Name ____________________________________________ Period. _________

Chem RG Chapter Packet 15 Acids and Bases

Assign Section # Name 10 5

1. Assignment Sheet printed

2. Notes 15.1

3. Notes 15.2

4. Notes 15.3

5. Worksheet 15.1

6. Worksheet 15.2

7. Worksheet 15.3

Lab A13 Titrations (turn in separately for graded points)

Ch 15 Test Review (turn in separately for graded points)

(Total Points = 7 x 10 = 70)

Notes: 1. Your lab report is turned in by itself and receives a separate grade. 2. Your test reviews are graded separately. 3. Website: http://chem-rg-flipped.santiago.groupfusion.net/

EVIDENCE (after you take notes.) You should have at least 4 types of evidence for each set of notes. 1. Number new concepts 1,2,3…/A,B,C… 2. Delete/Cross out unimportant information Unimportant

3. Circle vocab/key terms 4. Identify points of confusion ?

5. Underline/Highlight main Ideas Main Ideas 6. Identify information to be used on a test, essay… *

7. Fill in gaps of information. Reword or paraphrase. ^ 8. Create visuals/symbols of important

information Visuals/symbol

s

Key Terms

_Mr. Nogales

Chem RG Experiment A13 – Titration

Objectives • Use burets to accurately measure volumes of solution. • Recognize the end point of a titration. • Describe the procedure for standardizing a solution. • Determine the molarity of a base.

Introduction Titration determines the concentration of a solution by measuring its volume needed to react completely with a standard solution. The point at which equal numbers of moles of acid and base are present is the equivalence point. An indicator is changes color to show when the equivalence point (or end point) is reached. Phenolphthalein is a good indicator for this titration because it is colorless in acids and turns pink in bases. At the equivalence point, the number of moles of acid equals the number of moles of base.

molarity of acid x volume of acid = molarity of base x volume of base In this experiment, you will be given a standard HCl solution and use it to find how much of the NaOH is needed to neutralize it. Using the data and equation below, you will then calculate the molarity of the NaOH solution. Materials • 0.500 M HCl • 50 mL burets, 2 • 100 mL beakers, 3 • 125 mL Erlenmeyer

flask

• double buret clamp • NaOH solution of

unknown molarity

• phenolphthalein indicator

• ring stand • wash bottle

Procedure 1. Set up the apparatus as shown in Figure A (see below). Label the burets NaOH and HCl.

Label two beakers NaOH and HCl. Place approximately 80 mL of the appropriate solution into each beaker. Use litmus paper to verify the solutions (don’t trust the labels). Don’t mix up the funnels.

2. Also Label the sides of the ring stand with masking tape as acid or base so you don’t mix up your burets.

3. This is a backwards titration. You will start with a pink solution and titrate until it’s clear. 4. Pour 5 mL of NaOH solution from its beaker into the NaOH buret. Rinse the walls of the

buret thoroughly with this solution. Allow the solution to drain through the stopcock into another beaker and discard it.

5. Fill the buret with NaOH solution above the zero mark. Withdraw enough solution to remove any air from the buret tip, and bring the liquid level down within the graduated region of the buret. It doesn’t have to be on the zero mark, but be sure to record where you start.

6. Repeat steps 4 and 5 with the HCl buret, using HCl solution to rinse and fill it.

7. For trial 1 record the initial reading of each buret, estimating to the nearest 0.01 mL in the Data Table. Keep your eyes level with the top of the liquid each time you read the buret. Always read the scale at the bottom of the meniscus.

8. Draw off about 10 mL of NaOH solution into an Erlenmeyer flask. Add 5 - 10 mL distilled water to increase the volume. The amount of water doesn’t change the number of moles, but it makes the volume greater so any error is proportionally less. Use the wash bottles to do this, but make sure they really have distilled water).

9. Then add one or two drops of phenolphthalein solution as an indicator. 10. Begin the titration by slowly adding HCl from the buret to the Erlenmeyer flask while

mixing the solution by swirling it as shown in Figure B bekiw. Stop frequently and wash down the inside surface of the flask using your wash bottle.

11. When the pink color of the solution begins to disappear at the point of contact with the acid, add the acid drop by drop (go slow at this time!), swirling the flask gently after each addition. When the last drop added causes the color to disappear from the whole solution and the color does not reappear, stop the titration. Use a white sheet of paper under the Erlenmeyer flask to make it easier to detect the color change.

12. Now add NaOH solution dropwise just until the pink color returns. Then add HCl again, dropwise, until the color just disappears. Go back and forth over the end point several times until one drop of the basic solution just brings out a faint pink color. Read the burets to the nearest 0.01 mL, and record these final readings in your data table. Read the burets correctly. They read top to bottom. What looks like 7.5 mL if you read from the bottom up is really 6.5 mL because you are reading from the top down.

13. Discard the liquid in the flask, rinse thoroughly with distilled water, and run a second trial. Record results for both trials.

14. Record the known concentration of the standard HCl solution in the data table. Look at the materials list for this value or read the label on the HCl. Be sure to list the molarity of HCl at bottom of data table.

15. Leave unused acid/base in the burets next period. 16. Clean your area.

DATA TABLE

CALCULATIONS 1. Organizing Data: Calculate the volumes of acid used in the two trials. Show your

calculations (final value minus initial value). Trial 1: Volume of HCl = _____________ Trial 2: Volume of HCl = _____________

2. Organizing Data Calculate the volumes of base used in the two trials. Show calculations Trial 1: Volume of NaOH = ___________ Trial 2: Volume of NaOH = ___________

3. Organizing Data Use the equation moles = molarity times volume to determine the moles of acid in each of the trials. Trial 1: Moles of acid = ___________ Trial 2: Moles of acid = ___________

4. Relating Ideas Write the balanced equation for the reaction between HCl and NaOH 5. Organizing Ideas Use the mole ratio from your balanced equation and the moles of acid

from Calculation # 3 above to find the moles of base neutralized in each trial using this formula: # mols from Calc #3 times mole ratio from the balanced equation = your answer. Show your calculations. Trial 1: Moles of base neutralized = _______ Trial 2: Moles of base neutralized = _______

6. Organizing Data Use the equation below and substitute in the results of Calculations #s 2 and 5 to find the molarity of the base for each trial. Show your calculations and be sure to convert mL to L.

M1V1n1 = M2V2n2 Trial 1: Molarity of NaOH __________ Trial 1: Molarity of NaOH __________ 7. Organizing Conclusions Calculate the average molarity of the base. Record your result.

ChemRG Ch 15 Acids & Bases 15.1 What are Acids & Bases?

• List the properties of acids and bases. • Describe the properties of strong & weak bases. • Define Arrhenius acids and bases. • Compare Arrhenius and Bronsted-Lowry acids and bases • Identify conjugate acid-base pairs.

Properties Acids Bases

Electrolytes ________

________Taste ________Taste

Turn litmus ________ Turn litmus ________

Reacts with ________ ________feel

Types of Acids and Bases 1. Arrhenius Definition

Acids produce ________ions (H1+) in aqueous solution.

Bases produce ________ions (OH1-) when dissolved in water. Acids produce H+ in aqueous solutions: Acid + HCl H+(aq) + Cl- (aq) Bases produce OH- in aqueous solutions: NaOH Na+(aq) + OH- (aq)

Learning Check Describe the solution in each of the following as: 1) acid 2) base or 3)neutral.

A. ___soda

B. ___soap C. ___coffee

D. ___ wine E. ___ water F. ___ grapefruit

Identify each as characteristic of an A) acid or B) base

____ 1. Sour taste

____ 2. Produces OH- in aqueous solutions

____ 3. Chalky taste

____ 4. Is an electrolyte

____ 5. Produces H+ in aqueous solutions

Some Common Acids HCl hydrochloric acid HNO3 nitric acid

H3PO4 phosphoric acid H2SO4 sulfuric acid

CH3COOH acetic acid

Strength

Strong acids and bases are strong ________ They fall apart (ionize) completely.

Weak acids don’t completely ionize. Strength is different from ________

2. Brønsted-Lowry Definitions

Acid is proton ________; ________is proton ________. Acids and bases always come in ________. HCl + H2O H3O+ + Cl- donor acceptor NH3, A Bronsted-Lowry Base NH3 + H2O NH4

+(aq) + OH- (aq) Acceptor donor

Acids and bases come in pairs General equation is: HA(aq) + H2O(l) H3O+(aq) + A-(aq) Acid + Base Conj acid + Conj base NH3 + H2O NH4

1+ + OH1-

base acid c.a. c.b. HCl + H2O H3O1+ + Cl1-

acid base c.a. c.b. Amphoteric - acts as acid ________base Identify the conjugate (either add or subtract a hydrogen ion) – write in your answers!

F 1-

H2PO41-

H2O

HF

H3PO4

H3O1+

Identify the conjugate

Br 1-

HSO41-

CO32-

HBr

H2SO4

HCO31-

HC 15.2 Acidity, Basicity, and pH

• Use Kw in calculations. • Define pH and give the pH of a neutral solution at 25o C. • Explain & use the pH scale. • Find pH from either [H3O1+] or [OH1-]. • Find either [H3O1+] or [OH1-] from pH.

Pure Water is Neutral Pure water contains small, but ________amounts of ions: H3O+ and OH-

Kw = [ H3O+ ] [ OH- ] = [ 1 x 10-7 ][ 1 x 10-7 ] = 1 x 10-14 Acids - Increase H3O+ (sometimes written as H1+). HCl (g) + H2O (l) H3O+ (aq) + Cl- (aq) As H3O+ increases, OH- decreases. So [H3O+] > [OH-]

Bases - Increase the hydroxide ions (OH-). NaOH (s) Na+(aq) + OH- (aq) When OH- increases, H3O+ decreases. So, [OH−] > [H3O+] Ion Product Constant H2O H+ + OH- Kw is constant in every aqueous solution: [H+] x [OH-] = 1 x 10-14 M2

If [H+] > 10-7 then [OH-] < 10-7 . If [H+] < 10-7 then [OH-] > 10-7

If we know one, the other can be determined If [H+] > 10-7 , it is acidic and [OH-] < 10-7 . If [H+] < 10-7 , it is basic and [OH-] > 10-7

Basic solutions also called “________” Using Kw to Calculate [H3O+ ] & [OH- ] The [OH- ] of a solution is 1.0 x 10- 3

M. What is the [H3O+]? Kw = [H3O+ ] [OH- ] = 1.0 x 10-14

[H3O+] = 1.0 x 10-14

[OH-] [H3O+] = 1.0 x 10-14 = 1.0 x 10-11 M Acidic or Basic? ________ 1.0 x 10- 3 Using the Calculator The [H3O+] of lemon juice is 4.0 x 10- 5 M. What is the [OH-]? 1.0 x 10 -14

4.0 x 10-5

Enter 1.0 EE +/- 14 ÷ 4.0 EE +/- 5 = 2.5 x 10-10 You try with your calculator The [OH-] of a solution is 5 x 10 -5 M. What is the [H3O+ ] of the solution? 1) 2 x 10- 5 M 2) 1 x 1010 M 3) 2 x 10-10 M (Do the calculation, circle answer) Learning Check 3: Do “A” in your head A.The [OH-] when [H3O+ ] of 1 x 10- 4 M is: 1) 1 x 10-6 M 2) 1 x 10-8 M 3) 1 x 10-10 M B.The [H3O+] when [OH- ] of 5 x 10-9 M is: 1) 1 x 10- 6 M 2) 2 x 10- 6 M 3) 2 x 10-7 M

pH and the pH Scale Indicates the acidity [H3O+] of the solution. pH = - log [H3O+] Since based on the logarithmic scale a change in one pH unit corresponds to a ________-fold change in [H3O+] (either stronger or weaker, depending if the pH went up or down).

pH For [H3O+] we see that 1 x 10-exponent = [H3O+] and the exponent = pH So, [H3O+] = 1 x 10-pH M Some [H3O+] and pH [H3O+] pH 1 x 10-5 M 5 1 x 10-9 M 9

1 x 10-11 M 11

Logarithms and the pH concept Logarithms are powers of ten.. Shorthand for big or small numbers Definition: pH = -log[H+]. In neutral pH = -log(1 x 10-7) = 7. In acidic solution pH < 7 (from 0 to 7 is the acid range) In base, pH > 7 (7 to 14 is base range) pH Scale Summary

Learning Check pH (Circle the correct answer) A. The [H3O+] of tomato juice is 1 x 10-4 M. What is the pH of the solution 1) - 4 2) 4 3) 8

B. The [OH-] of an NH3 solution is 1 x 10-3 M. What is the pH? 1) 3 2) 11 3 ) -11

pH and pOH – USEFUL FORMULAS pH + pOH = 14 [H+] x [OH-] = 1 x 10-14 = KW pH = -log[H3O1+] [H+] = 10-pH and [OH-] = 10-pOH pOH = -log[OH1-] [H3O1+] is the same as [H1+]

[H+],[OH-],pH and pOH: Given any one of these we can find the other three.

Sample Problem Given pH = 7.52, is it acidic or basic and what is pOH, [H3O1+] and [OH1-]?

The pH tells us it must be which? ________ since > than 7.00.

pOH = ? ________ since pH + pOH = 14.00

[H3O1+] = 10-pH so [H3O1+] = Calculator steps: 2nd , log , ± key (to make negative), 7.52 = 3.02 x 10-8

Given [H3O1+] = 3.02 x 10-8 and pOH = 6.48, both just calculated, what is [OH1-]? [OH1-] = 10-pOH = ? Calculator steps: 2nd log ± 6.48 = 3.31 x 10-7

Can also do by Kw = [H3O1+][OH1-] [OH1-] = 1.0 x 10-14/3.02 x 10-8 = 1 EE ± 14 ÷ 3.02 EE ± 8 = 3.31 x 10-7

Learning Check pH The pH of a soap is 10. What is the [H3O+] of the soap solution? 1) 1 x 10-4 M 2) 1 x 1010 M 3) 1 x 10-10 M [H3O+] = 1 x 10-pH M = 1 x 10-10 M Acidic or Basic? . . .Basic 2nd Learning Check pH A soap solution has a [H3O+] = 2 x 10-8 M. What is the pH of the solution Circle answer: 1) 8 2) 7.7 3) 6 (no calculators on 3rd Qtr Exam)

2nd Solution pH A soap solution has a [H3O+] = 2.0 x 10-8 M. What is the pH of the solution? pH = -log [H3O+] so . . . B) +/- LOG 2.0 EE +/- 8 = 7.7 Acidic or Basic? ________

3rd Learning Check pH Identify each solution as 1. acidic 2. basic 3. neutral

A. _____ HCl with a pH = 1.5

B. _____ Pancreatic fluid [H+] = 1 x 10-8 M

C. _____ Sprite soft drink pH = 3.0

D. _____ pH = 7.0

E. _____ [OH- ] = 3 x 10-10 M

F. _____ [H+ ] = 5 x 10-12

pH on the Calculator

[H3O+] is 4.5 x 10-6 M. pH = +/- LOG 4.5 EXP(or EE) +/- 6 ENTER = 5.35

pH Test Question What is the pH of 0.050 M HNO3? – SHOW YOUR WORK HERE

Acid-Base Indicators An indicator is a weak acid or base that undergoes dissociation in a known pH range, and has different colors in solution. Examples: litmus, phenolphthalein, bromthymol blue.

15.3 Neutralization & Titrations • Predict the product of an acid-base reaction. • Describe the equivalence point in a titration. • Explain how to select an indicator. • Describe how to do a titration.

Neutralization ACID + BASE → SALT + WATER COMPLETE THE FOLLOWING!

HNO3 + KOH →

2HCl + Mg(OH)2 →

H2SO4 + 2NaOH →

Balancing Neutralization Equations Write the equation for the neutralization between magnesium hydroxide and nitric acid. 1. Write the formulas of the acid and base: Mg(OH)2 + HNO3 2. Balance to give equal OH- and H+: Mg(OH)2 + 2 HNO3 3. Write the products of Mg(OH)2 + 2HNO3: Mg(OH)2 + 2HNO3 → Mg(NO3)2 + HOH 4. Balance products with the reactants: Mg(OH)2 + 2 HNO3 → Mg(NO3)2 + 2 HOH Learning Check: Write a balanced equation for H2SO4 used to neutralize KOH. Put your work here:

Titration Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

Equivalence point (endpoint) - Point at which ________ amounts of H3O+ and OH- have been added.

Determined by ________ color change

Molarity & Titration When you add the same number of moles of acid and base, the solution is ________. By measuring the amount of a base added you can determine the concentration of the acid IF you know the concentration of the base. 42.5 mL of 1.3 M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4. Titration problem: How many mL of 2.00 M H2SO4 are required to neutralize 50.0 mL of 1.00 M KOH? H2SO4 + 2KOH → K2SO4 + 2H2O M1 x V1 x # of H+ = M2 x V2 x # of OH-

(2M) x (V1) x (2) = (1M) x (50mL) x (1) V1 = 12.5 mL. You try: A 25 mL sample of H3PO4 is neutralized by 40. mL of 1.5 M NaOH. What is the molarity of the phosphoric acid solution? Use M1 x V1 x # H+ = M2 x V2 x # OH-

3NaOH + H3PO4 → Na3PO4 + 3H2O Answer? 1) 0.45 M 2) 0.80 M 3) 7.2 M

What to do if this is hard Do your worksheets (see the sample problems) Come to tutoring. Practice!!!

Acids and Bases 15.1 Worksheet

Name:______________________ Period:__________ Date:________ Use the following key to fill in the table:

a) Acid b) Base c) Both Acid and Base

___1. tastes bitter

___2. electrolyte

___3. increases [OH−]

___4. turns cabbage pink

___5. neutralizes NaOH

___6. increases [H+]

___7. tastes sour

___8. neutralizes HCl

___9. feels slippery

___10. decreases [OH−]

___11. turns cabbage blue/green

___12. proton donor

___13. decreases [H+]

___14. corrosive

___15. proton acceptor

State whether each chemical is an acid, or a base.

1. H2SO4 ________________

2. Mg(OH)2 ________________

3. HI ________________

4. HC2H3O2 ________________

5. NH4OH ________________

6. HNO3 ________________

7. NaOH ________________

8. HCl ________________

9. H2O2 ________________

0. HF ________________

READ THIS! Bronsted-Lowry theory: an acid is a proton (H+) donor and a base is a proton acceptor. (Leave the right side of the reaction unlabeled for now. You will complete it at the end of this worksheet) Label the Bronsted- Lowry acid & base & show the direction of the proton transfer by drawing an arrow with the H1+ ion.

Example: H2O + Cl - OH - + HCl

Acid Base Conjugate Base Conjugate Acid 1. H2O + H2O ↔ H3O + + OH - _____ _____ ______________ _____________ 2. H2SO4

- + OH - ↔ HSO4 2- + H2O

_____ _____ ______________ _____________ 3. HSO4

1- + H2O ↔ SO4

-2 + H3O +

_____ _____ ______________ _____________ 4. OH - + H3O + ↔ H2O + H2O

_____ _____ ______________ ______________ 5. NH3 + H2O ↔ NH4 + + OH -

_____ _____ ______________ ______________ READ THIS! After an acid has given up its proton, it is capable of getting back that proton and acting as a base. A conjugate base is what is left after an acid gives up a proton and is on the right (product) side of the arrow. 2. Fill in the missing information in the table below:

ACID Conjugate BASE EQUATION 1. H2SO4 HSO4

- H2SO4 → H + + HSO4 -

2. H3PO4 3. F - 4. NO3

- 5. H2PO4

- 6. H2O 7. SO4

-2 8. HPO4

-2

3. Finally, go back to the exercise at the top of the page/ Label the conjugate acid and the conjugate base for each reaction AND draw an arrow with the hydrogen ion.

Example: H2O + Cl - ↔ OH - + HCl

Acid Base Conjugate Base Conjugate Acid

H1+

pH Scale

pH [H30+] [OH-] pOH 0 1x100 1x10-14 14 Most Acidic 1 1x10-1 1x10-13 13 2 1x10-2 1x10-12 12 3 1x10-3 1x10-11 11 4 1x10-4 1x10-10 10 5 1x10-5 1x10-9 9 6 1x10-6 1x10-8 8 7 1x10-7 1x10-7 7 Neutral 8 1x10-8 1x10-6 6 9 1x10-9 1x10-5 5 10 1x10-10 1x10-4 4 11 1x10-11 1x10-3 3 12 1x10-12 1x10-2 2 13 1x10-13 1x10-1 1 14 1x10-14 1x100 0 Most Basic

Useful Equations [H30

1+] is same as [H1+]

pH = - log [H301+]

pOH = - log [OH-]

[H301+] = 10-pH

[OH-] = 10-(14.00-pH)

pH + pOH = 14.00

[H301+] x [OH1-] = 1.0 x 10-14

Use these examples to solve the problems in this worksheet AND on your online homework.

Find the pH of a solution with [H30+] = 8.6 x 10-9 M Find the pH of a solution with [OH-] = 1.3 x 10-2 M

pH = - log [H30+] pH = - log [OH-]

pH = - log (8.6 x 10-9) pH = - log (1.3 x 10-2)

pH = 8.07 pOH = 1.89

pH = 14.00 – 1.89 = 12.11

Find the [H30+] of a solution with a pH = 9.27 Find the [OH-] of a solution with a pH = 3.21

[H30+] = 10-pH [OH-] = 10-(14.00-pH)

[H30+] = 10-9.27 [OH-] = 10-(14.00-3.21)

[H30+] = 5.37 x 10-10 M [OH-] = 10-(10.79)

[OH-] = 1.62 x 10-11 M

Chem RG 15.2 Worksheet Name:_________________________________________________Date:_______________Period:________ 1. Find the pH of a solution with [H3O+] = 2.3 x 10-4 M._____________ Acidic or basic?_____________

2. Find the pH of a solution with [H3O+] = 7.42 x 10-11 M._____________ Acidic or basic?____________

3. Vinegar (acetic acid) has a pH of 2.4. Determine its [H3O+]. ______________. Acidic or basic?_________

4. Baking soda has a pH of 8.15. Find its [H3O+] solution.__________________. Acidic or basic?__________

5. Find the pOH for a solution with [OH-] = 5.5 x 10-3 M._____________ Acidic or basic?_____________

6. Find the pOH for a solution with [OH-] = 3.71 x 10-6 M._____________ Acidic or basic?____________

7. A 0.05 M soln of NaOH has 0.05 M OH-. Find its pOH _________, then convert pOH to pH___________.

8. In a blood sample [OH-] = 3.2 x 10-7 M. Find its pOH ________, then convert the pOH to pH_______.

9. The pOH of household ammonia is 2.5. Determine its [OH-]_________. Acidic or basic? __________

10. Lemon juice has a pH of 3.6. Find its [H3O+] _____________. Acidic or basic? ________

Selected Answers: 1) 3.64 acidic; 2) 10.13; 3) 3.98 × 10-3; 4)7.08 × 10-9; 5) 2.26 basic; 6) 5.43; 7) pOH 1.30, pH 12.7; 8) pOH 6.49, pH 7.51; 9) 3.16 × 10-3 basic; 10) 2.51 × 10-4 acidic

ChemRG 15.3 Worksheet Name:_________________________________________________Date:_______________Period:________ Use this formula (from your skeleton notes) moles H3O1+ = moles OH1- M = molarity V = volume M1 • V1 • n1 = M2 • V2 • n2 n1 = # of H1+ in the acid n2 = # of OH1- in the base Book page 556: Practice Problems (top of page) #1-2: 1. If 20.6 mL of 0.010 M aqueous HCl is required to titrate 30.0 mL of an aqueous solution of NaOH to the equivalence point, what is the molarity of the NaOH solution? Ans. 6.9 × 10-3. 2. In the titration of 35.0 mL of drain cleaner that contains NaOH, 50.08 mL of 0.409 M HCl must be added to reach the equivalence point. What is the concentration of the base in the cleaner? 9. What volume of 0.250 M nitric acid is needed to neutralize 17.35 mL of 0.195 M KOH solution? Ans. 13.5 mL 12. In a titration of a sample of 0.31 M HNO3, it took 75 mL of a 0.24 M KOH solution to reach a pH of 7. What was the volume of the sample? Ans. 58 mL

Chem RG Test Review Worksheet Name:_________________________________________________Date:_______________Period:________ Book pages 567-568: 40, 43, 46, 47, 59, 63, 75, 77 40. If [H3O1+] = 1.63 × 10-8 what is [OH1-]? Hint: Use Kw = [H3O1+] x [OH1-] = 1.00 × 10-14. Ans. 6.13 × 10-7 M 43. If [H3O1+] = 1.87 × 10-3 what is [OH1-]? Ans. 5.35 × 10-12 46. If stomach acid, ha [HCl] = 0.03 mol/L what is its pH? Hint: pH = -log[H1+]. Ans. 1.52 47. If [OH1-] = 0.0134 mol/L what is its pH? Hint: find pOH, then subtract from 14. Ans. 12.13 59. If pH = 9.5 what is [H3O1+]? [OH1-]? Hint: [H3O1+] = 10-pH, then use Kw as in #40. Ans. [H3O1+] = 3.2 × 10-10; [OH1-] = 3.2 × 10-5 63. What is [OH1-] if pH = 8.72. Hint: Find pOH by 14 - pH, then use Kw as in #40. Ans. 5.25 × 10-6 75. What volume of 0.100 M NaOH required to neutralize 25.00 mL of 0.110 M H2SO4? Ans. 55.0 mL Hint: use M1 • V1 • n1 = M2 • V2 • n2 77. If 35.40 mL of 1.000 M HCl is neutralized by 67.50 mL of NaOH, what is the [NaOH]? Ans. 0.5260 M

Chapter  15:  Test Review p. 2       Name:________________________________  Period:____    Acids:  Taste:    Turn  Cabbage  Juice:    Turn  Litmus    Usually:  Solid/Liquid/Gas  Pick  all  that  apply    Make:  Hydronium  Ions/Hydroxide  Ions    Make:  H3O

+/OH-­‐  

 Protons:  Donate/Accept      

Bases:  Taste:    Turn  Cabbage  Juice:    Turn  Litmus    Usually:  Solid/Liquid/Gas  Pick  all  that  apply    Make:  Hydronium  Ions/Hydroxide  Ions    Make:  H3O

+/OH-­‐  

 Protons:  Donate/Accept      

Explain  the  difference  between  strong  acids  and  bases  and  weak  acids  and  bases  in  terms  of  electrolytes:  ______________________         _____________________________________________________________________________________________________       _____________________________________________________________________________________________________    Who  defined  acids  and  bases  by  the  types  of  ions  they  produced?  ______________________________________________________    Who  defined  acids  and  bases  by  emphasizing  the  role  of  protons?  ______________________________________________________    Define  a  conjugate  acid:  ________________________________________________________________________________________    Define  a  conjugate  base:  _______________________________________________________________________________________    Define  amphoteric:  ____________________________________________________________________________________________    What  is  a  common  amphoteric  substance?  _________________________________________________________________________    Define  equivalency  point:  _______________________________________________________________________________________    In  a  neutralization  reaction  ___________________  is  always  a  product    Pure  water  contains  _______________________,  _______________________,  _______________________    What  can  we  say  about  the  following  reaction:  (hint,  look  at  the  products)?  ______________________________________________           HCl    +    NaOH    →    NaCl    +    H2O      Bronsted-­‐Lowry:    Label  the  acid,  base,  conjugate  acid,  and  conjugate  base  for  the  following  reactions                                                Draw  an  arrow  to  show  which  substance  donated  a  proton  and  which  substance  accepted  a  proton                                                                                                                                                      H2O          +              HC2H3O2

               ↔                  H3O  +                +          C2H3O2

-­‐                              HCl                  +                H2O                ↔                            Cl-­‐                            +                  H3O  

+  

   HNO3          +          H2O              ↔              NO3  

-­‐                +                H3O  +  

       H2O                +              HF                ↔                    H3O  

+                +                  F-­‐  

The  pH  of  a  solution  is  2.        

What  is  the  pOH?  _____________________    

What  is  the  H3O+  concentration?  ____________  

 What  is  the  OH-­‐  concentration?  _____________  

    Is  the  solution  an  acid/base/or  neutral  _______    The  H3O

+  concentration  of  a  solution  is  1  x  10  -­‐9.        

What  is  the  OH-­‐  concentration?  _____________    What  is  the  pH?  _____________________    What  is  the  pOH?  _____________________  

    Is  the  solution  an  acid/base/or  neutral  _______  

The  pOH  of  a  solution  is  1.        

What  is  the  pH?  _____________________    

What  is  the  H3O+  concentration?  ____________  

 What  is  the  OH-­‐  concentration?  _____________  

    Is  the  solution  an  acid/base/or  neutral  _______    The  OH-­‐  concentration  of  a  solution  is  1  x  10  -­‐13.        

What  is  the  H3O+  concentration?  _____________  

 What  is  the  pH?  _____________________    What  is  the  pOH?  _____________________  

    Is  the  solution  an  acid/base/or  neutral  _______  

 If  the  pH  of  a  solution  is  3,  what  is  its  H3O

+  concentration?  ______________________    If  the  pH  of  a  solution  is  12,  what  is  its  OH-­‐  concentration?  ______________________    What  is  the  pH  of  a  1  x  10  -­‐6  M  HCl  solution?  ______________________    What  is  the  pH  of  a  1  x  10  -­‐4  M  NaOH  solution?  ______________________    Is  a  solution  with  a  pH  of  5  acidic,  basic,  or  neutral?  _______________    pH  of  7?  _______________    pH  of  14?  _______________    Is  a  solution  with  a  pOH  of  5  acidic,  basic,  or  neutral?  ______________    pOH  of  7?  ______________    pOH  of  14?  ______________    What  is  the  molarity  of  an  HCl  solution  if  50.0  mL  is  neutralized  in  a  titration  by  40.0  mL  of  0.400  M  NaOH?          What  is  the  molarity  of  an  HCl  solution  if  125  mL  is  neutralized  in  a  titration  by  76.0  mL  of  1.22  M  KOH?          What  is  the  molarity  of  an  NaOH  solution  if  4.37  mL  is  titrated  by  11.1  mL  of  0.0904  M  HNO3?          What  is  the  volume  of  a  0.25  M  HCl  solution  if  it  is  neutralized  in  a  titration  by  20.0  mL  of  0.400  M  NaOH?          What  is  the  volume  of  a  5.5  M  HCl  solution  if  it  is  neutralized  in  a  titration  by  85.0  mL  of  1.22  M  KOH?          What  is  the  volume  of  a  7.34  M  NaOH  solution  if  it  is  titrated  by  10.5  mL  of  0.0904  M  HNO3?