General Chemistry - Standalone book (MindTap Course List) 11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
1 Chemistry And Measurement 2 Atoms, Molescules, And Ions 3 Calculations With Chemical Formulas And Equaitons 4 Chemical Reactions 5 The Gaseous State 6 Thermochemisty 7 Quantum Theory Of The Atom 8 Electron Configurations And Periodicity 9 Ionic And Covalent Bonding 10 Molecular Geometry And Chemical Bonding Theory 11 States Of Matter; Liquids And Solids 12 Solutions 13 Rates Of Reaction 14 Chemical Equilibirum 15 Acids And Bases 16 Acid-base Equilibria 17 Solubility And Complex-ion Equilibria 18 Thermodynamics And Equilibrium 19 Electrochemistry 20 Nuclear Chemistry 21 Chemistry Of The Main-group Elements 22 The Transition Elements And Coordination Compounds 23 Organic Chemistry 24 Polymer Materials: Synthetic And Biological A.1 Scientific (exponential) Notation A.2 Logarithms A.3 Algebraic Operations And Graphing Chapter4: Chemical Reactions
4.1 Ionic Theory Of Solutions And Solubility Rules 4.2 Molecular And Ionic Equations 4.3 Precipitation Reactions 4.4 Acid-base Reactions 4.5 Oxidation-reduction Reactions 4.6 Balancing Simple Oxidation-reduction Equations 4.7 Molar Concentration 4.8 Diluting Solutions 4.9 Gravimetric Analysis 4.10 Volumetric Analysis Chapter Questions Section: Chapter Questions
Problem 4.1QP: Explain why some electrolyte solutions are strongly conducting, whereas others are weakly... Problem 4.2QP: Define the terms strong electrolyte and weak electrolyte. Give an example of each. Problem 4.3QP: Explain the terms soluble and insoluble. Use the solubility rules to write the formula of an... Problem 4.4QP: What are the advantages and disadvantages of using a molecular equation to represent an ionic... Problem 4.5QP: What is a spectator ion? Illustrate with a complete ionic reaction. Problem 4.6QP Problem 4.7QP Problem 4.8QP: Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid... Problem 4.9QP: Give an example of a neutralization reaction. Label the acid, base, and salt. Problem 4.10QP: Give an example of a polyprotic acid and write equations for the successive neutralizations of the... Problem 4.11QP Problem 4.12QP Problem 4.13QP: Why is the product of molar concentration and volume constant for a dilution problem? Problem 4.14QP: Describe how the amount of sodium hydroxide in a mixture can be determined by titration with... Problem 4.15QP: What is the net ionic equation for the following molecular equation? HF(aq)+KOH(aq)KF(aq)+H2O(l)... Problem 4.16QP: An aqueous sodium hydroxide solution mixed with an aqueous magnesium nitrate solution yields which... Problem 4.17QP: Which of the following compounds would produce the highest concentration of Cl ions when 0.10 mol of... Problem 4.18QP: In an aqueous 0.10 M HNO2 solution (HNO2 is a weak electrolyte), which of the following would you... Problem 4.19QP: The Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in... Problem 4.20QP: Working with Concentration (Molarity Concepts) Note: You should be able to answer all of the... Problem 4.21QP Problem 4.22QP Problem 4.23QP: You come across a beaker that contains water, aqueous ammonium acetate, and a precipitate of calcium... Problem 4.24QP: Three acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving... Problem 4.25QP: Would you expect a precipitation reaction between an ionic compound that is an electrolyte and an... Problem 4.26QP: Equal quantities of the hypothetical strong acid HX, weak acid HA, and weak base BZ are added to... Problem 4.27QP: Try and answer the following questions without using a calculator. a A solution is made by mixing... Problem 4.28QP: If one mole of the following compounds were each placed into separate beakers containing the same... Problem 4.29QP: Using solubility rules, predict the solubility in water of the following ionic compounds. a PbS b... Problem 4.30QP: Using solubility rules, predict the solubility in water of the following ionic compounds. a Al(OH)3... Problem 4.31QP: Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water.... Problem 4.32QP: Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water.... Problem 4.33QP: Write net ionic equations for the following molecular equations. HBr is a strong electrolyte. a... Problem 4.34QP: Write net ionic equations for the following molecular equations. HBr is a strong electrolyte. a... Problem 4.35QP: Lead(II) nitrate solution and sodium sulfate solution are mixed. Crystals of lead(II) sulfate come... Problem 4.36QP: Lithium carbonate solution reacts with aqueous hydrobromic acid to give a solution of lithium... Problem 4.37QP: Write the molecular equation and the net ionic equation for each of the following aqueous reactions.... Problem 4.38QP: Write the molecular equation and the net ionic equation for each of the following aqueous reactions.... Problem 4.39QP: For each of the following, write molecular and net ionic equations for any precipitation reaction... Problem 4.40QP: For each of the following, write molecular and net ionic equations for any precipitation reaction... Problem 4.41QP: Classify each of the following as a strong or weak acid or base. a HF b KOH c HClO4 d HIO Problem 4.42QP: Classify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3 Problem 4.43QP: Complete and balance each of the following molecular equations (in aqueous solution); include phase... Problem 4.44QP: Complete and balance each of the following molecular equations (in aqueous solution); include phase... Problem 4.45QP: For each of the following, write the molecular equation, including phase labels. Then write the net... Problem 4.46QP: For each of the following, write the molecular equation, including phase labels. Then write the net... Problem 4.47QP Problem 4.48QP: Complete the right side of each of the following molecular equations. Then write the net ionic... Problem 4.49QP: Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen... Problem 4.50QP: Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen... Problem 4.51QP: The following reactions occur in aqueous solution. Complete and balance the molecular equations... Problem 4.52QP: The following reactions occur in aqueous solution. Complete and balance the molecular equations... Problem 4.53QP: Write the molecular equation and the net ionic equation for the reaction of solid iron(II) sulfide... Problem 4.54QP: Write the molecular equation and the net ionic equation for the reaction of solid barium carbonate... Problem 4.55QP: Obtain the oxidation number for the element noted in each of the following. a Sn in SnO2 b Ta in... Problem 4.56QP: Obtain the oxidation number for the element noted in each of the following. a Cr in CrO3 b Hg in... Problem 4.57QP: Obtain the oxidation number for the element noted in each of the following. a N in NH2 b I in IO3 c... Problem 4.58QP Problem 4.59QP: Determine the oxidation numbers of all the elements in each of the following compounds. (Hint: Look... Problem 4.60QP: Determine the oxidation numbers of all the elements in each of the following compounds. (Hint: Look... Problem 4.61QP: In the following reactions, label the oxidizing agent and the reducing agent. a P4(s) + 5O2(g)... Problem 4.62QP: In the following reactions, label the oxidizing agent and the reducing agent. a ZnO(s) + C(s) Zn(g)... Problem 4.63QP: In the following reactions, label the oxidizing agent and the reducing agent. a 2Al(s) + 3F2(g) ... Problem 4.64QP: In the following reactions, label the oxidizing agent and the reducing agent. a Fe2O3(s) + 3CO(g) ... Problem 4.65QP: Balance the following oxidationreduction reactions by the half-reaction method. a CuCl2(aq) + Al(s) ... Problem 4.66QP: Balance the following oxidationreduction reactions by the half-reaction method. a FeI3(aq) + Mg(s) ... Problem 4.67QP: A sample of 0.0606 mol of iron(III) chloride, FeCl3, was dissolved in water to give 35.4 mL of... Problem 4.68QP: A 50.0-mL volume of AgNO3 solution contains 0.0345 mol AgNO3 (silver nitrate). What is the molarity... Problem 4.69QP: An aqueous solution is made from 0.798 g of potassium permanganate, KMnO4. If the volume of solution... Problem 4.70QP Problem 4.71QP: What volume of 0.120 M CuSO4 is required to give 0.150 mol of copper(II) sulfate, CuSO4? Problem 4.72QP Problem 4.73QP: An experiment calls for 0.0353 g of potassium hydroxide, KOH. How many milliliters of 0.0176 M KOH... Problem 4.74QP: What is the volume (in milliliters) of 0.100 M H2SO4 (sulfuric acid) containing 0.949 g H2SO4? Problem 4.75QP: Heme, obtained from red blood cells, binds oxygen, O2. How many moles of heme are there in 150 mL of... Problem 4.76QP: Insulin is a hormone that controls the use of glucose in the body. How many moles of insulin are... Problem 4.77QP Problem 4.78QP: Describe how you would prepare 2.50 102 mL of 0.50 M Na2SO4. What mass (in grams) of sodium... Problem 4.79QP: You wish to prepare 0.12 M HNO3 from a stock solution of nitric acid that is 15.8 M. How many... Problem 4.80QP Problem 4.81QP: A 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to... Problem 4.82QP: Calculate the concentrations of each ion present in a solution that results from mixing 50.0 mL of a... Problem 4.83QP: A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to... Problem 4.84QP: A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to... Problem 4.85QP: Copper has compounds with copper(I) ion or copper(II) ion. A compound of copper and chlorine was... Problem 4.86QP: Gold has compounds containing gold(I) ion or gold(III) ion. A compound of gold and chlorine was... Problem 4.87QP: A compound of iron and chlorine is soluble in water. An excess of silver nitrate was added to... Problem 4.88QP: A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a... Problem 4.89QP: What volume of 0.230 M HNO3 (nitric acid) reacts with 49.0 mL of 0.330 M Na2CO3 (sodium carbonate)... Problem 4.90QP Problem 4.91QP Problem 4.92QP: How many milliliters of 0.250 M KMnO4 are needed to react with 3.55 g of iron(II) sulfate, FeSO4?... Problem 4.93QP: A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4.... Problem 4.94QP Problem 4.95QP: Magnesium metal reacts with hydrobromic acid to produce hydrogen gas and a solution of magnesium... Problem 4.96QP: Aluminum metal reacts with perchloric acid to produce hydrogen gas and a solution of aluminum... Problem 4.97QP: Nickel(II) sulfate solution reacts with sodium hydroxide solution to produce a precipitate of... Problem 4.98QP: Potassium sulfate solution reacts with barium bromide solution to produce a precipitate of barium... Problem 4.99QP Problem 4.100QP: Decide whether a reaction occurs for each of the following. If it does not, write NR after the... Problem 4.101QP: Complete and balance each of the following molecular equations, including phase labels, if a... Problem 4.102QP Problem 4.103QP: Describe in words how you would do each of the following preparations. Then give the molecular... Problem 4.104QP Problem 4.105QP: Classify each of the following reactions as a combination reaction, decomposition reaction,... Problem 4.106QP: Classify each of the following reactions as a combination reaction, decomposition reaction,... Problem 4.107QP Problem 4.108QP Problem 4.109QP Problem 4.110QP Problem 4.111QP: A stock solution of potassium dichromate, K2Cr2O7, is made by dissolving 84.5 g of the compound in... Problem 4.112QP: A 71.2-g sample of oxalic acid, H2C2O4, was dissolved in 1.00 L of solution. How would you prepare... Problem 4.113QP Problem 4.114QP: An aqueous solution contains 3.75% NH3 (ammonia) by mass. The density of the aqueous ammonia is... Problem 4.115QP: A barium mineral was dissolved in hydrochloric acid to give a solution of barium ion. An excess of... Problem 4.116QP: Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride,... Problem 4.117QP Problem 4.118QP: An antacid tablet has calcium carbonate as the active ingredient; other ingredients include a starch... Problem 4.119QP: A sample of CuSO45H2O was heated to 110C, where it lost water and gave another hydrate of copper(II)... Problem 4.120QP Problem 4.121QP: A water-soluble compound of gold and chlorine is treated with silver nitrate to convert the chlorine... Problem 4.122QP: A solution of scandium chloride was treated with silver nitrate. The chlorine in the scandium... Problem 4.123QP: A 0.608-g sample of fertilizer contained nitrogen as ammonium sulfate, (NH4)2SO4. It was analyzed... Problem 4.124QP: An antacid tablet contains sodium hydrogen carbonate, NaHCO3, and inert ingredients. A 0.465-g... Problem 4.125QP: You order a glass of juice in a restaurant, only to discover that it is warm and too sweet. The... Problem 4.126QP Problem 4.127QP Problem 4.128QP Problem 4.129QP: Zinc acetate is sometimes prescribed by physicians for the treatment of Wilsons disease, which is a... Problem 4.130QP: Arsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent... Problem 4.131QP: When the following equation is balanced by the half-reaction method using the smallest set of... Problem 4.132QP: Identify each of the following reactions as being a neutralization, precipitation, or oxidation... Problem 4.133QP Problem 4.134QP Problem 4.135QP: A 25-mL sample of 0.50 M NaOH is combined with a 75-mL sample of 0.50 M NaOH. What is the... Problem 4.136QP: What is the molarity of pure water with a density of 1.00 g/mL? Problem 4.137QP Problem 4.138QP: How many grams of precipitate are formed if 175 mL of a 0.750 M aluminum sulfate solution and 375 mL... Problem 4.139QP Problem 4.140QP: Potassium hydrogen phthalate (abbreviated as KHP) has the molecular formula KHC8H4O4 and a molar... Problem 4.141QP: Lead(II) nitrate reacts with cesium sulfate in an aqueous precipitation reaction. What are the... Problem 4.142QP: Silver nitrate reacts with strontium chloride in an aqueous precipitation reaction. What are the... Problem 4.143QP: Elemental bromine is the source of bromine compounds. The element is produced from certain brine... Problem 4.144QP Problem 4.145QP Problem 4.146QP Problem 4.147QP: Iron forms a sulfide with the approximate formula Fe7S8. Assume that the oxidation state of sulfur... Problem 4.148QP: A transition metal X forms an oxide of formula X2O3. It is found that only 50% of X atoms in this... Problem 4.149QP: What volume of a solution of ethanol, C2H6O, that is 94.0% ethanol by mass contains 0.200 mol C2H6O?... Problem 4.150QP: What volume of a solution of ethylene glycol, C2H6O2, that is 56.0% ethylene glycol by mass contains... Problem 4.151QP: A 10.0-mL sample of potassium iodide solution was analyzed by adding an excess of silver nitrate... Problem 4.152QP: A 25.0-mL sample of sodium sulfate solution was analyzed by adding an excess of barium chloride... Problem 4.153QP: A metal, M, was converted to the sulfate, M2(SO4)3. Then a solution of the sulfate was treated with... Problem 4.154QP: A metal, M, was converted to the chloride MCl2. Then a solution of the chloride was treated with... Problem 4.155QP: Phosphoric acid is prepared by dissolving phosphorus(V) oxide, P4O10, in water. What is the balanced... Problem 4.156QP: Iron(III) chloride can be prepared by reacting iron metal with chlorine. What is the balanced... Problem 4.157QP: An alloy of aluminum and magnesium was treated with sodium hydroxide solution, in which only... Problem 4.158QP: An alloy of iron and carbon was treated with sulfuric acid, in which only iron reacts.... Problem 4.159QP: Determine the volume of sulfuric acid solution needed to prepare 37.4 g of aluminum sulfate,... Problem 4.160QP: Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4,... Problem 4.161QP: The active ingredients of an antacid tablet contained only magnesium hydroxide and aluminum... Problem 4.162QP: The active ingredients in an antacid tablet contained only calcium carbonate and magnesium... Problem 4.163QP Problem 4.160QP: Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4,...
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According to the balanced chemical reaction , how many grams of sodium carbonate and calcium hydroxide would be required to produce 96.7 g sodium hydroxide? Na2CO3 + Ca(OH)2 = 2NaOH + CaCO3
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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