Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter4: 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: Molarity is a conversion factor relating moles of solute in solution to the volume of the solution.... Problem 5RQ: What is a dilution? What stays constant in a dilution? Explain why the equation M1 V1 = M2 V2 works... Problem 6RQ: When the following beakers are mixed, draw a molecular-level representation of the product mixture... Problem 7RQ: Differentiate between the formula equation, the complete ionic equation, and the net ionic equation.... Problem 8RQ: What is an acid-base reaction? Strong bases are soluble ionic compounds that contain the hydroxide... Problem 9RQ: Define the terms oxidation, reduction, oxidizing agent, and reducing agent. Given a chemical... Problem 1ALQ: Assume you have a highly magnified view of a solution of HCl that allows you to see the HCl. Draw... Problem 2ALQ: You have a solution of table salt in water. What happens to the salt concentration (increases,... Problem 3ALQ: You have a sugar solution (solution A) with concentration x. You pour one-fourth of this solution... Problem 4ALQ: You add an aqueous solution of lead nitrate to an aqueous solution of potassium iodide. Draw highly... Problem 5ALQ: Order the following molecules from lowest to highest oxidation state of the nitrogen atom: HNO3,... Problem 6ALQ: Why is it that when something gains electrons, it is said to be reduced? What is being reduced? Problem 7ALQ: Consider separate aqueous solutions of HCl and H2SO4 with the same molar concentrations. You wish to... Problem 8ALQ Problem 10ALQ: On the basis of the general solubility rules given in Table 4.1, predict the identity of the... Problem 11ALQ Problem 12ALQ: The exposed electrodes of a light bulb are placed in a solution of H2SO4 in an electrical circuit... Problem 15ALQ: The equation Ag(aq) + Cu(s) Cu2(aq) + Ag(s) has equal numbers of each type of element on each side... Problem 16ALQ: In balancing oxidation-reduction reactions, why is it permissible to add water to either side of the... Problem 17Q: Differentiate between what happens when the following are added to water. a. polar solute versus... Problem 18Q: A typical solution used in general chemistry laboratories is 3.0 M HCl. Describe, in detail, the... Problem 19Q Problem 20Q: 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 21Q: List the formulas of three soluble bromide salts and three insoluble bromide salts. Do the same... Problem 22Q: When 1.0 mole of solid lead nitrate is added to 2.0 moles of aqueous potassium iodide, a yellow... Problem 23Q: What is an acid and what is a base? An acid-base reaction is sometimes called a proton-transfer... Problem 24Q: 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 25Q: Differentiate between the following terms. a. species reduced versus the reducing agent b. species... Problem 27E Problem 28E: Match each name below with the following microscopic pictures of that compound in aqueous solution.... Problem 29E: Calcium chloride is a strong electrolyte and is used to salt streets in the winter to melt ice and... Problem 30E: Commercial cold packs and hot packs are available for treating athletic injuries. Both types contain... Problem 31E: Calculate the molarity of each of these solutions. a. A 5.623-g sample of NaHCO3 is dissolved in... Problem 32E: A solution of ethanol (C2H5OH) in water is prepared by dissolving 75.0 mL of ethanol (density = 0.79... Problem 33E: Calculate the concentration of all ions present in each of the following solutions of strong... Problem 34E Problem 35E Problem 36E Problem 37E Problem 38E: If 10. g of AgNO3 is available, what volume of 0.25 M AgNO3 solution can be prepared? Problem 39E: The sodium level in a patients blood was measured at 137 mmol/L. If 15.0 mL of blood is drawn from... Problem 40E: High-density lipoprotein (HDL) cholesterol is the good cholesterol because adequate levels reduce... Problem 43E: A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of... Problem 44E: 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 45E: Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of... Problem 46E: Suppose 50.0 mL of 0.250 M CoCl2 solution is added to 25.0 mL of 0.350 M NiCl2 solution. Calculate... Problem 47E Problem 48E: A stock solution containing Mn2+ ions was prepaned by dissolving 1.584 g pure manganese metal in... Problem 49E: On the basis of the general solubility rules given in Table 6-1, predict which of the following... Problem 50E: On the basis of the general solubility rules given in Table 6-1, predict which of the following... Problem 51E: When the following solutions are mixed together, what precipitate (if any) will form? a. FeSO4(aq) +... Problem 52E: When the following solutions are mixed together, what precipitate (if any) will form? a.... Problem 53E: For the reactions in Exercise 47, write the balanced formula equation, complete ionic equation, and... Problem 54E: For the reactions in Exercise 48, write the balanced formula equation, complete ionic equation, and... Problem 55E: Write the balanced formula and net ionic equation for the reaction that occurs when the contents of... Problem 56E: Give an example how each of the following insoluble ionic compounds could be produced using a... Problem 57E: Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the... Problem 58E: Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the... Problem 59E: Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4,... Problem 60E: A sample may contain any or all of the following ions: Hg22+, Ba2+, and Mn2+. a. No precipitate... Problem 61E: What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100-M... Problem 62E: What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 150.0 mL of... Problem 63E: What mass of iron(III) hydroxide precipitate can be produced by reacting 75.0 mL of 0.105 M... Problem 66E: What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate... Problem 67E: A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous... Problem 69E: A 1.42-g sample of a pure compound, with formula M2SO4, was dissolved in water and treated with an... Problem 70E: You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into... Problem 71E: Write the balanced formula, complete ionic, and net ionic equations for each of the following... Problem 72E: Write the balanced formula, complete ionic, and net ionic equations for each of the following... Problem 73E: Write the balanced formula equation for the acid-base reactions that occur when the following are... Problem 74E Problem 75E: What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH? a.... Problem 76E Problem 77E: 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 78E: A student mixes four reagents together, thinking that the solutions will neutralize each other. The... Problem 79E: A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for... Problem 80E: A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with 0.5062... Problem 81E: What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric... Problem 82E: 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 83E: A student titrates an unknown amount of potassium hydrogen phthalate (KHC8H4O4, often abbreviated... Problem 84E: The concentration of a certain sodium hydroxide solution was determined by using the solution to... Problem 85E: Assign oxidation states for all atoms in each of the following compounds. a. KMnO4 b. NiO2 c.... Problem 87E: Assign the oxidation state for nitrogen in each of the following. a. Li3N b. NH3 c. N2H4 d. NO e.N2O... Problem 88E: Assign oxidatioo numbers to all the atoms in each of the following. a. SrCr2O7 b. CuCl2 c. O2 d.... Problem 89E: Specify which of the following are oxidationreduction reactions, and identify the oxidizing agent,... Problem 90E: Specify which of the following equations represent oxidationreduction reactions, and indicate the... Problem 91E: Balance the following oxidation-reduction reactions occur in acidic solution using the half-reaction... Problem 92E: Balance the following oxidation-reduction reactions that occur in acidic solution using the... Problem 93E: Balance the following oxidation-reduction reactions that occur in basic solution. a. Al(s) +... Problem 94E: Balance the following oxidation-reduction reactions that occur in basic solution. a. Cr(s) +... Problem 95E: Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with... Problem 96E Problem 98E: The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron... Problem 101AE: You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final... Problem 102AE: The figures below are molecular-level representations of four aqueous solutions of the same solute.... Problem 103AE Problem 104AE Problem 105AE: Many plants are poisonous because their stems and leaves contain oxalic acid H2C2O4, or sodium... Problem 106AE: Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active... Problem 107AE: Using the general solubility rules given in Table 6-1. name three reagents that would form... Problem 108AE: Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture... Problem 109AE: A 1.00-g sample of an alkaline earth metal chloride is treated with excess silver nitrate. All of... Problem 110AE: A mixture contains only NaCl and Al2(SO4)3. A 1.45-g sample of the mixture is dissolved in water and... Problem 112AE: A mixture contains only NaCl and Fe(NO3)3. A 0.456-g sample of the mixture is dissolved in water,... Problem 113AE: A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then... Problem 114AE: Some of the substances commonly used in stomach antacids are MgO, Mg(OH)2, and Al(OH)3. a. Write a... Problem 115AE: Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium... Problem 116AE: When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are... Problem 117AE: A 2.20-g sample of an unknown acid (empirical formula = C3H4O3) is dissolved in 1.0 L of water. A... Problem 118AE: Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only... Problem 119AE: Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g... Problem 120AE: Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894... Problem 121AE: Douglasite is a mineral with the formula 2KC1 FeCl2 2H2O. Calculate the mass percent of douglasite... Problem 122AE: Many oxidationreduction reactions can be balanced by inspection. Try to balance the following... Problem 123AE Problem 124CWP: Calculate the concentration of all ions present when 0.160 g of MgCl2 is dissolved in 100.0 mL of... Problem 125CWP: A solution is prepared by dissolving 0.6706 g oxalic acid (H2C2O4) in enough water to make 100.0 mL... Problem 126CWP: For the following chemical reactions, determine the precipitate produced when the two reactants... Problem 127CWP: What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a... Problem 128CWP Problem 129CWP: 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 130CWP: The zinc in a 1.343-g sample of a foot powder was precipitated as ZnNH4PO4. Strong heating of the... Problem 131CWP: A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944-M nitric acid for neutralization.... Problem 132CWP: When organic compounds containing sulfur are burned, sulfurdioxide is produced. The amount of SO2... Problem 133CWP: Assign the oxidation state for the element Listed in each of the following compounds: Oxidation... Problem 134CP: A 10.00-g sample consisting of a mixture of sodium chloride and potassium sulfate is dissolved in... Problem 135CP: The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental... Problem 136CP: In the spectroscopic analysis of many substances, a series of standard solutions of known... Problem 137CP: In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing... Problem 138CP: Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical... Problem 139CP: Consider the reaction of 19.0 g of zinc with excess silver nitrite to produce silver metal and zinc... Problem 140CP: A mixture contains only sodium chloride and potassium chloride. A 0.1586-g sample of the mixture was... Problem 141CP Problem 142CP: Zinc and magnesium metal each react with hydrochloric acid according to the following equations:... Problem 143CP: You made 100.0 mL of a lead(II) nitrate solution for lab but forgot to cap it. The next lab session... Problem 144CP: Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by... Problem 145CP: Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that... Problem 146CP: Complete and balance each acid-base reaction. a. H3PO4(aq) + NaOH(aq) Contains three acidic... Problem 147CP: What volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4?... Problem 148CP: A 10.00-mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium... Problem 149CP: A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of... Problem 150CP: A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete... Problem 151CP: Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g... Problem 152CP Problem 153CP: It took 25.06 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see... Problem 154CP: Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution:... Problem 155CP: Chromium has been investigated as a coating for steel cans. The thickness of the chromium film is... Problem 156IP Problem 157IP: 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 158IP: The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with... Problem 159IP: The unknown acid H2X can be neutralized completely by OH according to the following (unbalanced)... Problem 160MP: Three students were asked to find the identity of the metal in a particular sulfate salt. They... Problem 161MP: You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246%... Problem 10ALQ: On the basis of the general solubility rules given in Table 4.1, predict the identity of the...
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Watch this video of a double displacement experiment:
https://www.youtube.com/watch?v=mph8Hq_75vU
Write the balanced chemical reactions , including state of the matter
What is the precipitate that forms, and which color is it?
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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