1 Chemical Foundations 2 Atomic Structure And Periodicity 3 Bonding: General Concepts 4 Molecular Structure And Orbitals 5 Stoichiometry 6 Types Of Chemical Reactions And Solution Stoichiometry 7 Chemical Energy 8 Gases 9 Liquids And Solids 10 Properties Of Solutions 11 Chemical Kinetics 12 Chemical Equilibrium 13 Acids And Bases 14 Acid- Base Equilibria 15 Solubility And Complex Lon Equilibria 16 Spontaneity, Entropy, And Free Energy 17 Electrochemistry 18 The Nucleus: A Chemist's View 19 The Representative Elements 20 Transition Metals And Coordination Chemistry 21 Organic And Biological Molecules Chapter6: Types Of Chemical Reactions And Solution Stoichiometry
Chapter Questions Section: Chapter Questions
Problem 1RQ: The (aq) designation listed after a solute indicates the process of hydration. Using KBr(aq) and... Problem 2RQ: Characterize strong electrolytes versus weak electrolytes versus nonelectrolytes. Give examples of... Problem 3RQ: Distinguish between the terms slightly soluble and weak. electrolyte. Problem 4RQ Problem 5RQ Problem 6RQ: When the following beakers are mixed, draw a molecular-level representation of the product mixture... Problem 7RQ Problem 8RQ: What is an acid-base reaction? Strong bases are soluble ionic compounds that contain the hydroxide... Problem 9RQ Problem 1ALQ: Assume you have a highly magnified view of a solution of HCl that allows you to see the HCl. Draw... Problem 2ALQ Problem 3ALQ: You have a sugar solution (solution A) with concentration x. You pour one-fourth of this solution... Problem 4ALQ Problem 5ALQ Problem 6ALQ Problem 7ALQ: Consider separate aqueous solutions of HCl and H2SO4 with the same molar concentrations. You wish to... Problem 8ALQ Problem 9ALQ Problem 10ALQ: The exposed electrodes of a light bulb are placed in a solution of H2SO4 in an electrical circuit... Problem 13Q: Differentiate between what happens when the following are added to water. a. polar solute versus... Problem 14Q: Consider the following electrostatic potential diagrams for some covalent compounds. Which of the... Problem 15Q Problem 16Q: A typical solution used in general chemistry laboratories is 3.0 M HCl. Describe, in detail, the... Problem 17Q Problem 18Q: A student wants to prepare 1.00 L of a 1.00-M solution of NaOH (molar mass = 40.00 g/mol). If solid... Problem 19Q: List the formulas of three soluble bromide salts and three insoluble bromide salts. Do the same... Problem 20Q: When 1.0 mole of solid lead nitrate is added to 2.0 moles of aqueous potassium iodide, a yellow... Problem 21Q: What is an acid and what is a base? An acid-base reaction is sometimes called a proton-transfer... Problem 22Q: A student had 1.00 L of a 1.00-M acid solution. Much to the surprise of the student, it took 2.00 L... Problem 23Q Problem 24Q Problem 25E Problem 26E: Match each name below with the following microscopic pictures of that compound in aqueous solution.... Problem 27E Problem 28E: Commercial cold packs and hot packs are available for treating athletic injuries. Both types contain... Problem 29E: Calculate the molarity of each of these solutions. a. A 5.623-g sample of NaHCO3 is dissolved in... Problem 30E: A solution of ethanol (C2H5OH) in water is prepared by dissolving 75.0 mL of ethanol (density = 0.79... Problem 31E: Calculate the concentration of all ions present in each of the following solutions of strong... Problem 32E Problem 33E Problem 34E Problem 35E Problem 36E Problem 37E Problem 38E Problem 39E: A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of... Problem 40E: A solution was prepared by mixing 50.00 mL of 0.100 M HNO3 and 100.00 mL of 0.200 M HNO3. Calculate... Problem 41E: Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of... Problem 42E: Suppose 50.0 mL of 0.250 M CoCl2 solution is added to 25.0 mL of 0.350 M NiCl2 solution. Calculate... Problem 43E Problem 44E: A stock solution containing Mn2+ ions was prepaned by dissolving 1.584 g pure manganese metal in... Problem 45E: On the basis of the general solubility rules given in Table 6-1, predict which of the following... Problem 46E: On the basis of the general solubility rules given in Table 6-1, predict which of the following... Problem 47E: When the following solutions are mixed together, what precipitate (if any) will form? a. FeSO4(aq) +... Problem 48E: When the following solutions are mixed together, what precipitate (if any) will form? a.... Problem 49E: For the reactions in Exercise 47, write the balanced formula equation, complete ionic equation, and... Problem 50E: For the reactions in Exercise 48, write the balanced formula equation, complete ionic equation, and... Problem 51E: Write the balanced formula and net ionic equation for the reaction that occurs when the contents of... Problem 52E: Give an example how each of the following insoluble ionic compounds could be produced using a... Problem 53E: Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the... Problem 54E: Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the... Problem 55E Problem 56E Problem 57E: What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100-M... Problem 58E: What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 150.0 mL of... Problem 59E: What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to... Problem 60E: What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride... Problem 61E: What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M... Problem 62E: What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate... Problem 63E: A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous... Problem 65E: A 1.42-g sample of a pure compound, with formula M2SO4, was dissolved in water and treated with an... Problem 66E: You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into... Problem 67E: Write the balanced formula, complete ionic, and net ionic equations for each of the following... Problem 68E: Write the balanced formula, complete ionic, and net ionic equations for each of the following... Problem 69E: Write the balanced formula equation for the acid-base reactions that occur when the following are... Problem 70E Problem 71E: What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH? a.... Problem 72E Problem 73E: Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is... Problem 74E Problem 75E: A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for... Problem 76E: A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with 0.5062... Problem 77E: What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric... Problem 78E: A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M... Problem 79E: A student titrates an unknown amount of potassium hydrogen phthalate (KHC8H4O4, often abbreviated... Problem 80E: The concentration of a certain sodium hydroxide solution was determined by using the solution to... Problem 81E: Assign oxidation states for all atoms in each of the following compounds. a. KMnO4 b. NiO2 c.... Problem 83E: Assign the oxidation state for nitrogen in each of the following. a. Li3N b. NH3 c. N2H4 d. NO e.N2O... Problem 84E Problem 85E: Specify which of the following are oxidationreduction reactions, and identify the oxidizing agent,... Problem 86E: Specify which of the following equations represent oxidationreduction reactions, and indicate the... Problem 87E: Consider the reaction between sodium metal and fluorine (F2) gas to form sodium fluoride. Using... Problem 88E: Consider the reaction between oxygen (O2) gas and magnesium metal to form magnesium oxide. Using... Problem 89E: Balance each of the following oxidationreduction reactions by using the oxidation states method. a.... Problem 90E: Balance each of the following oxidationreduction reactions by nsing the oxidation states method. a.... Problem 91AE Problem 92AE Problem 93AE Problem 94AE Problem 95AE Problem 96AE: Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture... Problem 97AE: A 1.00-g sample of an alkaline earth metal chloride is treated with excess silver nitrate. All of... Problem 98AE: A mixture contains only NaCl and Al2(SO4)3. A 1.45-g sample of the mixture is dissolved in water and... Problem 99AE: The thallium (present as Tl2SO4) in a 9.486-g pesticide sample was precipitated as thallium(I)... Problem 100AE Problem 101AE: A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then... Problem 102AE Problem 103AE: Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium... Problem 104AE: When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are... Problem 105AE: A 2.20-g sample of an unknown acid (empirical formula = C3H4O3) is dissolved in 1.0 L of water. A... Problem 106AE: Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only... Problem 107AE: Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g... Problem 108AE Problem 109AE Problem 110AE: Many oxidationreduction reactions can be balanced by inspection. Try to balance the following... Problem 111AE Problem 112CWP: Calculate the concentration of all ions present when 0.160 g of MgCl2 is dissolved in 100.0 mL of... Problem 113CWP: A solution is prepared by dissolving 0.6706 g oxalic acid (H2C2O4) in enough water to make 100.0 mL... Problem 114CWP: For the following chemical reactions, determine the precipitate produced when the two reactants... Problem 115CWP: What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a... Problem 116CWP Problem 117CWP: A 450.0-mL sample of a 0.257-M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium... Problem 118CWP: The zinc in a 1.343-g sample of a foot powder was precipitated as ZnNH4PO4. Strong heating of the... Problem 119CWP Problem 120CWP: When organic compounds containing sulfur are burned, sulfurdioxide is produced. The amount of SO2... Problem 121CWP Problem 122CP Problem 123CP: The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental... Problem 124CP Problem 125CP Problem 126CP Problem 127CP: Consider the reaction of 19.0 g of zinc with excess silver nitrite to produce silver metal and zinc... Problem 128CP: A mixture contains only sodium chloride and potassium chloride. A 0.1586-g sample of the mixture was... Problem 129CP Problem 130CP Problem 131CP Problem 132CP: Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by... Problem 133CP Problem 134CP Problem 135CP: What volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4?... Problem 136CP: A 10.00-mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium... Problem 137CP Problem 138CP: A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete... Problem 139CP: Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g... Problem 140CP Problem 141CP Problem 142IP: Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate... Problem 143IP: In a 1-L beaker, 203 mL of 0.307 M ammonium chromate was mixed with 137 mL of 0.269 M chromium(III)... Problem 144IP: The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with... Problem 145IP: The unknown acid H2X can be neutralized completely by OH according to the following (unbalanced)... Problem 146MP: Three students were asked to find the identity of the metal in a particular sulfate salt. They... Problem 147MP: You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246%... Problem 111AE
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Concept explainers
Just solve questions 3-7, thanks.
1
Given the reaction: 2HNO3 + Cu + H+ à 2NO2 + Cu2+ + 2H2 O. Which statement is correct?
A) N is the reducing agent and Cu is the oxidizing agent.
B) N is the reducing agent and H+ is the oxidizing agent.
C) Cu is the reducing agent and H+ is the oxidizing agent.
D) Cu is the reducing agent and N is oxidizing agent.
E) H+ is the reducing agent and Cu is the oxidizing agent.
2
In which of the following species does sulfur have the same oxidation number as it does in H2 SO4 ?
(A) H2 SO3 (B) S2 O3 2 − (C) S2 − (D) S8 (E) SO2 Cl2
3
Given the balanced redox reaction: 6 I− + 2 MnO4 − + 4 H2 O(l) à 3 I2(s) + 2 MnO2(s) + OH−
Which of the following statements regarding the reaction represented by the equation above is correct?
(A) Iodide ion is oxidized by hydroxide ion. (D) The oxidation number of Mn remains the same.
(B) MnO4 − is oxidized by iodide ion. (E) The oxidation number of Iodine changes from −1 to 0.
(C) The oxidation number of Mn changes from +7 to +2.
4
The balanced half reaction is given: Cr2 O7 2− + __ e− + 14 H+ à 2 Cr3+ + 7 H2 O(l)
What is the appropriate coefficient to reflect the number of electrons needed?
A) 4 B) 5 C) 6 D) 9 E) 12
5
The oxidation number of chromium in dichromate, Cr2 O7 2− , is:
A) 2 B) 4 C) 6 D) 7 E) -2
6
In Fe2 (SO4 )3 , the oxidation numbers of Fe, S and O, respectively, are:
A) 2, 3, -4 B) 3, 6, -2 C) 2, 4, -8 D) 2, 4, -2 E) 4, 5, -3
7
Consider the following redox reaction:
2Cr(OH)3 + ClO3 - + OH- à CrO4 2- + 2 H2 O
A) The reaction is balanced and occurred in an acidic environment
B) The reaction is unbalanced and occurred in a basic environment
C) The reaction is balanced and occurred in a basic environment
D) The reaction is unbalanced and occurred in an acidic environment
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
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