Name: _____________________________________________Period: _______________________

Unit 11 Acids and Bases pHUNSHEET

Part A: Write the molecular equation, complete ionic equation, and net ionic equation for the following reactions. Be sure to BALANCE all reactions AND include states of matter. Identify the spectator ions for each reaction.

1) ____Mg(OH)2(s) + ____HI(aq) _______________________________________________________________

2) A solution of hydrochloric acid is added to a solution of strontium hydroxide.

3) Solutions of hydrofluoric acid and sodium hydroxide.

4) Cesium hydroxide is mixed with perchloric acid.

5) ____HC2H3O2(aq) + ____LiOH(aq) ______________________________________________________________

6) ____HNO3(aq) + ____Zn(OH)2(s) ______________________________________________________________

7) Hydrobromic acid is reacted with barium hydroxide.

8) Sulfuric acid is reacted with ammonium hydroxide.

Part B: Using Arrhenius definition, classify the following examples as acids, bases, or salts.

1)

1

2) HBr__________________________

3) Mg(OH)2 __________________________

4) HCl__________________________

5) KNO2__________________________

6) Ba(OH)2__________________________

7) H3PO4__________________________

8) HClO__________________________

9) KCl__________________________

10) Al(OH)3__________________________

11) KC2H3O2__________________________

12) NaCl__________________________

13) NH3__________________________

14) Explain why NH3 is considered a Bronsted-Lowry base, but not an Arrhenius base.

15) What happens to the charge of a substance if it gains a proton (H+)? ____________________________________

16) What happens to the charge of a substance if it loses a proton (H+)?____________________________________

17) When an acid (gains/loses) a proton, it becomes the conjugate (acid/base). (circle the correct answers)

18) When a base (gains/loses) a proton, it become the conjugate (acid/base). (circle the correct answers)

19) For the following, write in the missing information for each conjugate pair.

For the following equations, label the Bronsted-Lowry acid/base AND label the conjugate acid and conjugate base.

20) HC2H3O2 + H2O H3O+1 + C2H3O2-1 ______________+____________ _____________+______________

21) HCO3-1 + H2O H2CO3 + OH-1 ______________+____________ _____________+______________

22) HNO3 + SO4-2 HSO4-1 + NO3-1 ______________+____________ _____________+______________

23) HF + H2O F-1 + H3O+1 ______________+____________ _____________+______________

24) HNO2 + H2O H3O+1 + NO2-1 ______________+____________ _____________+______________

25) H2O + S-2 HS-1 + OH-1 ______________+____________ _____________+______________

26) CN-1 + HC2H3O2 C2H3O2-1 + HCN ______________+____________ _____________+______________

27) NH3 + H2O NH4+1 + OH-1 ______________+____________ _____________+______________

28) OH-1 + NH4+1 H2O + NH3 ______________+____________ _____________+______________

29) HSO4-1 + H2O H3O+ + SO42- ______________+____________ _____________+______________

Part C: Using your knowledge of pH and pOH and the equations below answer the following questions. Show all work!

Formulas

1) What is the pH of a 0.0235 M H2SO4 solution?

2) What is the pOH of a 0.0235 M HCl solution?

3) What is the pH of a 6.50 x 10-3 M Ca(OH)2 solution? (Hint: this is a basic solution)

4) What is the [H3O+] of a 6.2 x 10-5 M Ba(OH)2 solution?

5) A solution with an H3O+ concentration of 1.00 x 10-7 M is said to be neutral. Why?

6) Dr. Pepper has a [H+] = 1.4 x 10-5 M. What is its pH?

7) Fill in the chart below :

[H3O+]

[OH-]

pH

pOH

Acidic, Basic, or Neutral?

a.

1.5 x 10-3 M

b.

4.2 x 10-9 M

c.

8.72

d.

12

e.

Neutral

f.

1.8

g.

4.7

h.

2.0 x 10-6 M

i.

3.8 x 10-5 M

j.

13.1

k.

1 x 10-10 M

l.

2.67

Part D: Answer the following questions about acid-base neutralization reactions and titrations.

1) Fill in the table below. Indicate if the parent acid and parent base are strong or weak:

Parent Acid

Parent Base

Salt Produced (along with water)

Type of Salt (Acidic, Basic, Neutral, or Undetermined)

(strong/weak)

(strong/weak)

NaCl

HC2H3O2 (strong/weak)

Ba(OH)2 (strong/weak)

(strong/weak)

(strong/weak)

AgF

HClO3 (strong/weak)

LiOH (strong/weak)

(strong/weak)

(strong/weak)

CaSO4

HI (strong/weak)

Fe(OH)3 (strong/weak)

(strong/weak)

(strong/weak)

RbClO4

HNO3 (strong/weak)

Sr(OH)2 (strong/weak)

HBr (strong/weak)

KOH (strong/weak)

(strong/weak)

(strong/weak)

Cs2S

2) 25.0 mL of an unknown concentration of aluminum hydroxide is titrated with 45.5 mL of 0.750 M hydrochloric acid. What is the concentration of the aluminum hydroxide?

3) 100.0 mL of an unknown concentration of acetic acid is titrated. It requires 89.2 mL of 0.35 M sodium hydroxide to neutralize. What is the concentration of the acetic acid?

a. What would the pH be at the equivalence point for the titration above? ________________________

4) What volume of 0.25 M lithium hydroxide is needed to fully neutralize 30.0 mL of 0.90 M sulfuric acid?

a. What would the pH be at the equivalence point for the titration above? __________________________

5) What volume of 2.50 M nitric acid is needed to fully neutralize 230.0 mL of 1.00 M iron (II) hydroxide?

a. What would the pH be at the equivalence point for the titration above? __________________________

PART D CONTINUES ON THE NEXT PAGE!!

6) 250.0 mL of an unknown concentration of magnesium hydroxide is titrated with 305.0 mL of 0.350 M hydrobromic acid. What is the concentration of the magnesium hydroxide?

7) 10.0 mL of an unknown concentration of phosphoric acid is titrated. It requires 9.20 mL of 0.85 M cesium hydroxide to neutralize. What is the concentration of the phosphoric acid?

8) What volume of 0.66 M titanium (II) hydroxide is needed to fully neutralize 30.0 mL of 0.90 M chloric acid?

9) Clearly label the equivalence point on the titration curves below. Identify the titrant and analyte as strong/weak acid/base.

10) 80.00 mL of a weak monoprotic acid of an unknown concentration was titrated with 1.250 M potassium hydroxide. Using the titration curve to the right, calculate the concentration of the weak monoprotic acid.

11) The graph to the left was obtained when 15.0 mL of an unknown concentration of chloric acid was titrated with 0.450 M NaOH. Using the titration curve, calculate the concentration of chloric acid.

Part E: Using your knowledge of acids and bases, answer the following questions.

1) Fill in the following Venn diagram about properties of acids and bases. You must fill in at least 4 facts in each.

Properties of Acids

Properties of Bases

Both

2) Give an example of each of the following:

a.

b. Monoprotic acid: __________________

c. Diprotoic acid: ____________________

d. Triprotic acid: _____________________

e. Monobasic: ______________________

f. Dibasic: __________________________

g. Tribasic: _________________________

3)

4) Fill in the chart below:

List 3 Weak Acids

List 7 Strong Acids

List 3 Weak Bases

List 8 Strong Bases:

5) When describing an acid or a base, what do the terms strong and weak mean?

6) In your own words, what is the difference between Arrhenius’s definition and Bronsted-Lowry’s definition of acids and bases?

7) What type of substances are strong electrolytes?

8) What type of substances are weak electrolytes?

9) What is an amphoteric substance? Given an example of one.

PART E CONTINUES ON THE NEXT PAGE!!

10) Write the reaction for the auto ionization of water:

11) What is the formula for hydronium and how can be it abbreviated?

12) What are the similarities and difference between molecular equations, complete ionic equations, and net ionic equations?

13) What is a conjugate acid/base pair?

14) Explain how you would determine the acid, base, conjugate acid, and conjugate base when given a reaction. Be detailed.

15) If a substance has a high pH…. (circle your answers)

a. The substance is (ACIDIC/BASIC/NEUTRAL)

b. The substance has a (HIGH/LOW/NEUTRAL) hydronium ion concentration.

c. The substance has a (HIGH/LOW/NEUTRAL) pOH

d. The substance has a (HIGH/LOW/NEUTRAL) hydroxide ion concentration.

16) If a substance has a high hydronium ion concentration… (circle your answer)

a. The substance is (ACIDIC/BASIC/NEUTRAL)

b. The substance has a (HIGH/LOW/NEUTRAL) pH

c. The substance has a (HIGH/LOW/NEUTRAL) pOH

d. The substance has a (HIGH/LOW/NEUTRAL) hydroxide ion concentration.

17) What is a neutralization reaction?

18) What is the net ionic equation for the reaction between a strong acid and a strong base?

19) What is a buffer?

20) What is a buffer made of?

21) Give an example of a buffer and explain what it is used for.

22) List 3 ways to test a solution’s pH.

23) What is a titration?

24) In a titration, what is an equivalence point?

25) Draw and label a setup of a titration.

Solubility Rules

All compounds of the group I metals and NH4+ are soluble

All NO3-, ClO4-, ClO3-, C2H3O2- salts are soluble

All chlorides, bromides, and iodides are soluble except those with Ag+, Pb2+, Cu2+, Hg+, and Hg22+

All sulfates are soluble except those with Pb2+, Ca2+, Ba2+, Sr2+, Ag+, and Hg22+

All hydroxides and all metal oxides are insoluble except those combined with Group I, NH4+, Ca2+, Ba2+, and Sr2+

All PO43-, CO32-, SO32-, S2-, CrO42- and SCN- salts are insoluble except those with group I and NH4+