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OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
11th Edition
ISBN: 9781305673939
Author: Darrell Ebbing; Steven D. Gammon
Publisher: Cengage Learning US
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Chapter 4, Problem 4.84QP
A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?
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6. Consider the following exothermic reaction below.
2Cu2+(aq) +41 (aq)2Cul(s) + 12(aq)
a. If Cul is added, there will be a shift left/shift right/no shift (circle one).
b. If Cu2+ is added, there will be a shift left/shift right/no shift (circle one).
c. If a solution of AgNO3 is added, there will be a shift left/shift right/no shift (circle one).
d. If the solvent hexane (C6H14) is added, there will be a shift left/shift right/no shift (circle
one). Hint: one of the reaction species is more soluble in hexane than in water.
e. If the reaction is cooled, there will be a shift left/shift right/no shift (circle one).
f. Which of the changes above will change the equilibrium constant, K?
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Chapter 4 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
Ch. 4.1 - Which of the following would you expect to be...Ch. 4.1 - Determine whether the following compounds are...Ch. 4.1 - Prob. 4.2CCCh. 4.2 - Write complete ionic and net ionic equations for...Ch. 4.3 - You mix aqueous solutions of sodium iodide and...Ch. 4.3 - Your lab partner tells you that she mixed two...Ch. 4.4 - Complete and balance the two chemical equations....Ch. 4.4 - Label each of the following as a strong or weak...Ch. 4.4 - Write the molecular equation and the net ionic...Ch. 4.4 - Write molecular and net ionic equations for the...
Ch. 4.4 - Prob. 4.7ECh. 4.4 - Prob. 4.5CCCh. 4.5 - Obtain the oxidation numbers of the atoms in each...Ch. 4.6 - Prob. 4.9ECh. 4.7 - A sample of sodium chloride, NaCl, weighing 0....Ch. 4.7 - How many milliliters of 0. 163 M NaCl are required...Ch. 4.7 - How many moles of sodium chloride should be put in...Ch. 4.8 - You have a solution that is 1.5 M H2SO4 (sulfuric...Ch. 4.8 - Consider the following beakers. Each contains a...Ch. 4.9 - You are given a sample of limestone, which is...Ch. 4.10 - Nickel sulfate, NiSO4, reacts with sodium...Ch. 4.10 - A 5.00-g sample of vinegar is titrated with 0.108...Ch. 4.10 - Consider three flasks, each containing 0.10 mol of...Ch. 4 - Explain why some electrolyte solutions are...Ch. 4 - Define the terms strong electrolyte and weak...Ch. 4 - Explain the terms soluble and insoluble. Use the...Ch. 4 - What are the advantages and disadvantages of using...Ch. 4 - What is a spectator ion? Illustrate with a...Ch. 4 - Prob. 4.6QPCh. 4 - Prob. 4.7QPCh. 4 - Describe in words how you would prepare pure...Ch. 4 - Give an example of a neutralization reaction....Ch. 4 - Give an example of a polyprotic acid and write...Ch. 4 - Prob. 4.11QPCh. 4 - Prob. 4.12QPCh. 4 - Why is the product of molar concentration and...Ch. 4 - Describe how the amount of sodium hydroxide in a...Ch. 4 - What is the net ionic equation for the following...Ch. 4 - An aqueous sodium hydroxide solution mixed with an...Ch. 4 - Which of the following compounds would produce the...Ch. 4 - In an aqueous 0.10 M HNO2 solution (HNO2 is a weak...Ch. 4 - The Behavior of Substances in Water Part 1: a...Ch. 4 - Working with Concentration (Molarity Concepts)...Ch. 4 - Prob. 4.21QPCh. 4 - Prob. 4.22QPCh. 4 - You come across a beaker that contains water,...Ch. 4 - Three acid samples are prepared for titration by...Ch. 4 - Would you expect a precipitation reaction between...Ch. 4 - Equal quantities of the hypothetical strong acid...Ch. 4 - Try and answer the following questions without...Ch. 4 - If one mole of the following compounds were each...Ch. 4 - Using solubility rules, predict the solubility in...Ch. 4 - Using solubility rules, predict the solubility in...Ch. 4 - Using solubility rules, decide whether the...Ch. 4 - Using solubility rules, decide whether the...Ch. 4 - Write net ionic equations for the following...Ch. 4 - Write net ionic equations for the following...Ch. 4 - Lead(II) nitrate solution and sodium sulfate...Ch. 4 - Lithium carbonate solution reacts with aqueous...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - For each of the following, write molecular and net...Ch. 4 - For each of the following, write molecular and net...Ch. 4 - Classify each of the following as a strong or weak...Ch. 4 - Classify each of the following as a strong or weak...Ch. 4 - Complete and balance each of the following...Ch. 4 - Complete and balance each of the following...Ch. 4 - For each of the following, write the molecular...Ch. 4 - For each of the following, write the molecular...Ch. 4 - Prob. 4.47QPCh. 4 - Complete the right side of each of the following...Ch. 4 - Write molecular and net ionic equations for the...Ch. 4 - Write molecular and net ionic equations for the...Ch. 4 - The following reactions occur in aqueous solution....Ch. 4 - The following reactions occur in aqueous solution....Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Prob. 4.58QPCh. 4 - Determine the oxidation numbers of all the...Ch. 4 - Determine the oxidation numbers of all the...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - Balance the following oxidationreduction reactions...Ch. 4 - Balance the following oxidationreduction reactions...Ch. 4 - A sample of 0.0606 mol of iron(III) chloride,...Ch. 4 - A 50.0-mL volume of AgNO3 solution contains 0.0345...Ch. 4 - An aqueous solution is made from 0.798 g of...Ch. 4 - Prob. 4.70QPCh. 4 - What volume of 0.120 M CuSO4 is required to give...Ch. 4 - Prob. 4.72QPCh. 4 - An experiment calls for 0.0353 g of potassium...Ch. 4 - What is the volume (in milliliters) of 0.100 M...Ch. 4 - Heme, obtained from red blood cells, binds oxygen,...Ch. 4 - Insulin is a hormone that controls the use of...Ch. 4 - Prob. 4.77QPCh. 4 - Describe how you would prepare 2.50 102 mL of...Ch. 4 - You wish to prepare 0.12 M HNO3 from a stock...Ch. 4 - Prob. 4.80QPCh. 4 - A 8.50 g sample of KCl is dissolved in 66.0 mL of...Ch. 4 - Calculate the concentrations of each ion present...Ch. 4 - A chemist added an excess of sodium sulfate to a...Ch. 4 - A soluble iodide was dissolved in water. Then an...Ch. 4 - Copper has compounds with copper(I) ion or...Ch. 4 - Gold has compounds containing gold(I) ion or...Ch. 4 - A compound of iron and chlorine is soluble in...Ch. 4 - A 1.345-g sample of a compound of barium and...Ch. 4 - What volume of 0.230 M HNO3 (nitric acid) reacts...Ch. 4 - Prob. 4.90QPCh. 4 - Prob. 4.91QPCh. 4 - How many milliliters of 0.250 M KMnO4 are needed...Ch. 4 - A solution of hydrogen peroxide, H2O2, is titrated...Ch. 4 - Prob. 4.94QPCh. 4 - Magnesium metal reacts with hydrobromic acid to...Ch. 4 - Aluminum metal reacts with perchloric acid to...Ch. 4 - Nickel(II) sulfate solution reacts with sodium...Ch. 4 - Potassium sulfate solution reacts with barium...Ch. 4 - Prob. 4.99QPCh. 4 - Decide whether a reaction occurs for each of the...Ch. 4 - Complete and balance each of the following...Ch. 4 - Prob. 4.102QPCh. 4 - Describe in words how you would do each of the...Ch. 4 - Prob. 4.104QPCh. 4 - Classify each of the following reactions as a...Ch. 4 - Classify each of the following reactions as a...Ch. 4 - Prob. 4.107QPCh. 4 - Prob. 4.108QPCh. 4 - Prob. 4.109QPCh. 4 - Prob. 4.110QPCh. 4 - A stock solution of potassium dichromate, K2Cr2O7,...Ch. 4 - A 71.2-g sample of oxalic acid, H2C2O4, was...Ch. 4 - Prob. 4.113QPCh. 4 - An aqueous solution contains 3.75% NH3 (ammonia)...Ch. 4 - A barium mineral was dissolved in hydrochloric...Ch. 4 - Bone was dissolved in hydrochloric acid, giving...Ch. 4 - Prob. 4.117QPCh. 4 - An antacid tablet has calcium carbonate as the...Ch. 4 - A sample of CuSO45H2O was heated to 110C, where it...Ch. 4 - Prob. 4.120QPCh. 4 - A water-soluble compound of gold and chlorine is...Ch. 4 - A solution of scandium chloride was treated with...Ch. 4 - A 0.608-g sample of fertilizer contained nitrogen...Ch. 4 - An antacid tablet contains sodium hydrogen...Ch. 4 - You order a glass of juice in a restaurant, only...Ch. 4 - Prob. 4.126QPCh. 4 - Prob. 4.127QPCh. 4 - Prob. 4.128QPCh. 4 - Zinc acetate is sometimes prescribed by physicians...Ch. 4 - Arsenic acid, H3AsO4, is a poisonous acid that has...Ch. 4 - When the following equation is balanced by the...Ch. 4 - Identify each of the following reactions as being...Ch. 4 - Prob. 4.133QPCh. 4 - Prob. 4.134QPCh. 4 - A 25-mL sample of 0.50 M NaOH is combined with a...Ch. 4 - What is the molarity of pure water with a density...Ch. 4 - Prob. 4.137QPCh. 4 - How many grams of precipitate are formed if 175 mL...Ch. 4 - Prob. 4.139QPCh. 4 - Potassium hydrogen phthalate (abbreviated as KHP)...Ch. 4 - Lead(II) nitrate reacts with cesium sulfate in an...Ch. 4 - Silver nitrate reacts with strontium chloride in...Ch. 4 - Elemental bromine is the source of bromine...Ch. 4 - Prob. 4.144QPCh. 4 - Prob. 4.145QPCh. 4 - Prob. 4.146QPCh. 4 - Iron forms a sulfide with the approximate formula...Ch. 4 - A transition metal X forms an oxide of formula...Ch. 4 - What volume of a solution of ethanol, C2H6O, that...Ch. 4 - What volume of a solution of ethylene glycol,...Ch. 4 - A 10.0-mL sample of potassium iodide solution was...Ch. 4 - A 25.0-mL sample of sodium sulfate solution was...Ch. 4 - A metal, M, was converted to the sulfate,...Ch. 4 - A metal, M, was converted to the chloride MCl2....Ch. 4 - Phosphoric acid is prepared by dissolving...Ch. 4 - Iron(III) chloride can be prepared by reacting...Ch. 4 - An alloy of aluminum and magnesium was treated...Ch. 4 - An alloy of iron and carbon was treated with...Ch. 4 - Determine the volume of sulfuric acid solution...Ch. 4 - Determine the volume of sodium hydroxide solution...Ch. 4 - The active ingredients of an antacid tablet...Ch. 4 - The active ingredients in an antacid tablet...Ch. 4 - Prob. 4.163QP
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