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 106AE: Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active...
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Concept explainers
By now your baking soda conversion experiment should be nearly complete. If not, take a short break while you wait for the 1-hour chemical reaction to finish.
Before baking in the oven I recorded that: mass foil in grams is 0.55g
Mass foil + baking soda - 3.65g
Mass of baking soda alone - 3.10g
after 1 hour in oven - mass of foil and baking soda - 2.63 g
Begin by coping the following table the following table into your lab notebook or digital software of choice (eg. word, google sheets, excel, etc.). You will submit the completed table at the end of this question.
Mass of aluminum foil + product in grams (2)2.63gMass of aluminum foil alone in grams (3)0.55g Actual yield in grams (3)Initial mass of reactant (baking soda) in grams (4)Initial moles of reactant (baking soda) (4)Moles of sodium carbonate (soda ash) product expected (5)Molar mass of sodium carbonate (soda ash) (6)Theoretical yield in grams (6)Percent yield of experiment (7)After 1 hour is complete, turn off the oven and carefully remove your aluminum foil pan from your oven or toaster oven. Allow to cool for at least 2 minutes.Take the mass of the aluminum foil pan and the product of your reaction. Do not attempt to remove the carbonate product from the foil pan before taking the mass.Copy the mass of the aluminum foil pan into your data table (this was recorded in part 1). Calculate the mass of the carbonate product by subtracting the foil+pan mass from the mass of the foil pan.The mass of product is your actual yield – the amount of carbonate that you ACTUALLY created in this experiment. Now we will calculate your theoretical yield the amount that we THEORETICALLY expect based on our starting quantity of baking soda. State the initial mass and moles of baking soda in your data table (which should come from your existing data).Calculate the number of moles of soda ash (sodium carbonate) that we expect from this reaction. Remember our chemical equation? This states that every 2 moles of the bicarbonate will make 1 mole of the carbonate! Therefore, we can calculate this using:
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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