.16

29. What volume of 0.5 M sulfuric acid is needed to react completely with 10 ml of 2.0 M LiOH
H2SO4 + 2LiOH → Li2SO4 + 2H2O .02L

30. Molarity = HCH3COO=0.367 Normality = M x eq = 0.367 x 1 = 0.367
A 20 ml sample of 0.55 M KOH solution required 30 ml of aqueous acetic acid solution in a titration experiment. Calculate M & N &pH of the acid.
Molarity = HCH3COO=0.367
Normality = M x eq = x 1 = 0.367
pH= -log [N]= -log(0.367) = .435

31. If you start with a pH of 1 and add water what should you expect to have happen to the pH?
You should expect it to neutralize
pH of 1 = .1M
When you add water you dilute it so the next step would be .01M. The pH would be 2.
.001M = pH 3 etc.
What would a graph look like?

32. You have a 4 M solution of NaOH. You need to make up 2000 ml of a 1
You have a 4 M solution of NaOH. You need to make up 2000 ml of a 1.5 M solution. How many mls of the 4 M solution do you need? How much water would you need?
V x M1 = V x M2
V x 4M = x 1.5
V1=750ml

33. What is the salt produced when KOH is used to neutralize sulfuric acid?
K2SO4