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: Cengage Learning
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Textbook Question
Chapter 4, Problem 4.14QP
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
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General Chemistry - Standalone book (MindTap Course List)
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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- Write the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forwardAn aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.arrow_forwardWhat is the solid that precipitates, and how much of it forms, when an excess of sodium chloride solution is mixed with 10.0 mL of a 2.10 M silver nitrate solution?arrow_forward
- The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.arrow_forwardOn the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.arrow_forwardHow many grams of precipitate are formed if 175 mL of a 0.750 M aluminum sulfate solution and 375 mL of a 1.15 M sodium hydroxide solution are mixed together?arrow_forward
- Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?arrow_forwardOne method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?arrow_forward
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