Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.
|
|
- Amos Gilbert
- 6 years ago
- Views:
Transcription
1 Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following acids and bases. 6. HNO H 3 PO 3 7. HClO 11. KOH 8. H 2 SO H 2 CO 3 9. HC 2 H 3 O CH 3 NH 2 Acid and Base Definitions 1. Identify each of the following as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. The first one is done for you. a. HNO 3 (aq) acid, HNO 3 (aq) H + (aq) + NO 3 (aq) b. KOH(aq) c. HC 2 H 3 O 2 (aq) d. Sr(OH) 2 2. Identify each of the following as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. NaOH(aq) b. HBr(aq) c. Sr(OH) 2 (aq) d. H 2 SO 4 (aq) 3. For each of the following, identify the Bronsted-acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. a. HBr(aq) + H 2 O(l) H 3 O + (aq) + Br - (aq) Unit 11 Student Handout 1
2 b. NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH - (aq) c. HNO 3 (aq) + H 2 O(l) H 3 O + (aq) + NO 3 - (aq) d. C 5 H 5 N(aq) + H 2 O(l) C 5 H 5 NH + (aq) + OH - (aq) 4. Which of the following are conjugate acid-base pairs? a. NH 3, NH 4 + b. HCl, HBr c. C 2 H 3 O 2 -, HC 2 H 3 O 2 d. HCO 3 -, NO 3-5. Which of the following are conjugate acid-base pairs? a. HI, I - b. HCHO 2, SO 4 2- c. PO 4 3-, HPO 4 2- d. CO 3 2-, HCl 6. Write the dissociation equation for each of the following acids or bases in water. Identify the conjugate acid/base pairs. The first one is done for you: a. HI(aq) + H 2 O(l) H 3 O + (aq) + I - (aq) Acid base conj acid conj base b. CH 3 NH 2 c. CO 3 2- d. H 2 CO 3 7. Write the dissociation equation for each of the following acids or bases in aqueous solution. Identify the conjugate acid/base pairs. a. HCl b. H 2 SO 3 c. HClO d. HCHO 2 e. HF 8. Write the formula for the conjugate acid of each of the following bases. a. CH 3 NH 2 b. C 5 H 5 N Unit 11 Student Handout 2
3 c. Cl - d. F - Strong Acids and Strong Bases REVIEW!! Strong Acids StrongBases Hydrochloric, HCl All Alkali metal hydroxides LiOH, KOH, NaOH, etc. Hydrobromic, HBr Ca(OH) 2 Hydroiodic, HI Ba(OH) 2 Perchloric, HClO 4 Sr(OH) 2 Chloric, HClO 3 Sulfuric, H 2 SO 4 Nitric, HNO 3 * If an acid or base is not listed in the above list it can be considered weak. * Keep in mind that conjugate acids/bases of STRONG acids/bases are considered WEAK. * Keep in mind that conjugate acids/bases of WEAK acids/bases are considered STRONG. Strong and Weak Acids and Bases 9. Classify each of the following acids as strong or weak. Write its conjugate base and classify it as weak or strong. The first one is done for you: a. HCHO 2 weak acid CHO strong base b. HCl c. HNO 3 d. H 2 CO 3 e. HC 2 H 3 O 2 f. H 3 PO 3 Acide/Base Equilibria: K a, K b, K w 10. Butylamine (C 4 H 9 NH 2 ) is a weak base. If the initial concentration of butylamine is M and the equilibrium concentration of hydroxide ion is 8.6 x 10 6 M, calculate the K b for butylamine. Answ: 3.2x10-10 Unit 11 Student Handout 3
4 11. If mol of a weak acid is dissolved in water to a total volume of 0.75 L. At equilibrium the concentration of hydronium ion is M, calculate the K a for this acid. Answ: 6.3x Phenol (C 6 H 5 OH), commonly called carbolic acid, is a weak organic acid (K a = 1.3 x ). First, write the dissociation equation. If you dissolve g of the acid in enough water to make 125 ml of solution, what is the equilibrium hydronium ion concentration? What is the ph of the solution? Answ: [H 3 O + ]=1.50x10-6 M, ph = The weak base methylamine, CH 3 NH 2, has K b = 4.2x10-4. First, write the dissociation equation. Calculate the equilibrium hydroxide ion concentration in a 0.25 M solution of the base. What are the ph and poh of the solution? Answ: [OH - ]=1.0x10-2 M, ph = What is the hydronium ion concentration in 0.1 M ammonia if hydroxide ion concentration = 1.26 x 10 3 M? Is ammonia acidic, basic, or neutral? Answ: [H 3 O + ]=7.94x10-12 M, ph = 11, basic Unit 11 Student Handout 4
5 15. What is the hydroxide ion concentration in butter if hydronium ion concentration = 6.00 x 10 7 M? Is butter acidic, basic, or neutral? Answ: [OH - ]=1.67x10-8 M, ph = 6.22, slightly acidic 16. During the course of the day, human saliva varies between acidic and basic. What is the hydronium ion concentration in saliva if hydroxide ion concentration = 3.16 x 10 8 M? Is this sample of saliva acidic, basic, or neutral? Answ: [H 3 O + ]=3.16x10-7 M, ph = 6.50, slightly acidic 17. Determine [H 3 O + ] in each of the following acid solutions. For weak acids, give what [H 3 O + ] is less than. The first one is done for you. a. 2.5 M HI - [H 3 O + ] is 2.5 M b. 1.2 M HClO 2 - [H 3 O + ] is less than 1.2 M c M HClO 3 d M HNO Classify each of the following bases as strong or weak. a. C 5 H 5 N b. NaOH c. Ba(OH) 2 d. CO Determine [OH - ] in each of the following base solutions. For weak bases, give what [OH - ] is less than. a M NaOH b M NH 3 c M Sr(OH) 2 Unit 11 Student Handout 5
6 d M KOH ph and poh Calcualtions 20. Calculate [OH - ] given [H 3 O + ] in each of the following aqueous solutions and classify the solution as acidic or basic. a. [H 3 O + ] = 1.5 x 10-9 M b. [H 3 O + ] = 9.3 x 10-9 M c. [H 3 O + ] = 2.2 x 10-6 M d. [H 3 O + ] = 7.4 x 10-4 M 21. Calculate the ph of each of the following solutions. a. [H 3 O + ] = 1.7 x 10-8 M b. [H 3 O + ] = 1.0 x 10-7 M c. [H 3 O + ] = 2.2 x 10-6 M d. [H 3 O + ] = 7.4 x 10-4 M 22. Calculate [H 3 O + ] for each of the following solutions. a. ph = 8.55 b. ph = c. ph = 2.87 d. ph = Calculate [OH - ] for each of the following solutions. a. ph = 4.25 b. ph = c. ph = 1.50 d. ph = Calculate the ph of each of the following solutions: a M HBr b x 10-3 M KOH c x 10-3 M HNO 3 d x 10-4 M Sr(OH) 2 Unit 11 Student Handout 6
7 25. Calculate the poh of each of the following solutions: a x 10-3 M HClO 4 b M NaOH c M HBr d x 10-5 M Ba(OH) 2 Acid-Base Reactions 26. Write neutralization reactions for each of the following acids and bases. a. HI(aq) and NaOH(aq) b. HBr(aq) and KOH(aq) c. HNO 3 (aq) and Ba(OH) 2 (aq) d. HClO 4 (aq) and Sr(OH) 2 (aq) 27. Write neutralization reactions for each of the following acids and bases. a. HF(aq)and Ba(OH) 2 (aq) b. HClO 4 (aq) and NaOH(aq) c. HBr(aq) and Ca(OH) 2 (aq) d. HCl(aq) and KOH(aq) 28. Explain how a neutralization reaction is different from a dissociation equation. Provide an example of each. Acid-Base Titrations 29. Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCl solution, the volume of NaOH solution required to reach the endpoint, and the concentration of each NaOH solution. Calculate the concentration (in M) of the unknown HCl solution in each case. HCl Volume (ml) [HCl] (M) NaOH Volume (ml) [NaOH] (M) (a) ml ml M (b) 15.00mL ml M Unit 11 Student Handout 7
8 30. Four solutions of unknown NaOH concentration are titrated with solutions of HCl. The following table lists the volume of each unknown NaOH Solution, the volume of HCl solution required to reach the endpoint, and the concentration of each HCl solution. Calculate the concentration (in M) of the unknown NaOH solution in each case. NaOH Volume (ml) [NaOH] (M) HCl Volume (ml) [HCl] (M) (a) 5.00 ml 9.77 ml M (b) ml 11.34mL M 31. A mL sample of an H 2 SO 4 solution of unknown concentration is titrated with a M KOH solution. A volume of ml of KOH was required to reach the endpoint. What is the concentration of the unknown H 2 SO 4 solution? Answ: M 32. A 5.00-mL sample of an H 3 PO 4 solution of unknown concentration is titrated with a M NaOH solution. A volume of 5.99mL of the NaOH solution was required to reach the endpoint. What is the concentration of the unknown H 3 PO 4 solution? Answ: M 33. What volume in milliliters of a M NaOH solution is required to reach the endpoint in the complete titration of a 10.0-mL sample of M H 2 SO 4? Answ: 27.3 ml Unit 11 Student Handout 8
9 34. What volume in milliliters of M NaOH solution is required to reach the endpoint in the complete titration of a 15.0-mL sample of M H 3 PO 4? Answ: 48.6 ml Acid-Base Hydrolysis Hydrolysis occurs when certain salts dissolve in water to form solutions that have acidic or basic properties. A rule for predicting the properties of solutions of salts is based upon the concept of strong acids and strong bases in the Bronsted-Lowry sense. The rules are summarized in the table below: Salt formed from Water solution exhibits Example Strong acid + strong base no hydrolysis - neutral solutions KCl Strong acid + weak base hydrolysis to form acidic solution NH 4 SO 4 Weak acid + strong base hydrolysis to form basic solution Na 2 CO 3 Weak acid + weak base Must use K a and K b to determine Pb(C 2 H 3 O 2 ) 2 The commonly used strong acids are hydrochloric, nitric and sulfuric. The commonly used strong bases are sodium hydroxide, potassium hydroxide, and calcium hydroxide. Predict the hydrolysis effect of each of the following salts. For each answer write acidic, basic neutral or need K a and K b. 1. Na 3 PO 4 2. Na 2 SO 4 3. NaC 2 H 3 O 2 4. NH 4 NO 3 5. NH 4 Cl 6. Fe 3 (PO 4 ) 2 7. Ca(NO 3 ) 2 8. KC 2 H 3 O 2 9. CuSO Al(NO 3 ) NaCl 12. K 2 CO 3 Cummulative 35. A g sample of a monoprotic acid of unknown molar mass is dissolved in water and titrated with M NaOH. The endpoint is reached after adding ml of base. What is the molar mass of the unknown acid? Answ: 60.0 g/mol Unit 11 Student Handout 9
10 36. A 0.1O5-g sample of a diprotic acid of unknown molar mass is dissolved in water and titrated with M NaOH. The endpoint is reached after adding 15.2 ml of base. What is the molar mass of the unknown acid? Answ: 107 g/mol 37. Antacids, such as milk of magnesia, are often taken to reduce the discomfort of acid stomach or heartburn. The recommended dose of milk of magnesia is 1 teaspoon, which contains 400 mg of Mg(OH) 2. What volume of HCl solution with a ph of 1.1 can be neutralized by 1 dose of milk of magnesia? (Assume two significant figures in your calculations.) Answ: 170 ml 38. For each of the following strong base solutions, determine [OH - ], [H 3 O + ], and ph. a. 0.15M NaOH b. 8.7 x 10-5 M KOH 39. For each of the following weak base solutions, determine [OH - ], [H 3 O + ], and ph. a. Al(OH) 3 (Ksp = 3.0x10-34 ) b. Cd(OH) 2 (Ksp = 7.2x10-15 ) Unit 11 Student Handout 10
11 40. Methylamine, CH 3 NH 2, is a weak base. If the ph of a M solution of the amine is 11.70, what is the value of K b? Answ: 3.8x10-4 M 41. A popular classroom demonstration consists of filing notches into a new penny and soaking the penny in hydrochloric acid overnight. Since new pennies are made of zinc coated with copper, and since hydrochloric acid dissolves zinc and not copper, the inside of the penny is dissolved by the acid, while the outer copper shell remains. Suppose the penny contains 2.5 g of zinc and is soaked in 20.0mL of 6.0M HCl. Calculate the concentration of the HCl solution after all of the zinc has dissolved. Calculate the ph and poh of the resulting solution. Answ: [HCl] = 2 M, ph = -0.3, poh = What is the ph of a solution formed by mixing ml of M HCl with 75.0 ml of M NaOH? Answ: ph = Calculate the hydroxide ion concentration and the ph of the solution that results when 22.0 ml of 0.15 M of acetic acid is mixed with 22.0 ml of 0.15 M NaOH. (Remember salt hydrolysis. What type of salt is formed from the reaction of acetic acid with NaOH? What side-reaction will occur as a result of this salt dissolving in water? Kb: C 2 H 3 O 2 - = 5.6x10-10 ) Answ: [OH - ]=6.5x10-6 M, poh = 5.2, ph = 8.8 (The side reaction is the acetate conj base reacting with water!) Unit 11 Student Handout 11
12 44. How many H + (or H 3 O + ) ions are present in one drop (0.050 ml) of pure water at 25 C? Answ: [H 3 O + ]=1.x10-7 M, 3.0x10 12 ions 60. You are titrating a 50.0 ml sample of hydrochloric acid with M potassium hydroxide. After you have already added 42.3 ml of the potassium hydroxide you realize that you forgot to add the phenolphthalein indicator. When you add the indicator, the solution turns bright pink indicating that you have already missed the end point. You decide to back-titrate by adding M nitric acid. The solution turns colorless after an addition of 10.1 ml of the nitric acid. What is the concentration of the original solution of hydrochloric acid? Answ: M Unit 11 Student Handout 12
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 informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationIndicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus
Unit 9: Acids and Bases Notes Introduction and Review 1. Define Acid: 2. Name the following acids: HCl H2SO4 H2SO3 H2S 3. Bases usually contain 4. Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Properties
More informationNotes: Acids and Bases
Name Chemistry Pre-AP Notes: Acids and Bases Period I. Describing Acids and Bases A. Properties of Acids taste ph 7 Acids change color of an (e.g. blue litmus paper turns in the presence of an acid) React
More informationName. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com
Periodic Table Name Academic Chemistry Acids & Bases Notes Unit #14 Test Date: 20 cincochem.pbworks.com Acid Base cincochem.pbworks.com Notes Find ph To go from [H 3 O + ] to ph EXAMPLE: [H 3 O + ] = 3.23
More informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
More informationTopic 9: Acids & Bases
Topic 9: Acids & Bases Regents Chemistry Mr. Mancuso Electrolytes Substances that conduct electricity when Include Ability to conduct electricity is due to the presence of Dissociation: ~ 1 ~ Acids and
More informationChapter 10 - Acids & Bases
Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic
More information-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form
NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:
More informationUnit 9: Acids and Bases Chapter 19
Unit 9: Acids and Bases Chapter 19 I. Introduction In aqueous solutions, the solvent is. Aqueous solutions contain. In the self-ionization of water, the hydrogen ion (H+) exists in solution as the ion.
More informationAcids and Bases. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationAcids and Bases. Properties, Reactions, ph, and Titration
Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some
More informationAcids and Bases. Acid. Acid Base 2016 OTHS. Acid Properties. A compound that produces H + ions when dissolved in water. Examples!
Acids and Bases Acid A compound that produces H + ions when dissolved in water. Examples! Vinegar Acetic acid Lemon Juice Citric acid Sour Candy Malic acid (and others) Milk Lactic acid HCl(aq) Acid Properties
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
More informationACIDS & BASES PROPERTIES OF ACIDS ACIDS PROPERTIES OF ACIDS PROPERTIES OF ACIDS 11/1/2016
SC STANDARD COVERED ACIDS & BASES Standard PS-3.7 Classify various solutions as acids or bases according to their physical properties, chemical properties (including neutralization and reaction with metals),
More informationACID BASE EQUILIBRIUM
ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric
More informationINTRODUCTION TO ACIDS AND BASES
INTRODUCTION TO ACIDS AND BASES ALIGNED STANDARDS S.C. 912.P.8.11 Relate acidity and basicity to hydronium and hydroxide concentration and ph. S.C.912.N.1.2 Describe and explain what characterizes science
More informationAcids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.
Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others
More informationACIDS AND BASES CONTINUED
ACIDS AND BASES CONTINUED WHAT HAPPENS WHEN AN ACID DISSOLVED IN WATER? Water acts as a Brønsted Lowry base and abstracts a proton (H+) from the acid. As a result, the conjugate base of the acid and a
More informationCHAPTER 14: ACIDS AND BASES
CHAPTER 14: ACIDS AND BASES Arrhenius Acids and Bases There are a few definitions of acids and bases, some are somewhat narrow and others are much broader. Arrhenius Acids dissociate when dissolved in
More informationWorksheet 4.1 Conjugate Acid-Base Pairs
Worksheet 4.1 Conjugate AcidBase Pairs 1. List five properties of acids that are in your textbook. Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 4 Acid and Bases 2 Acids Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce
More informationDo Now April 24, 2017
Do Now April 24, 2017 Obj: Observe and describe neutralization reactions. Copy: Neutralization is when an acid and base react to product a salt and water. e.g. HCl + NaOH NaCl + H 2 O acid base salt water
More informationChapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
More informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationUnit 12: Acids and Bases REGENTS CHEMISTRY
REGENTS CHEMISTRY 1 Behavior of many acids and bases can be explained by the Arrhenius theory. Arrhenius acid and bases are electrolytes. (3.1uu) An electrolyte is a substance which, when dissolved in
More informationChem 30A. Ch 14. Acids and Bases
Chem 30A Ch 14. Acids and Bases Acids and Bases Acids and Bases Acids Sour taste Dissolve many metals Turn litmus paper red. Egs. Ace9c acid (vinegar), citric acid (lemons) Bases Bi>er taste, slippery
More informationAP 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 informationCHAPTER 19. Acids, Bases, and Salts Acid Base Theories
CHAPTER 19 Acids, Bases, and Salts 19.1 Acid Base Theories ACIDS tart or sour taste Electrolytes Strong acids are corrosive Acid Facts... indicators will change color Blue litmus paper turns pink react
More informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationA) 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 informationACIDS, 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 informationDuncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) 1. hydro- - HF 2. root of
More informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationAcids and Bases. Acids and Bases in. our Lives. Acids and Bases in our Lives. Acids and Bases in our Lives. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives We produce lactic acid in our muscles when we exercise. Acid from bacteria turns milks sour in the products of yogurt and cottage cheese. We have
More informationName 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 informationEquations. 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 informationAcid/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 informationChapter 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 informationPractice Examination #8B
Practice Examination #8B Name: Date: 1. Equal volumes of 0.5 M HCl and 0.5 M NaOH are mixed. The total volume of the resulting mixture is 2 liters. The ph of the resulting solution is 1. A. 1 B. 2 C. 7
More informationThe ph of aqueous salt solutions
The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More informationProblem Solving. ] Substitute this value into the equation for poh.
Skills Worksheet Problem Solving In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic sour milk, sore muscles acetic vinegar phosphoric soft drinks citric citrus fruits malic apples PROPERTIES OF ACIDS PROPERTIES OF BASES 1. Taste sour 1. Taste bitter 2. react
More information*KEY* * KEY * Mr. Dolgos Regents Chemistry. NOTE PACKET Unit 9: Acids, Bases, & Salts
*KEY* * KEY * Mr. Dolgos Regents Chemistry NOTE PACKET Unit 9: Acids, Bases, & Salts 1 *KEY* Unit 9: Acids, Bases, & Salts *KEY* Unit Vocabulary: Amphoteric Arrhenius acid Arrhenius base Bronsted-Lowry
More informationAcid 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 informationName: Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 13: Acids & Bases
Name: Regents Chemistry: Dr. Shanzer Practice Packet Chapter 13: Acids & Bases 1 Characteristics of Acids & Bases Objective: How can we recognize characteristics of acids and bases? How can we determine
More informationAcids and Bases. Feb 28 4:40 PM
Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to
More informationAcids and Bases Unit 11
Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid
More informationUnit #6, Chapter 8 Outline Acids, Bases and ph
Lesson Topics Covered 1&2 Review of Acids from Grade 11 Arrhenius acids and bases, definition chemical properties of acids & bases naming acids and bases Unit #6, Chapter 8 Outline Acids, Bases and ph
More informationSolubility Rules for Ionic Compounds Arrhenius Acid Base Theory
Chapter 4 Reactions in Aqueous Solutions Ionic compounds dissociate in water yielding electrolyte solutions. H 2 O NaCl(s) Na + (aq) + Cl - (aq) The ions are hydrated by water. Strong & Weak Electrolytes
More informationChapter 4 Reactions in Aqueous Solutions
Chapter 4 Reactions in Aqueous Solutions Ionic compounds dissociate in water yielding electrolyte solutions. H 2 O NaCl(s) Na + (aq) + Cl - (aq) The ions are hydrated by water. The Electrical Conductivity
More informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
More informationObj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH.
Do Now Date: April 13, 2015 Obj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH. HCl + KOH KCl(aq) + H 2 O(l) Practice
More informationAcids, Bases and Salts
(Hebden Unit 4 page 109 182) 182) We will cover the following topics: 1. Definition of Acids and Bases 2. Bronsted-Lowry Acids and Bases 2 1 Arrhenius Definition of Acids and Bases An acid is a substance
More informationUnit 9. Acids, Bases, & Salts Acid/Base Equilibrium
Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals
More informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 2 Acid and Bases 3 Acid and Bases 4 Acids 5 Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain
More informationChem 110 Acids, Bases, ph, and Redox
Chem 110 Acids, Bases, ph, and Redox 1. If 10.0 ml of 0.100 M HCl is titrated with 0.200 M NaOH, what volume of sodium hydroxide solution is required to neutralize the acid? HCl(aq) + NaOH(aq) NaCl(aq)
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 2 Acid and Bases 3 Acid and Bases 4 Acids 5 Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain
More informationChapter 14 Acids and Bases
Chapter 14 Acids and Bases General Properties of Acids 1. An acid tastes sour - acidus = Latin, sour; acetum= Latin, vinegar 2. An acid turns indicator dye litmus from blue to red. 3. An acid reacts with
More informationChapter 16 - Acids and Bases
Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) Practice: 1. hydro- - HF
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
More informationAcids and Bases. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationph 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 informationChapter 15 - Acids and Bases Fundamental Concepts
Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates
More informationChapter 11. Acids and Bases. Lecture Presentation. Karen C. Timberlake Pearson Education, Inc.
Lecture Presentation Chapter 11 Acids and Bases Chapter 11 Acids and Bases Clinical laboratory technicians prepare specimens for the detection of cancerous tumors and type blood samples for transfusions.
More informationUnit 9: Acids, Bases, & Salts
STUDENT VERSION Unit 9: Acids, Bases, & Salts Unit Vocabulary: Arrhenius acid Arrhenius base Bronsted-Lowry acid Bronsted-Lowry base Electrolyte hydronium ion hydroxide ion indicator (acid/base) neutralization
More informationREVIEW 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 informationStrong 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 informationAcids and Bases. Acids and Bases in our Lives. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationACID BASE TEST (2 nd half of class) Acid-base titration lab 2 nd half. Chapter 18 Acids and Bases Campbell Chemistry Name
Date In Class 3/31 Thurs. Equilibrium Test Homework (to be done that night, or before coming to the next class) Watch Acid Base Video 1. What are Acids and Bases? 4/1 Fri Video 1 discussion: Identifying
More informationACID-BASE EQUILIBRIA. Chapter 16
P a g e 1 Chapter 16 ACID-BASE EQUILIBRIA Nature of Acids and Bases Before we formally define acids and bases, let s examine their properties. Properties of Acids Sour taste Ability to dissolve many metals
More informationElectrolytes, Acids and Bases ) 3
Chapter 15 Acid (Latin acidus - sour): sour taste; turns plant dye litmus red; dissolves metals producing H 2 gas. Substances that are neither acids nor bases were called neutral substances. Electrolytes,
More informationCh 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs.
Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs. Ch 18 - Acids and Bases I CAN: 1) Compare properties of acids
More informationHomework Chapter 10 Chemistry 51 Los Angeles Mission College
10.71 Identify each of the following as an acid, base, or salt, and give its name: a. LiOH b. Ca(NO3)2 c. HBr d. Ba(OH)2 e. H2CO3 f. HClO2 10.72 Identify each of the following as an acid, base, or salt,
More informationACIDS 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 informationWhat are Acids &Bases?
Chemistry 481(01) Spring 2013 Instructor: Dr. Upali Siriwardane e-mail: upali@coes.latech.edu Office: CTH 311 Phone 257-4941 Office Hours: 8:00-9:00 a.m. & 11:00-12:00 a.m. M, W; 8:00-10:00 a.m. Tu, Th,
More informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
More informationAcids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
More informationLecture 20 Chapter 17, Sections 4-5 More weak acids and bases. Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases
Lecture 20 Chapter 17, Sections 4-5 More weak acids and bases Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases Acids and Bases Strong vs. Weak K a vs. K b ph = -log([h])
More informationIn the Brønsted-Lowry system, a Brønsted-Lowry acid is a species that donates H + and a Brønsted-Lowry base is a species that accepts H +.
16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 BrønstedLowry Acids and Bases In the BrønstedLowry system, a BrønstedLowry
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationPart 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 informationchem 101 Lec 6b Winter 10 2/13/10 page 1 of 1 Chem 101 lecture 6b
chem 101 Lec 6b Winter 10 2/13/10 page 1 of 1 Chem 101 lecture 6b Admin: Return tests last time: 0) Thermal analysis 1) liquid solutions 2) net ionic equations (review) 3) acids Today: 1) Bases 2) Lecture:
More informationCH19 Bronsted-Lowry Definitions
CH19 Bronsted-Lowry Definitions 1 BRONSTED-LOWRY DEFINITIONS [Acids] An acid is a substance that can donate H + ions HCl hydrochloric acid HNO 3 nitric acid HOAc acetic acid H 3 0 + hydronium ion NH +
More informationUnit 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 informationPractice Packet Unit 10: Acids and Bases
Name: Regents Chemistry: Practice Packet Unit 10: Acids and Bases 1 Vocabulary: For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something
More informationreversible reaction: R P and P R Acid dissociation is a reversible reaction. H 2 SO 4 2 H SO 4
Unit : Equilibrium / Acids and Bases reversible reaction: R P and P R Acid dissociation is a reversible reaction. H 2 SO 4 2 H + + SO 4 Rate at which equilibrium: R P = Rate at which P R -- looks like
More informationChemistry 281(01) Winter 2014
Chemistry 281(01) Winter 2014 CTH 277 10:00-11:15 am Instructor: Dr. Upali Siriwardane E-mail: upali@latech.edu Office: 311 Carson Taylor Hall ; Phone: 318-257-4941; Office Hours: MTW 8:00 am - 10:00 am;
More informationName Class Date. volume of solution molarity of solution amount of solute in moles
Skills Worksheet Problem Solving Titrations Chemists have many methods for determining the quantity of a substance present in a solution or other mixture. One common method is titration, in which a solution
More informationCHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM
CHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM 1. The ph of a 0.10 M solution of NH3 containing 0.10 M NH 4 Cl is 9.20. What is the [H3O + ]? a) 1.6 x 10-5 b) 1.0 x 10-1 c) 6.3 x 10-10 d) 1.7 x 10-10 e) 2.0 x
More informationUnit 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 informationAcids 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 informationACID, BASE, AND ph STUDYGUIDE
ACID, BASE, AND ph STUDYGUIDE Naming Acids: (back of PT) Binary acid (Only 2 elements): Hydro- ic acid Oxyacid (More than 2 elements): Name of anion with new ending If anion ends with ate If anion ends
More information