Acid/Base Review

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

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

List the 6 strong acids

• HBr• HI• HCl

• HNO3

• H2SO4

• HClO4

• Remember these acids ionize completely in water creating a strong electrolyte!

Explain the difference between an oxyacid and a binary acid and give

an example of each

• Oxyacid has oxygen in the compoundH2SO4

• Binary acid means that there are two compounds present HCl

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

Give two examples of weak acids and one example of a weak base

• H2S-Hydrosulfuric Acid

• HCH3COO-acetic acid

• NH3 – ammonia (weak base)

List the strong bases

• Anything in column 1 & 2 bonded with an OH-

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)

• Base – produces OH- in water NaOH Na+ + OH-

NH3 + H2O NH4

+ + OH-

Explain the Arrhenius Base Definition

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!!

Explain conjugate Acid/Base

• Conjugate Acid – formed when BL base gains a proton

• Conjugate Base – formed when BL acid looses a proton

• HCl + NH3 NH4+ + Cl-

• a b ca cb

• H2SO4 + 2H2O 2 H3O+ + SO42-

a b ca cb

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

Study your conjugate acid/base worksheet as there are a few questions on recognizing a/cb

and b/ca pairs

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 + NH3 NH4 + + OH - Water(proton donor)

Complete the following Reactions

• 3KOH + H3PO4 →

K3PO4 + 3 H2O

• Mg(OH)2 + 2 HCl →

2H2O + MgCl2

• 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

Are strong acids/bases strong or weak electrolytes?

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

• 5 moles

What does pH measure?

pH – related to the concentration of H3O + ions in solutions. The more H3O+ ions, the lower the pH.

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

Given the pH find the Hydronium or hydroxide ion concentration

• pH= 3.1

• [H3O+]= 7.9x10-4

• pH= 10.5

• [H3O+]=3.2x10-11

Draw a strong acid/strong base titration curve

Draw a weak base strong acid titration curve

Summary of titration curves

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.

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

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 pOHThen you take 14-1.44=12.56 which gives you

the pHpH=12.56

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

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

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 = 0.367 x 1 = 0.367

• pH= -log [N]= -log(0.367) = .435

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?

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?

• V1 x M1 = V2 x M2

• V1 x 4M = 2000 x 1.5

• V1=750ml

What is the salt produced when KOH is used to neutralize sulfuric

acid?

• K2SO4