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 4.70QP
Related questions
Net ionic equation practice problems:
An aqueous solution of sodium sulfide (Na2S) is added to aluminum chloride (AlCl3) dissolved into water. Upon mixing of the solutions, a precipitate forms.
a. Write out the balanced, molecular equation, including states of matter.
b. Write the ionic equation by separating all aqueous ionic compounds into their constituent ions. the spectator ions.
c. Write the net ionic equation by eliminating the spectator ions on both sides of the equation.
Transcribed Image Text: molecular equation
Ba(OH)2(aq)
Na,so
Ba(OH)2 (aq) + Na2S04 (aq) → BaSO4 (s) + 2 NaOH (aq)
+
4(ад)
Ва(ОН),
net ionic equation
3.
molecular equation
AGNO,
3(aq)
MgCl,
2(aq)
net ionic equation
2.
Definition Definition Substance that constitutes everything in the universe. Matter consists of atoms, which are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction: solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
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