Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Size: px
Start display at page:

Download "Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site."

Transcription

1 Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check out our Tutoring page to find the help you need. Good Luck!

2 NONE OF THE MULTIPLE CHOICE PROBLEMS REQUIRES EXTENSIVE OR TIME COMSUMING CALCULATIONS. IF YOUR METHOD REQUIRES EXTENSTIVE CALCULATIONS IT IS EITHER WRONG OR HARDER THAN WHAT IS REQUIRED. 1. A 0.1 M solution of each acid in the table is prepared. Which has the HIGHEST ph. Careful. a. Acetic b. Fluoroacetic c. Formic d. Hydrocyanic e. Hydrofluoric g NaOH is diluted to 5.0 L. What is the ph? a b c d e ml of 0.45 M HNO 3 is mixed with 200. ml of 0.55 M HCN? What is the ph? a b c d e ml of 0.30 M HNO 3 is mixed with 40. ml of 0.20 M HCl? What is the ph? a b c d e. 0.52

3 ml of 0.62 M HCl is mixed with 80. ml of 0.10 M KOH. What is the ph? a b c d e. >10 6. What is the hydrogen ion concentration of a 0.77 M HF? K a = 6.76 x 10-4 M. a. < 0.01 M b M c M d M e M 7. A M solution of a weak acid, HB, has a ph of What is K a? a. 1.8x10-4 M b. 1.3x10-4 M c. 2.5x10-7 M d. >10-2 M e. <10-8 M 8. Which of the following ions is neutral? a. Al 3+ + d. NH 4 b. Br - e. CBr 3 COO - c. F -

4 9. H 2 B (B = conjugate base) is a diprotic acid. A solution of 0.23 M KHB is prepared. Is it acidic, basic, or neutral? + 6 HBaq + HOaq HO aq + HB aq K = 510 x ( ) ( ) ( ) ( ) ( ) ( ) ( ) ( ) a1 HB aq + H O aq H O aq + B aq K = 2x a2 a. Neutral because K a and K b for HB - = 2x10-9. b. Acidic because K + is an acidic ion. c. Acidic because K a for HB - = 5x10-6 > K b for HB - = 2x10-9 d. Basic because K a for HB - = 2x10-9 < K b for HB - = 5x ml of 0.30 M acetic acid is added to 200 ml of 0.40 M sodium acetate. What is the ph? K a = 1.74 x a b c d e Hydoxylanime (NH 2 OH) is a weak base like ammonia. K b = 1.07x10-8 and pk b = It can be used to prepare a buffer solution whose ph is If the NH 2 OH concentration is M, what is the required NH 3 OH + concentration? Careful! a. < 0.1 M b M c M d M e. > 5 M 12. Buffers neutralize both acids and bases. When HBr is added to a buffer solution consisting of Sodium cyanide (NaCN) and hydrocyanic acid (HCN), which reaction (when completed) shows the neutralization of the acid? a. H (aq) +CN - (aq) b. H (aq) + Na + (aq) c. H (aq) + Br - (aq) d. H (aq) + HCN(aq) e. None of the above

5 ml of 0.20 M HCl is added to 60.0 ml of 0.75 M NaCH 3 COO. What is the ph of the resulting solution? (K a = 1.74 x 10-5 M for acetic acid.) a b c d e ( ) ( ) HO aq + CHCOO aq What is the ph of 0.55 M NaF. K a for HF is 6.76 x a b c d e In which of the following reactions does the underlined compound act as a either a BrØnsted- Lowry or Lewis base? (Note, I and II are different reactions.) I. HCO + H O H CO + OH II. HCO + H O CO + H O ( ) ( ) III. PH + B OH PH B OH where the P is bonded to the B (a) only I (b) only II (c) only III (d) I and II (e) I, II, and III 16. Which of the following solutions is not a buffer solution? a. 0.1 M acetic acid and 0.5 M conjugate base. b. 0.3 M Fe(H 2 O) 3+ 6 and 0.3 M Fe(H 2 O) 5 OH 2+ d. 0.2 M N(CH 3 ) and 1.4 M NH(CH 3 ) + e M H + - and 0.60 M NO 3

6 PROBLEMS (12 POINTS EACH) I. (a) The magnitude of the K sp of Fe(OH) 2 is 1.0 x at room temperature. (2 PTS) Write the solubility reaction or the solubility product expression (K sp =?): (b) (5 PTS) What is the solubility of Fe(OH) 2 in pure water at room temperature in mol/l? USE CORRECT NUMBER OF SIGNIFICANT FIGURES. (c) (5 PTS) What is the solubility of Fe(OH) 2 in a solution buffered to a ph of 11 at 25ºC?

7 II. 35 ml of a KCN are titrated with M HCl. (a) (3 PTS) What is the neutralization reaction? (b) (3 PTS) It takes 22.0 ml of the acid to reach the equivalence point (to neutralize all of the base). What was the initial concentration of KCN? (c) (3 PTS) After 11.0 ml of acid are added to the original solution the ph is What is K b for CN -? Hint, what is CN - converted to? (d) (3 PTS) What is the ph after 30 ml of acid are added to the original 35 ml of KCN?

8 III. Pot-pourri (a) (3 PTS) A solution of Pb(CH 3 COO) 2 is added to a solution of NaI. A yellow precipitate forms. What is it? + (b) (3 PTS) ( ) ( ) ( ) HO l H aq OH aq H 2 + > 0 7. What is the ph of pure water just above freezing? Explain why.. At room temperature the ph of pure water is (c) (4 PTS) The solubility product constant, K sp, of Ca(OH) 2 is 5.0 x10-6 M ml of M Ca(NO 3 ) 2 is added to 40. ml of a buffer solution having a ph of What is Q? Careful. (d) (2 PTS) In the last problem, does a precipitate form? Why? (No credit without proper justification--just a few words.)

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? heck out

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates

Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate

More information

Name Date Class ACID-BASE THEORIES

Name Date Class ACID-BASE THEORIES 19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary

More information

Solutions are aqueous and the temperature is 25 C unless stated otherwise.

Solutions are aqueous and the temperature is 25 C unless stated otherwise. Solutions are aqueous and the temperature is 25 C unless stated otherwise. 1. According to the Arrhenius definition, an acid is a substance that produces ions in aqueous solution. A. H C. OH B. H + D.

More information

Chapter 16: Acids and Bases

Chapter 16: Acids and Bases 1. Which is not a characteristic property of acids? A) neutralizes bases B) turns litmus from blue to red C) reacts with active metals to produce H 2 (g) D) reacts with CO 2 (g) to form carbonates E) All

More information

CHM 152/154 HOUR EXAM II Diebolt Summer multiple choice 52 Parts II and III 73 Total Pts 125

CHM 152/154 HOUR EXAM II Diebolt Summer multiple choice 52 Parts II and III 73 Total Pts 125 CHM 152/154 HOUR EXAM II Diebolt Summer 2010 pts earned name pts possible multiple choice 52 Parts II and III 73 Total Pts 125 Part One: Multiple choice. Mark the correct answers on the provided scantron

More information

ACIDS, BASES, AND SALTS

ACIDS, BASES, AND SALTS ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none

More information

Northern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006

Northern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006 Northern Arizona University Exam #3 CHM 152, General Chemistry II Dr. Brandon Cruickshank Section 2, Spring 2006 April 21, 2006 Name ID # INSTRUCTIONS: Code the answers to the True-False and Multiple-Choice

More information

Salt Hydrolysis Problems

Salt Hydrolysis Problems Salt Hydrolysis Problems Page 169 Salt Hydrolysis Problems 1) Write the Brønsted-Lowry reaction between the base CN! and the weak acid H 2 O. CN! + H 2 O W HCN + OH! 2) Write the Brønsted-Lowry reaction

More information

Northern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006

Northern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006 Northern Arizona University Exam #3 CHM 152, General Chemistry II Dr. Brandon Cruickshank Section 2, Spring 2006 April 21, 2006 Name ID # INSTRUCTIONS: Code the answers to the True-False and Multiple-Choice

More information

Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria

Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly

More information

Chem 112, Fall 05 Exam 3A

Chem 112, Fall 05 Exam 3A Before you begin, make sure that your exam has all 10 pages. There are 32 required problems (3 points each, unless noted otherwise) and two extra credit problems (3 points each). Stay focused on your exam.

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this mteril useful? You cn help our tem to keep this site up nd bring you even more content consider donting vi the link on our site. Still hving trouble understnding the mteril? Check out our Tutoring

More information

Chapter 14. Acids and Bases

Chapter 14. Acids and Bases Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton

More information

AP Chapter 15 & 16: Acid-Base Equilibria Name

AP Chapter 15 & 16: Acid-Base Equilibria Name AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show

More information

1032_2nd Exam_ (A)

1032_2nd Exam_ (A) 1032_2nd Exam_1040422 (A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Give the equation for a saturated solution in comparing Q with Ksp. A)

More information

Problem 1. What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10-5 )?

Problem 1. What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10-5 )? Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10-5 )? Problem 2 A 489mL sample of 0.5542M HNO 3 is mixed with 427mL sample of NaOH (which has a ph of 14.06).

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Consider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA?

Consider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA? ch16blank Page 1 Chapter 16: Aqueous ionic equilibrium Topics in this chapter: 1. Buffers 2. Titrations and ph curves 3. Solubility equilibria Buffersresist changes to the ph of a solution. Consider a

More information

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and

More information

Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria

Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good

More information

= ) = )

= ) = ) Basics of calculating ph 1. Find the ph of 0.07 M HCl. 2. Find the ph of 0.2 M propanoic acid (K a = 10-4.87 ) 3. Find the ph of 0.4 M (CH 3 ) 3 N (K b = 10-4.20 ) 4. Find the ph of 0.3 M CH 3 COO - Na

More information

General Chemistry II CHM 1046 E Exam 2

General Chemistry II CHM 1046 E Exam 2 General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of

More information

I II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is

I II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is 1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium

More information

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any

More information

Unit Nine Notes N C U9

Unit Nine Notes N C U9 Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release

More information

Acid/Base Definitions

Acid/Base Definitions Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases

More information

CHM 2046 Test #3 Review: Chapters , 15, & 16

CHM 2046 Test #3 Review: Chapters , 15, & 16 Chapter 14 1. For the following reaction Kc = 0.513 at 500 K. N 2 O 4 (g) 2 NO 2 (g) If a reaction vessel initially contains an N 2 O 4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations

More information

Chem1120pretest2Summeri2015

Chem1120pretest2Summeri2015 Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has

More information

CHEMISTRY 102 Fall 2010 Hour Exam III Page My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:

CHEMISTRY 102 Fall 2010 Hour Exam III Page My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: Hour Exam III Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml

More information

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.

Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check

More information

Ch 8 Practice Problems

Ch 8 Practice Problems Ch 8 Practice Problems 1. What combination of substances will give a buffered solution that has a ph of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K a for NH 4 = 5.6 10 10 ;

More information

Problem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x

Problem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10 5 )? Write out acid dissociation reaction: C 6 H 5 COOH C 6 H 5 COO H Make an ICE chart since this is a weak

More information

Completion of acid/base/buffer chemistry. Hanson Activity Clicker quiz 3/11/2013. Chs 7 8 of Zumdahl

Completion of acid/base/buffer chemistry. Hanson Activity Clicker quiz 3/11/2013. Chs 7 8 of Zumdahl Completion of acid/base/buffer chemistry Chs 7 8 of Zumdahl Hanson Activity 16 3 Discuss Key Questions 1 of Activity 16 3, page 301, with your partner for three minutes. The clicker quiz will commence

More information

SCH4U Chapter 8 review

SCH4U Chapter 8 review Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic

More information

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate

More information

Strong and Weak. Acids and Bases

Strong and Weak. Acids and Bases Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF

More information

Chem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation

Chem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation Chem 106 3--011 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation 3//011 1 The net ionic equation for the reaction of KOH(aq) and

More information

Chem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice

Chem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice Chem 103 Exam #1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry

More information

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O.

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O. 1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H O. HCN + H O º H O + + CN ) Write the Brønsted-Lowry reaction for weak base NH reacting with H O NH + H O º OH + NH + ) Using the

More information

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion. Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when

More information

5. What is the percent ionization of a 1.4 M HC 2 H 3 O 2 solution (K a = ) at 25 C? A) 0.50% B) 0.36% C) 0.30% D) 0.18% E) 2.

5. What is the percent ionization of a 1.4 M HC 2 H 3 O 2 solution (K a = ) at 25 C? A) 0.50% B) 0.36% C) 0.30% D) 0.18% E) 2. Name: Date: 1. For which of the following equilibria does K c correspond to an acid-ionization constant, K a? A) NH 3 (aq) + H 3 O + (aq) NH 4 + (aq) + H 2 O(l) B) NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H

More information

k 1 I 2 2 I k -1 k 2 2 HI H I

k 1 I 2 2 I k -1 k 2 2 HI H I Example: Write the overall reaction and the rate law for the reaction that occurs in the following two steps. The second step is the rate determining step. I 2 k 1 k -1 2 I H 2 + 2 I k 2 2 HI Example.

More information

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH

More information

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species 3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates

More information

Chem1120pretest2Summeri2015

Chem1120pretest2Summeri2015 Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward

More information

Chemistry Lab Equilibrium Practice Test

Chemistry Lab Equilibrium Practice Test Chemistry Lab Equilibrium Practice Test Basic Concepts of Equilibrium and Le Chatelier s Principle 1. Which statement is correct about a system at equilibrium? (A) The forward and reverse reactions occur

More information

REVIEW QUESTIONS Chapter Identify the Lewis acid and base in each of the following reactions:

REVIEW QUESTIONS Chapter Identify the Lewis acid and base in each of the following reactions: Chemistry 102 REVIEW QUESTIONS Chapter 16 1. For each reaction below, identify the Brønsted-Lowry acid and base and their conjugates: A) NH 4 + (aq) + CN (aq) HCN (aq) + NH 3 (aq) B) (CH 3 ) 3 N (aq) +

More information

AP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga

AP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the

More information

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base Acid-Base Equilibria 1 Will the following salts be acidic, basic or neutral in aqueous solution? 1.NH 4 Cl.NaCl.KC H O 4.NaNO A = acidic B = basic C = neutral Solutions of a Weak Acid or Base The simplest

More information

Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute)

Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) CHAPTER 16: ACID-BASE EQUILIBRIA Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) A. Weak Monoprotic Acids. (Section 16.1) 1. Solution of Acetic Acid: 2. See Table

More information

Acid / Base Properties of Salts

Acid / Base Properties of Salts Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,

More information

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin)

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 2 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a

More information

a) most likely to gain two electrons Br O Al Mg b) greatest tendency to form a negative ion Na Li S Mg c) a non-metal Sr S Al K

a) most likely to gain two electrons Br O Al Mg b) greatest tendency to form a negative ion Na Li S Mg c) a non-metal Sr S Al K 1. (4 pts) Name the following compounds: Al 2 (SO 4 ) 3 N 2 O 3 2. (4 pts) Give the chemical formulas for the following compounds: chromium (III) carbonate magnesium phosphate 3. (16 pts) Circle the formula

More information

Acid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.

Acid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated. Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators

More information

(for tutoring, homework help, or help with online classes)

(for tutoring, homework help, or help with online classes) www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 16.1-27 The ph of a 0.10 M solution of a weak base is 9.82. What is the K b for this base? A. 8.8 10-8 B. 2.1

More information

CHE 107 Spring 2017 Exam 3

CHE 107 Spring 2017 Exam 3 CHE 107 Spring 2017 Exam 3 Your Name: Your ID: Question #: 1 What is the ph of a 0.20 M solution of hydrocyanic acid at 25ºC? The Ka of HCN at 25ºC is 4.9 10 10. A. 2.08 B. 5.00 C. 3.89 D. 8.76 Question

More information

Judith Herzfeld 1996,1998. These exercises are provided here for classroom and study use only. All other uses are copyright protected.

Judith Herzfeld 1996,1998. These exercises are provided here for classroom and study use only. All other uses are copyright protected. Judith Herzfeld 1996,1998 These exercises are provided here for classroom and study use only. All other uses are copyright protected. 3.3-010 According to Bronsted-Lowry Theory, which of the following

More information

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

Ch 16 and 17 Practice Problems

Ch 16 and 17 Practice Problems Ch 16 and 17 Practice Problems The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,

More information

Chemistry 12 Dr. Kline 26 October 2005 Name

Chemistry 12 Dr. Kline 26 October 2005 Name Test 1 first letter of last name Chemistry 12 Dr. Kline 26 October 2005 Name This test consists of a combination of multiple choice and other questions. There should be a total of 24 questions on 8 pages;

More information

Unit 6: ACIDS AND BASES

Unit 6: ACIDS AND BASES Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric

More information

Unit 9: Acid and Base Multiple Choice Practice

Unit 9: Acid and Base Multiple Choice Practice Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.

More information

Chapter 14: Acids and Bases

Chapter 14: Acids and Bases Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many

More information

Questions #4-5 The following two questions refer to the following system: A 1.0L solution contains 0.25M HF and 0.60M NaF (Ka for HF = 7.2 x 10-4 ).

Questions #4-5 The following two questions refer to the following system: A 1.0L solution contains 0.25M HF and 0.60M NaF (Ka for HF = 7.2 x 10-4 ). Multiple Choice 1) A solution contains 0.250 M HA (K a = 1.0 x 10-6 ) and 0.45 M NaA. What is the ph after 0.10 mole of HCl is added to 1.00L of this solution? a. 3.17 b. 3.23 c. 6.00 d. 10.77 e. 10.83

More information

Acid Base Review Package

Acid Base Review Package Acid Base Review Package 1. In which of the following eqb systems is HCO 3 acting as a BronstedLowry base? 2 a. HCO 3 H+ + CO 3 b. HCO 3 + HS 2 H 2 S + CO 3 c. HCO 3 + H 2 S H 2 CO 3 + HS d. HCO 3 + H

More information

AP Study Questions

AP Study Questions ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025

More information

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

X212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2

X212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2 PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste

More information

Formation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic

Formation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic Formation of a salt (ionic compound): Neutralization reaction molecular Full ionic Eliminate spect ions to yield net ionic Hydrolysis/ reaction with water Anions of Weak Acids Consider the weak acid HF

More information

Acids and Bases Written Response

Acids and Bases Written Response Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink

More information

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions? JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a

More information

Exam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]=

Exam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]= Chem 101B Study Questions Name: Chapters 14,15,16 Review Tuesday 3/21/2017 Due on Exam Thursday 3/23/2017 (Exam 3 Date) This is a homework assignment. Please show your work for full credit. If you do work

More information

ACIDS AND BASES. for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet

ACIDS AND BASES. for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet ACIDS AND BASES for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet Learning objectives Name and write formulae for common acids and bases Describe acids and bases according

More information

Chem 401 Unit 3 Exam F18 (Buffers, Titrations, Ksp, Transition Metals & Electrochemistry)

Chem 401 Unit 3 Exam F18 (Buffers, Titrations, Ksp, Transition Metals & Electrochemistry) Seat #: Date: Chem 401 Unit 3 Exam F18 (Buffers, Titrations, Ksp, Transition Metals & Electrochemistry) Multiple Choice Identify the choice that best completes the statement or answers the question. (4.2pts

More information

Reactions in Aqueous Solutions I: Acids, Bases & Salts

Reactions in Aqueous Solutions I: Acids, Bases & Salts 10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER GOALS 1. Properties of Aqueous Solutions of Acids and Bases 2. The Arrhenius Theory 3. The Hydronium Ion (Hydrated Hydrogen Ion) 4. The

More information

Unit 2 Acids and Bases

Unit 2 Acids and Bases Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions

More information

8.1 Theories of acids and bases

8.1 Theories of acids and bases 8. Acids and bases 8.1 Theories of acids and bases Sour-tasting substances (acids) have been known for thousands of years. Lavoisiers early theory: Acid= a compound of oxygen and a nonmetal. Arrhenius

More information

Practice test Chapters 15 and 16: Acids and Bases

Practice test Chapters 15 and 16: Acids and Bases Name: Class: Date: Practice test Chapters 15 and 16: Acids and Bases 1. Which of the following pairs of species is not a conjugate acid base pair? A) HOCl, OCl B) HNO 2, NO + 2 C) O 2, OH D) HSO 4, SO

More information

Please print: + log [A- ] [HA]

Please print: + log [A- ] [HA] Please print: Last name: First name: Chem 1062 Exam 3 Spring 2005 Andy Aspaas, Instructor Thursday, April 7, 2005 Equations: K c = [C]c [D] d [A] a [B] b ph =! log[h 3 O + ] poh =! log[oh! ] ph + poh =

More information

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression. Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products

More information

Part 01 - Assignment: Introduction to Acids &Bases

Part 01 - Assignment: Introduction to Acids &Bases Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4

More information

Chemistry I Notes Unit 10: Acids and Bases

Chemistry I Notes Unit 10: Acids and Bases Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,

More information

CHE 107 Summer 2017 Exam 3

CHE 107 Summer 2017 Exam 3 CHE 107 Summer 2017 Exam 3 Question #: 1 What is the ph of a 0.10 M hydrocyanic acid (HCN) solution. Ka = 4.9 10-10. A. 2.56 C. 4.04 B. 3.17 D. 5.15 Question #: 2 Original Windex has a ph = 11.60 and [H

More information

Chem1120pretest2Summeri2016

Chem1120pretest2Summeri2016 Chem1120pretest2Summeri2016 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has

More information

Chapter 10. Acids and Bases

Chapter 10. Acids and Bases Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.

More information

CH 15 Summary. Equilibrium is a balance between products and reactants

CH 15 Summary. Equilibrium is a balance between products and reactants CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium

More information

Name AP Chemistry January 25, 2013

Name AP Chemistry January 25, 2013 Name AP Chemistry January 25, 2013 AP Chemistry Midterm Exam Part I: 75 Questions, 80 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on your scantron for each of the following.

More information

CHEM Dr. Babb s Sections Exam #3 Review Sheet

CHEM Dr. Babb s Sections Exam #3 Review Sheet CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry

More information

Chemistry 1A Fall 2013 MWF 9:30 Final Test Form A

Chemistry 1A Fall 2013 MWF 9:30 Final Test Form A Chemistry 1A Fall 2013 MWF 9:30 Final Test Form A 1. How many moles of P 4 molecules are in 141.4 g of phosphorus? A) 4.566 mol B) 1.752 x10 4 mol C) 1.141 mol D) 2.348 x 10 1 mol E) 1.414 x 10 1 mol 2.

More information

Chapter 15. Acid-Base Equilibria

Chapter 15. Acid-Base Equilibria Chapter 15 Acid-Base Equilibria Section 15.1 Solutions of Acids or Bases Containing a Common Ion Common Ion Effect Shift in equilibrium position that occurs because of the addition of an ion already involved

More information

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many

More information

7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M

7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)

More information

CHEM 212 Practice Exam 2 1

CHEM 212 Practice Exam 2 1 CHEM 212 Practice Exam 2 1 1. In the following reaction NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H 3 O + (aq) a. NH 4 + is an acid and NH 3 is its b. H 2 O is an acid and H 3 O + is its c. NH 4 + is an acid

More information

Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2

Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution

More information

CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).

CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ). CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).

More information