SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
|
|
- Shauna Thomas
- 5 years ago
- Views:
Transcription
1 SCHOOL YEAR NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute whose water solution conducts electricity is called a(n) a. nonconductor. b. electrolyte. c. nonelectrolyte. d. aqueous solution. 2. Which solution has the highest boiling point? a m glucose in water b m potassium iodide in water c m glucose in water d m calcium chloride in water 3. When an ionic solid dissolves in water, which of the following does not occur? a. The compound dissociates. b. Hydration occurs. c. The compound ionizes. d. Polar ends of water molecules approach the ions, releasing energy. 4. Colligative properties depend on the a. number of solute particles present. b. size of solute particles present. c. mass of solute particles present. d. charge on solute particles present. 5. Nonvolatile solutes a. depress both the freezing point and the boiling point. b. elevate both the freezing point and the boiling point. c. depress the freezing point and elevate the boiling point. d. elevate the freezing point and depress the boiling point.
2 Use the table to answer the following questions. Solubility Rules for Some Common Ionic Compounds Compounds containing these ions are soluble in water: Alkali metals (Group 1), except LiF Ammonium, NH + Bromides, Br, except those of Ag +, Pb 2+, and Hg Chlorides, Cl, except those of Ag +, Pb 2+, and Hg Nitrates, NO Sulfates, SO, except those of Ca 2+, Sr 2+, Ba 2+, Pb 2+, and Hg Compounds containing these ions are insoluble in water: Carbonates, CO Hydroxides, OH, except those of Group 1 Oxides, O 2 Phosphates, PO, except those of Group 1, Ca 2+, Sr 2+, and Ba 2+ (which form hydroxides), except those of Group 1 and NH Sulfides, S 2, except those of Group 1, Mg 2+, Ca 2+, Ba 2+, and NH 6. Using the table above, which of the following compounds is soluble in water? a. PbBr 2 b. MgCl 2 c. BaSO 4 d. CaCO 3 7. Using the table above, which of the following compounds is insoluble in water? a. (NH 4 ) 2 S b. Na 2 O c. LiOH d. Al 2 O 3 Choose the best answer from the options that follow each question. 8. Compared with the freezing-point depression of a 0.01 m C 6 H 12 O 6 solution, the freezing-point depression of a 0.01 m NaCl solution is a. almost half. b. exactly the same. c. exactly twice as great. d. almost twice as great. 9. Which of the following is an ionic compound that dissociates in water? a. NaCl b. C1 2 c. CCl 4 d. C 6 H 6
3 10. Which of these is a spectator ion in the following equation? a. S b. Cu 2+ c. Zn 2+ d. None of the above Cu 2+ (aq) Zn 2 (aq) + 2S (aq) CuS(s) + ZnS(s) 11. What happens when a weak electrolyte dissolves in water? a. The boiling point decreases. b. The solution does not conduct electricity. c. Few ions form. d. 100% of the molecules ionize. 12. What is the freezing point of a 1.5 m solution of sucrose in water? (Kf = 1.86C /m) a. 2.8 C b. 1.2 C c C d C 13. What concentration of ethylene glycol is needed to raise the boiling point of water to 105 C? (K b C /m) a. 1.5 m b. 2.5 m c. 9.8 m d. 205 m 14. Compared with a 1.0 m solution of C 12 H 22 O 11, the vapor pressure of a 1.0 m solution of C 5 H 12 O 6 a. is exactly double. b. is the same. c. is exactly half. d. cannot be determined. 15. How many moles of Cl ions are produced when 0.5 mol of NaCl is dissolved in water? a. 0.5 b. 1.0 c. 1.5 d What is the net ionic equation for the precipitation reaction between BaCl 2 and Na 2 SO 4? a. Ba 2 (aq) + SO (aq) BaSO 4 (s) b. Na + (aq) + Cl(aq) NaCl(s) c. Ba 2+ (aq) + 2Cl (aq) + 2Na + (aq) + SO (aq) BaSO 4 (s) + 2Cl (aq) + 2Na + (aq) d. BaCl 2 (aq) + Na 2 SO 4 (aq) BaSO 4 (s) + 2NaCl(aq) 17. Which solute will have the greatest effect on the boiling point of water? a. C 6 H 12 O 6 b. NaCl c. HF d. CH 3 COOH
4 18. What is the approximate freezing-point depression of a 0.10 m aqueous CaCl 2 solution? (K f = 1.86C /m) a C b C c C d C 19. The external pressure that must be applied to stop osmosis is called a. atmospheric pressure. b. vapor pressure. c. osmotic pressure. d. None of the above 20. Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes a. are volatile. b. have higher boiling points. c. produce fewer moles of solute particles per mole of solvent. d. produce more moles of solute particles per mole of solvent. 21. A 12 m acetic acid solution is a. concentrated and a weak electrolyte. b. dilute and a weak electrolyte. c. concentrated and a strong electrolyte. d. dilute and a strong electrolyte. 22. A 2 m solution contains a. 2 mol of solute dissolved in 1 L of solvent. b. 1 mol of solute dissolved in 2 L of solvent. c. 2 mol of solute dissolved in 1 mol of solvent. d. 2 mol of solute dissolved in 1 kg of solvent. 23. What is the boiling-point elevation of a solution made from 15.0 g of a nonelectrolyte solute and g of water? The molar mass of the solute is 50.0 g and K b = 0.51 C/m. a C b C c C d C 24. The hydronium ion forms when hydrogen ions a. dissociate. b. ionize. c. combine with HCl. d. combine with H 2 O. 25. What is the expected boiling point of a solution of 128 g KCl (a strong electrolyte) dissolved in 1.3 kg of water. The molar mass of KCl is g and K b = 0.51C /m. a C b C c C d C
5 TEST B PART I Choose the best answer from the options that follow each question. 1. A colligative property is one that depends on a. the number of solute particles but not their identity. b. the identity of solute particles but not their number. c. both the number and the identity of solute particles. d. neither the number nor the identity of solute particles. 2. Which of the following is not a colligative property? a. boiling-point elevation b. lowering vapor pressure c. freezing-point depression d. conducting electricity 3. How many moles of ions are produced when 2 mol of Na 2 CO 3 dissociate? a. 2 b. 3 c. 6 d If the following equation were written as a net ionic equation, which ion(s) is (are) the spectator ion(s)? Zn(s) + CuSO 4 (aq) Cu(s)ZnSO 4 (aq) a. Cu 2+ (aq) b. Zn 2+ (aq) c. SO (aq) d. All of the above 5. To determine the molar mass of a solute by using colligative properties, you must know the a. volume of the solution. b. mass of the solute. c. temperature of the solution. d. volume of the solute. 6. What is the net ionic equation for the precipitation reaction between silver nitrate solution and sodium sulfide solution? a. 2Ag + (aq) + 2NO (aq) + 2Na + (aq) + S 2 (aq) Ag 2 S(s) + 2Na + (aq) b. c. d. 2Ag + (aq) +S 2 (aq) Ag 2 S(s) 2Ag + (aq) + 2NO (aq) + 2Na + (aq) + S 2 (aq) Ag 2 S(s) + 2NaNO 3 (s) + S 2 (aq) 2Ag (aq) + S 2+ (aq) Ag 2 S(s) 7. Which ions are not spectator ions for the precipitation reaction that occurs when solutions of Zn(NO 3 ) 2 and Na 3 PO 4 are mixed? a. Zn 2+ (aq) and NO (aq) b. Na + (aq) and Zn 2+ (aq) c. Zn 2+ (aq) and PO (aq)
6 d. Na + (aq) and NO (aq) 8. When nonvolatile, nonionic solutes are added to water, they a. depress freezing point and elevate boiling point. b. elevate freezing point and depress boiling point. c. depress both freezing and boiling points. d. elevate both freezing and boiling points. PART II Write the correct term (or terms) in the space provided. 9. When a solid is formed from the combination of two solutions of ionic compounds, it is called. 10. allow the movement of some particles while blocking the movement of others. 11. Any substance whose water solution conducts electricity is a(n). 12. An ion that does not take part in a chemical reaction is called a(n). 13. The number of moles of ions produced by the dissociation of 1 mol of MgCl 2 is. 14. is the external pressure that must be applied to stop osmosis. 15. The symbol for the hydronium ion is. 16. The ions Ca 2+ (aq) and NO (aq) are produced by the dissociation of the compound whose formula is. 17. The vapor pressure of pure water is than the vapor pressure for an aqueous solution. 18. The boiling point for a 1 M solution of glucose (a nonelectrolyte) will be than for a 1 M solution of NaCl (a strong electrolyte). 19. The right-hand side of the equation for the dissolving of K 2 S is. PART III Write the answers to the following questions. 20. Explain how ionization and dissociation differ. 21. Distinguish between the dissolution of a strong electrolyte and that of a weak electrolyte. 22. Why is the hydronium ion used to represent the hydrogen ion in a solution? 23. Explain why salt is frequently poured on icy roads in the winter. PART IV For the following questions, use the guidelines below to determine which of the following combinations of solutions will produce a precipitate. If no precipitate will form, write none. If a precipitate will form, write the net ionic equation for the reaction.
7 General Solubility Guidelines 1. Most sodium, potassium, and ammonium compounds are soluble in water. 2. Most nitrates, acetates, and chlorates are soluble. 3. Most chlorides are soluble except those of silver, mercury(ii), and lead. Lead(II) chloride is soluble in hot water. 4. Most sulfates are soluble except those of calcium, barium, strontium, and lead. 5. Most carbonates, phosphates, and silicates are insoluble except those of sodium, potassium, and ammonium. 6. Most sulfides are insoluble except those of calcium, strontium, sodium, potassium, and ammonium. 24. KCl and Ca(NO 3 ) Na 2 SO 4 and BaCl (NH 4 ) 2 S and Cd(NO 3 ) NH 4 Cl and Na 2 SO Ca(NO 3 ) 2 and CuCl A solution with 3.11 g of a nonelectrolyte solute in 38 g of water (K b = 0.51 C/m) has a boiling point elevated by 1.00 C. What is the molar mass of the solute? 30. The boiling point of a solvent is elevated by 2.4 C when the solute concentration is 3.1 m. What is K b? 31. What is the freezing-point depression of a solution that contains mol of a nonelectrolyte solute in 5.02 kg of water? (K f 1.86 C/m) 32. The freezing point of a solvent is lowered by 2.89 C when the solute concentration is 1.03 m. What is K f? 33. How many grams of a nonelectrolyte solute that has a molar mass of 41.9 g/mol must be added to g of water to raise the boiling point 0.84 C? (K b 0.51C /m) 34. What is the boiling-point elevation of water for a solution that contains 125 g of barium nitrate, Ba(NO 3 ) 2, dissolved in 1.00 kg of water? The molar mass of the solute is g/mol. (K b = 0.51 C/m)
8 SCHOOL YEAR NAME: CH- 14 ACIDS AND BASESE SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. Which of the properties listed below is not characteristic of an acid? a. a sour taste b. a slippery feel c. the ability to conduct an electric current d. reactivity with metals 2. Which is an example of a weak acid? a. HCl b. H 2 SO 4 c. H 3 PO 4 d. HNO 3 3. Acetic acid is found in a. vinegar. b. the stomach. c. antacids. d. oranges. 4. A characteristic of an Arrhenius base is that it a. is an electrolyte. b. tastes bitter. c. dissociates to form OH ions. d. All of the above 5. Which of the following is a Brønsted-Lowry base? a. HCl b. HCO c. H 3 O + d. H 3 PO 4 6. In the reaction represented by the equation H 2 C 2 O 4 (aq) + CH 3 NH 2 (aq) HC 2 O 4 (aq) + CH 3 NH (aq), which of these is a conjugate acid-base pair? a. H 2 C 2 O 4 (aq) and CH 3 NH 2 (aq) b. H 2 C 2 O 4 (aq) and CH 3 NH (aq)
9 c. CH 3 NH 2 (aq) and CH 3 NH (aq) d. HC 2 O (aq) and CH 3 NH (aq) 7. What is the correct formula for hydrosulfuric acid? a. H 2 SO 4 b. H 2 S c. H 2 SO 3 d. SO 8. What is the correct acid name for an aqueous solution of HClO 4? a. hypochlorous acid b. chlorous acid c. chloric acid d. perchloric acid 9. A substance that increases the concentration of OH ions in an aqueous solution is known as a(n) a. Arrhenius acid. b. Arrhenius base. c. Lewis acid. d. Lewis base. 10. An Arrhenius acid in an aqueous solution a. attracts negatively charged anions. b. attracts positively charged cations. c. gives up one or more of its hydrogen ions to water molecules. d. forms ionic bonds with water molecules. 11. Which of the following is an indication of acid strength? a. the number of hydrogen atoms in the formula of the acid b. how strongly an aqueous solution of the acid conducts an electric current c. how quickly the acid dissolves in water d. the number of total atoms in one molecule of the acid 12. Which of the following is an organic acid? a. CH 3 COOH b. H 2 SO 4 c. HI d. HClO The neutralization of any strong acid and strong base produces mostly a. H 2 O molecules. b. H 3 O + and OH ions. c. H 3 O + ions. d. OH ions. 14. A strong base in an aqueous solution a. is a weak electrolyte. b. produces many H + ions. c. will not dissolve. d. completely dissociates into ions.
10 15. In a Brønsted-Lowry acid-base reaction, what are transferred from one reactant to another? a. electrons b. water molecules c. protons d. OH ions 16. How many protons per molecule can a monoprotic acid donate? a. one b. two c. three d. zero 17. How many stages of ionization does phosphoric acid go through? a. one b. two c. three d. four 18. Which substance is a Lewis acid in the reaction shown by the equation below? BF 3 (aq) + F (aq) BF 4 (aq) a. BF 3 b. F c. BF d. None of the above 19. What is the conjugate acid of water? a. OH b. H 3 O + c. H 2 O 2 d. HOH 20. HCl is a strong acid. When it combines with water, the conjugate of HCl will be a a. weak base. b. weak acid. c. strong base. d. strong acid. 21. Which is the stronger base in the reaction represented by the following equation? CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO (aq) a. CH 3 COOH b. CH 3 COO c. H 3 O + d. H 2 O 22. Consider the reaction represented by the equation below. HClO 4 (aq) + H 2 O(l) H 3 O + (aq) + ClO (aq) Which substances are present in the greatest concentrations? a. HClO 4 and H 2 O b. HClO 4 and ClO c. H 3 O + and ClO
11 d. H 2 O and H 3 O Consider the two equations below. H 2 SO 4 (aq) + H 2 O(l) H 3 O + (aq) + HSO (aq) NH 3 (g) + H 2 O(l) NH (aq) + OH (aq) They illustrate that water is a. an acid in both reactions. b. a base in both reactions. c. amphoteric. d. a weak electrolyte. 24. What is the correct net ionic equation for the neutralization reaction between the substances below? HNO 3 (aq) + KOH(aq) a. NO (aq) + K + (aq) KNO 3 (aq) b. H 3 O + (aq) + OH (aq) 2H 2 O(l) c. H 3 O + (aq) + NO (aq) + K + (aq) + OH (aq) NO (aq) + K + (aq) + 2H 2 O(l) d. HNO 3 (aq) + KOH(aq) KNO 3 (aq) + H 2 O(l) 25. Sulfur trioxide gas dissolves in atmospheric water. The product of the reaction, which falls to the ground as a component of acid rain or snow, is a. H 2 SO 4 (aq). b. HS(aq). c. H 3 O + (aq). d. SO (aq).
12 TEST B PART I Choose the best answer from the options that follow each question. 1. Which of the following is an oxyacid? a. HCl b. H 2 O c. H 2 S d. H 2 SO 4 2. Which acid is produced in the stomach? a. HNO 3 b. CH 3 COOH c. H 2 SO 4 d. HCl 3. Which of the following is a strong base? a. NH3 b. aniline c. NaOH d. acetate ion 4. In the reaction represented by the equation HF(aq) + H 2 O(l) H 3 O + (aq) + F (aq), a conjugate acid-base pair is a. F and H 2 O. b. H 3 O + and HF. c. HF and F. d. HF and H 2 O. 5. If H 2 O in the reaction represented by the equation H 2 O + C 2 H 3 COOH H 3 O + + C 2 H 3 COO is considered to be a weaker base, then H 3 O is a a. stronger acid. b. stronger base. c. weaker acid. d. weaker base. 6. Proton-transfer reactions favor production of the a. stronger acid and stronger base. b. weaker acid and weaker base. c. stronger acid and weaker base. d. weaker acid and stronger base. 7. Aqueous solutions of most bases contain a. hydroxide ions and cations. b. hydroxide ions and anions. c. hydrogen ions and anions. d. hydrogen ions and cations. 8. Acid strength increases with a. increasing polarity and increasing bond strength. b. increasing polarity and decreasing bond strength. c. decreasing polarity and increasing bond strength.
13 d. decreasing polarity and decreasing bond strength. PART II Write the correct term (or terms) in the space provided. 9. A substance that ionizes almost completely in aqueous solutions, producing H 3 O + ions, is a(n) acid. 10. An acid that contains hydrogen and only one other element is called a(n) acid. 11. The species that forms when an acid has given up a proton is called the acid s. 12. An acid that can donate two protons per molecule is called a(n) acid. 13. Bases are said to be neutralized when they react with to yield and a(n). 14. Any species that can react as either an acid or a base is described as. 15. Barium carbonate will react with hydrochloric acid to produce,, and. PART III Write the name of each of the following acids in the space provided. 16. HNO HCl 18. H 2 CO H 2 SO HI 21. HBrO Write the formula for each of the following acids in the space provided. 22. hydrosulfuric acid 23. nitric acid 24. phosphorous acid 25. perchloric acid Refer to the equation below to answer the following questions. HCl(g) + NH 3 (l) NH (aq) + Cl (aq)
14 26. List the conjugate acid-base pairs. 27. Identify each reactant and product as acidic or basic. Refer to the equation below to answer the following questions. H 2 O(l) + NH 3 (g) NH (aq) + OH (aq) 28. List the conjugate acid-base pairs. 29. Identify each reactant and product as a proton donor or a proton acceptor. Refer to the following statement to answer the following questions: Dilute HCl(aq) and NaOH(aq) are mixed in chemically equivalent quantities 30. Write the chemical equation for the reaction. 31. Write the overall ionic equation for the reaction. 32. Write the net ionic equation. Use the following three acids to answer the following questions. 33. Give the formulas for these three acids. iodic acid hypoiodous acid periodic acid 34. List the acids in order of increasing acid strength. PART IV Write the answers to the following questions in the space provided. 35. Explain the difference between strong acids and weak acids. 36. Explain how the production of sulfur trioxide, SO 3, in industrial processes can result in acid rain. Write an equation for the reaction. 37. List five properties of aqueous acids. 38. Write the balanced equations that describe the three-stage ionization of phosphoric acid in a dilute aqueous
Chapter Test B. Chapter: Acids and Bases
Assessment Chapter Test B Chapter: Acids and Bases PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the
More informationIons in Aqueous Solutions and Colligative Properties
Ions in Aqueous Solutions and Colligative Properties Section 1 Compounds in Aqueous Solutions Dissociation When compound made from ions dissolves in water, ions separate Dissociation à separation of ions
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationReaction Classes. Precipitation Reactions
Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
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 informationChapter 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 informationO + (aq) In this reaction, the water molecule is a Brønsted-Lowry base. It accepts a proton from HF to form H 3
AcidBase Reactions Key Terms conjugate base conjugate acid amphoteric neutralization salt In the previous sections, you learned about three acidbase theories: Arrhenius, BrønstedLowry, and Lewis. The BrønstedLowry
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationIons in Aqueous Solutions and Colligative Properties
CHAPTER 13 REVIEW Ions in Aqueous Solutions and Colligative Properties SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Use the guidelines in Table 1 on page 437 of the text
More information15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.
15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More informationChapter 6. Acids, Bases, and Acid-Base Reactions
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin
Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Acids and Bases Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water.
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
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 informationAnnouncements. There are 3-classes of chemical reactions that occur in aqueous solution.
Announcements Exam 1 Results: Mean: 71% Range: 39.5%-93.5% Median: 72% Other Bio-LS Class Mean 72% Please read Chapter 4 and complete problems. Please see me for help. There are 3-classes of chemical reactions
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
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 informationReactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
More informationH H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent.
Role of Water Role of Water Chemical Reactions in Aqueous Solution Role of H 2 O(l) as solvent The polar nature of water molecule Two key features: 1. The distribution of bonding electrons O H covalent
More information9/24/09 Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter
Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter 4.1-4.4 KEY VOCABULARY: 1. Ionic compound a compound composed of cations (+) and anions (-). Many ionic compounds dissociate
More informationPrinciples of Reactivity: The Chemistry of Acids and Bases. Acids, Bases and Arrhenius
Principles of Reactivity: The Chemistry of Acids and Bases **a lot of calculations in this chapter will be done on the chalkboard Do not rely on these notes for all the material** Acids, Bases and Arrhenius
More informationChemical reactions describe processes involving chemical change
1.1 Chemical Reactions 1.2 Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into
More informationCHEMICAL REACTIONS. There are three ways we write chemical equations. 1. Molecular Equations 2. Full Ionic Equations 3. Net Ionic Equations
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2 Unit 2 Chemical Reactions The unit 2 exam will cover material from multiple chapters. You are responsible for the following from your text on exam
More informationSolution Stoichiometry
Chapter 8 Solution Stoichiometry Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the
More informationReactions 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 informationLecture 4 :Aqueous Solutions
LOGO Lecture 4 :Aqueous Solutions International University of Sarajevo Chemistry - SPRING 2014 Course lecturer : Jasmin Šutković 11 th March 2014 Contents International University of Sarajevo 1. Aqueous
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationMixtures. Chapters 12/13: Solutions and Colligative Properties. Types of Solutions. Suspensions. The Tyndall Effect: Colloid
Mixtures Chapters 12/13: Solutions and Colligative Properties Solution - a homogeneous mixture of two or more substances in a single phase Soluble - capable of being dissolved Solutions - 2 Parts Solvent
More informationChapter 4. Reactions In Aqueous Solution
Chapter 4 Reactions In Aqueous Solution I) General Properties of Aqueous Solutions Homogeneous mixture on a molecular level - prop. same throughout - separable by physical means - variable composition
More informationI. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*
Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in
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 informationCHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS
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 informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationSolubility Rules. Electrolytes, Weak and Strong. Examples. Another Example:
Electrolytes, Weak and Strong Electrolytes are compounds that ionize in water to produce aqueous solutions that conduct an electric current. Nonelectrolytes are substances that do not ionize, remain as
More informationChapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does
More informationChemistry deals with matter and its changes CHEMICAL REACTIONS
Chemistry deals with matter and its changes CHEMICAL REACTIONS CHEMICAL EQUATIONS N 2 + 3 H 2 2 NH 3 2 N 6 H 2 N 6 H reactants products balanced means equal numbers of atoms of each element on each side
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationChemistry 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 informationReactions in aqueous solutions Precipitation Reactions
Reactions in aqueous solutions Precipitation Reactions Aqueous solutions Chemical reactions that occur in water are responsible for creation of cenotes. When carbon dioxide, CO2, dissolves in water, the
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationChapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in
More informationChapter Four: Reactions in Aqueous Solution
Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products
More informationAcids Bases and Salts Acid
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
More informationChapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)
Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationPractice questions for Chapter 4
Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More information9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS
9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS Work directly from Zumdahl (Chapter 4). Work through exercises as required, then summarise the essentials of the section when complete. To understand the
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More information7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
More information9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions
Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationChemistry 1A. Chapter 5
Chemistry 1A Chapter 5 Water, H 2 O Water Attractions Liquid Water Solutions A solution, also called a homogeneous mixture, is a mixture whose particles are so evenly distributed that the relative concentrations
More informationChapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationPart One: Ions in Aqueous Solution
A. Electrolytes and Non-electrolytes. CHAPTER FOUR: CHEMICAL REACTIONS Part One: Ions in Aqueous Solution 1. Pure water does not conduct electric current appreciably. It is the ions dissolved in the water
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 informationChapter 4 Outline. Electrolytic Properties
+4.1 - General Properties of Aqueous Solutions Solution = a homogeneous mixture of two or more substances Solvent = substance present in greatest quantity Solute = the other substance(s) present in a solution
More informationSection 4: Aqueous Reactions
Section 4: Aqueous Reactions 1. Solution composition 2. Electrolytes and nonelectrolytes 3. Acids, bases, and salts 4. Neutralization ti reactions 5. Precipitation reactions 6. Oxidation/reduction reactions
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 informationSI session Grue 207A
Chem 105 Wednesday 21 Sept 2011 1. Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30
More informationThe Major Classes of Chemical Reactions
Chapter 4 The Major Classes of Chemical Reactions 5.1 Properties of compounds in Aqueous Solution 5.2 Precipitation Reaction 5.3 Acids and Bases 5.4 Reactions of Acid and Bases 5.5 Gas-forming Reactions
More informationChapter 4. Reactions in Aqueous Solutions. Aqueous solutions and their chemistry. Various types of reactions.
Chapter 4 Reactions in Aqueous Solutions Dr. A. AlSaadi 1 Preview Aqueous solutions and their chemistry. Various types of reactions. Precipitation reactions. Acidbase reactions. Oxidationreduction reactions.
More informationChapter Menu Chapter Menu
Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationChapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions
Chapter 4 in Solution 4.1 General Properties of Solutions Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other
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 informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More informationChapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
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 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 informationIons in Solution. Solvent and Solute
Adapted from Peer-led Team Learning Begin at the beginning and go on till you come to the end: then stop." Early ideas of atoms and compounds, developed primarily through the reactions of solids and gases,
More informationConcentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.
CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION CONCENTRATION Solute Solvent Concentration Units mass NaCl / unit volume of solution g L -1 (M, molarity) concentration in moles per litre of solution c NaCl c B
More informationElectrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.
Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look
More informationA reaction in which a solid forms is called a precipitation reaction. Solid = precipitate
Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Chapter 8 Prep Test Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. General Solubility Guidelines 1. Most sodium, potassium, and ammonium compounds
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 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 informationREACTIONS IN AQUEOUS SOLUTIONS
REACTIONS IN AQUEOUS SOLUTIONS [ MH5; Ch. 4] Most reactions in water involve hydrated, charged species [ (aq) ]. Any substance which is ionic in the solid state will form ions in solution. EXAMPLE: KCR
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationName%% %Period%% % Precipitation+Reaction+Practice+
Name%% %Period%% % Precipitation+Reaction+Practice+ 1.%Write%a%balanced%equation%for%the%following%precipitation%reactions,%circle%the%precipitate%that%is% formed:% a) K 3 PO 4 %+%3%Sr(NO 3 ) 2 %% % %
More informationAP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry
HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance
More informationChapter 4: Reactions in Aqueous Solutions
Chapter 4: Reactions in Aqueous Solutions Water 60 % of our bodies heat modulator solvent for reactions covers 70% of Earth Chapter 4 3 types of reactions that occur in H 2 O 1. precipitation 2. acid-base
More information