CHEMISTRY:ATOMS FIRST-2 YEAR CONNECT
2nd Edition
ISBN: 9781260592320
Author: Burdge
Publisher: MCG
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Chapter 16, Problem 16.101QP
In a certain experiment, a student finds that the pH values of 0.10-M solutions of three potassium salts KX, KY, and KZ are 7.0, 9.0, and 11.0, respectively. Arrange the acids HX, HY, and HZ in order of increasing acid strength.
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Chapter 16 Solutions
CHEMISTRY:ATOMS FIRST-2 YEAR CONNECT
Ch. 16.1 - What is (a) the conjugate base of HNO3, (b) the...Ch. 16.1 - What is (a) the conjugate acid of ClO4, (b) the...Ch. 16.1 - HSO3 is the conjugate acid of what species? HSO3...Ch. 16.1 - Which of the models represents a species that has...Ch. 16.1 - Prob. 16.2WECh. 16.1 - Identify and label the species in each reaction....Ch. 16.1 - Prob. 2PPBCh. 16.1 - Write the formula and charge for each species in...Ch. 16.1 - Prob. 16.1.1SRCh. 16.1 - Prob. 16.1.2SR
Ch. 16.2 - Predict the relative strengths of the oxoacids in...Ch. 16.2 - Prob. 3PPACh. 16.2 - Based on the information in this section, which is...Ch. 16.2 - Prob. 3PPCCh. 16.2 - Prob. 16.2.1SRCh. 16.2 - Prob. 16.2.2SRCh. 16.2 - Prob. 16.2.3SRCh. 16.3 - Prob. 16.4WECh. 16.3 - The concentration of hydroxide ions in the antacid...Ch. 16.3 - The value of Kw at normal body temperature (37C)...Ch. 16.3 - Prob. 4PPCCh. 16.3 - Prob. 16.3.1SRCh. 16.3 - Prob. 16.3.2SRCh. 16.4 - Determine the pOH of a solution at 25C in which...Ch. 16.4 - Determine the pOH of a solution at 25C in which...Ch. 16.4 - Determine the pOH of a solution at 25C in which...Ch. 16.4 - Prob. 5PPCCh. 16.4 - Calculate the hydroxide ion concentration in a...Ch. 16.4 - Prob. 6PPACh. 16.4 - Prob. 6PPBCh. 16.4 - Prob. 6PPCCh. 16.4 - Prob. 16.4.1SRCh. 16.4 - Prob. 16.4.2SRCh. 16.4 - Prob. 16.4.3SRCh. 16.4 - Prob. 16.4.4SRCh. 16.5 - Calculate the pH of an aqueous solution at 25C...Ch. 16.5 - Prob. 7PPACh. 16.5 - Prob. 7PPBCh. 16.5 - Prob. 7PPCCh. 16.5 - Prob. 16.8WECh. 16.5 - Calculate the concentration of HNO3 in a solution...Ch. 16.5 - Prob. 8PPBCh. 16.5 - Which of the plots [(i)(iv)] best approximates the...Ch. 16.5 - Prob. 16.9WECh. 16.5 - Prob. 9PPACh. 16.5 - Prob. 9PPBCh. 16.5 - Prob. 9PPCCh. 16.5 - Prob. 16.10WECh. 16.5 - Prob. 10PPACh. 16.5 - Prob. 10PPBCh. 16.5 - Prob. 10PPCCh. 16.5 - Prob. 16.5.1SRCh. 16.5 - Prob. 16.5.2SRCh. 16.5 - Prob. 16.5.3SRCh. 16.5 - Prob. 16.5.4SRCh. 16.5 - Prob. 16.5.5SRCh. 16.5 - Prob. 16.5.6SRCh. 16.5 - Prob. 16.5.7SRCh. 16.6 - The Ka of hypochlorous acid (HClO) is 3.5 108....Ch. 16.6 - Calculate the pH at 25C of a 0.18-M solution of a...Ch. 16.6 - Prob. 11PPBCh. 16.6 - The diagrams show solutions of four different weak...Ch. 16.6 - Determine the pH and percent ionization for acetic...Ch. 16.6 - Determine the pH and percent ionization for...Ch. 16.6 - At what concentration does hydrocyanic acid...Ch. 16.6 - Prob. 12PPCCh. 16.6 - Aspirin (acetylsalicylie acid, HC9H7O4) is a weak...Ch. 16.6 - Prob. 13PPACh. 16.6 - Prob. 13PPBCh. 16.6 - Calculate Ka values (to two significant figures)...Ch. 16.6 - Prob. 16.6.1SRCh. 16.6 - Prob. 16.6.2SRCh. 16.6 - Prob. 16.6.3SRCh. 16.7 - Prob. 16.14WECh. 16.7 - Calculate the pH at 25C of a 0.0028-M solution of...Ch. 16.7 - Prob. 14PPBCh. 16.7 - The diagrams represent solutions of three...Ch. 16.7 - Caffeine, the stimulant in coffee and tea, is a...Ch. 16.7 - Prob. 15PPACh. 16.7 - Prob. 15PPBCh. 16.7 - Prob. 15PPCCh. 16.7 - Prob. 16.7.1SRCh. 16.7 - Prob. 16.7.2SRCh. 16.7 - Prob. 16.7.3SRCh. 16.8 - Prob. 16.16WECh. 16.8 - Prob. 16PPACh. 16.8 - Prob. 16PPBCh. 16.8 - Prob. 16PPCCh. 16.8 - Prob. 16.8.1SRCh. 16.8 - Prob. 16.8.2SRCh. 16.8 - Prob. 16.8.3SRCh. 16.9 - Oxalic acid (H2C2O4) is a poisonous substance used...Ch. 16.9 - Calculate the concentrations of H2C2O4, HC2O4,...Ch. 16.9 - Calculate the concentrations of H2SO4, HSO4, SO42,...Ch. 16.9 - Prob. 17PPCCh. 16.9 - Prob. 16.9.1SRCh. 16.9 - Prob. 16.9.2SRCh. 16.9 - Prob. 16.9.3SRCh. 16.10 - Prob. 16.18WECh. 16.10 - Determine the pH of a 0.15-M solution of sodium...Ch. 16.10 - Prob. 18PPBCh. 16.10 - Winch of the graphs [(i)(iv)] best represents the...Ch. 16.10 - Calculate the pH of a 0.10-M solution of ammonium...Ch. 16.10 - Determine the pH of a 0.25-M solution of...Ch. 16.10 - Prob. 19PPBCh. 16.10 - Prob. 19PPCCh. 16.10 - Predict whether a 0.10-M solution of each of the...Ch. 16.10 - Predict whether a 0.10-M solution of each of the...Ch. 16.10 - Prob. 20PPBCh. 16.10 - Prob. 20PPCCh. 16.10 - Prob. 16.10.1SRCh. 16.10 - Prob. 16.10.2SRCh. 16.10 - Prob. 16.10.3SRCh. 16.10 - Prob. 16.10.4SRCh. 16.10 - Prob. 16.10.5SRCh. 16.12 - Identify the Lewis acid and Lewis base in each of...Ch. 16.12 - Prob. 21PPACh. 16.12 - Prob. 21PPBCh. 16.12 - Which of the diagrams best depicts the combination...Ch. 16.12 - Prob. 16.12.1SRCh. 16.12 - Prob. 16.12.2SRCh. 16 - F or a species to act as a Brnsted base, an atom...Ch. 16 - Identify the acid-base conjugate pairs in each of...Ch. 16 - Prob. 16.3QPCh. 16 - Prob. 16.4QPCh. 16 - Write the formulas of the conjugate bases of the...Ch. 16 - Prob. 16.6QPCh. 16 - Prob. 16.7QPCh. 16 - List four factors that affect the strength of an...Ch. 16 - Prob. 16.9QPCh. 16 - Prob. 16.10QPCh. 16 - Prob. 16.11QPCh. 16 - Prob. 16.12QPCh. 16 - Prob. 16.13QPCh. 16 - Write the equilibrium expression for the...Ch. 16 - Write an equation relating [H+] and [OH] in...Ch. 16 - Write an equation relating [H+] and [OH] in...Ch. 16 - Prob. 16.17QPCh. 16 - Prob. 16.18QPCh. 16 - Prob. 16.19QPCh. 16 - Prob. 16.20QPCh. 16 - Prob. 16.21QPCh. 16 - Prob. 16.22QPCh. 16 - Prob. 16.23QPCh. 16 - Calculate the concentration of H+ ions in a 0.62 M...Ch. 16 - Calculate the concentration of OH ions in a 1.4 ...Ch. 16 - Calculate the pH of each of the following...Ch. 16 - Calculate the pH of each of the following...Ch. 16 - Prob. 16.28QPCh. 16 - Prob. 16.29QPCh. 16 - Prob. 16.30QPCh. 16 - How much NaOH (in grams) is needed to prepare 546...Ch. 16 - Prob. 16.32QPCh. 16 - Why are ionizations of strong acids and strong...Ch. 16 - Prob. 16.34QPCh. 16 - Prob. 16.35QPCh. 16 - Prob. 16.36QPCh. 16 - Prob. 16.37QPCh. 16 - Prob. 16.38QPCh. 16 - Prob. 16.39QPCh. 16 - Prob. 16.40QPCh. 16 - Prob. 16.41QPCh. 16 - Prob. 16.42QPCh. 16 - Prob. 16.43QPCh. 16 - Prob. 16.1VCCh. 16 - Prob. 16.2VCCh. 16 - Prob. 16.3VCCh. 16 - Prob. 16.4VCCh. 16 - Prob. 16.44QPCh. 16 - Prob. 16.45QPCh. 16 - Prob. 16.46QPCh. 16 - Why do we normally not quote Ka values for strong...Ch. 16 - Why is it necessary to specify temperature when...Ch. 16 - Which of the following solutions has the highest...Ch. 16 - Prob. 16.50QPCh. 16 - The Ka for benzoic acid is 6.5 105. Calculate the...Ch. 16 - Calculate the pH of an aqueous solution at 25C...Ch. 16 - Calculate the pH of an aqueous solution at 25C...Ch. 16 - Determine the percent ionization of the following...Ch. 16 - Determine the percent ionization of the following...Ch. 16 - Prob. 16.56QPCh. 16 - A 0.015-M solution of a monoprotic acid is 0.92%...Ch. 16 - Prob. 16.58QPCh. 16 - Prob. 16.59QPCh. 16 - Prob. 16.60QPCh. 16 - Prob. 16.61QPCh. 16 - Prob. 16.62QPCh. 16 - In biological and medical applications, it is...Ch. 16 - Classify each of the following species as a weak...Ch. 16 - Prob. 16.65QPCh. 16 - Prob. 16.66QPCh. 16 - Prob. 16.67QPCh. 16 - Which of the following has a higher pH: (a) 1.0 M...Ch. 16 - Prob. 16.69QPCh. 16 - Prob. 16.70QPCh. 16 - Prob. 16.71QPCh. 16 - What is the original molarity of an aqueous...Ch. 16 - Prob. 16.73QPCh. 16 - Prob. 16.74QPCh. 16 - Prob. 16.75QPCh. 16 - Prob. 16.76QPCh. 16 - Prob. 16.77QPCh. 16 - Calculate Ka for each of the following ions: NH4+,...Ch. 16 - The following diagrams represent aqueous solutions...Ch. 16 - Prob. 16.80QPCh. 16 - Write all the species (except water) that are...Ch. 16 - Write the Ka1 and Ka2 expressions for sulfurous...Ch. 16 - Prob. 16.83QPCh. 16 - Prob. 16.84QPCh. 16 - Prob. 16.85QPCh. 16 - Prob. 16.86QPCh. 16 - Calculate the pH at 25C of a 0.25-M aqueous...Ch. 16 - The first and second ionization constants of a...Ch. 16 - Prob. 16.89QPCh. 16 - Prob. 16.90QPCh. 16 - Explain why small, highly charged metal ions are...Ch. 16 - Prob. 16.92QPCh. 16 - Specify which of the following salts will undergo...Ch. 16 - Prob. 16.94QPCh. 16 - Calculate the pH of a 0.42 M NH4Cl solution. (Kb...Ch. 16 - Calculate the pH of a 0.082 M NaF solution. (Ka...Ch. 16 - Calculate the pH of a 0.91 M C2H5NH3I solution....Ch. 16 - Prob. 16.98QPCh. 16 - Predict whether the following solutions are...Ch. 16 - Prob. 16.100QPCh. 16 - In a certain experiment, a student finds that the...Ch. 16 - Prob. 16.102QPCh. 16 - Prob. 16.103QPCh. 16 - Classify the following oxides as acidic, basic,...Ch. 16 - Prob. 16.105QPCh. 16 - Explain why metal oxides tend to be basic if the...Ch. 16 - Arrange the oxides in each of the following groups...Ch. 16 - Prob. 16.108QPCh. 16 - Prob. 16.109QPCh. 16 - Prob. 16.110QPCh. 16 - Prob. 16.111QPCh. 16 - Prob. 16.112QPCh. 16 - In terms of orbitals and electron arrangements,...Ch. 16 - Prob. 16.114QPCh. 16 - Prob. 16.115QPCh. 16 - Which would be considered a stronger Lewis acid:...Ch. 16 - Prob. 16.117QPCh. 16 - Identify the Lewis acid and the Lewis base in the...Ch. 16 - Identify the Lewis acid and the Lewis base in the...Ch. 16 - Prob. 16.120QPCh. 16 - Prob. 16.121QPCh. 16 - Prob. 16.122QPCh. 16 - Prob. 16.123QPCh. 16 - Prob. 16.124QPCh. 16 - Calculate the pH and percent ionization of a 0.88...Ch. 16 - Prob. 16.126QPCh. 16 - Prob. 16.127QPCh. 16 - The pH of a 0.0642-M solution of a monoprotic acid...Ch. 16 - Prob. 16.129QPCh. 16 - HA and HB are both weak acids although HB is the...Ch. 16 - Prob. 16.131QPCh. 16 - Prob. 16.132QPCh. 16 - Use the data in Table 16.5 to calculate the...Ch. 16 - Prob. 16.134QPCh. 16 - Most of the hydrides of Group 1A and Group 2 A...Ch. 16 - Prob. 16.136QPCh. 16 - Novocaine, used as a local anesthetic by dentists,...Ch. 16 - Which of the following is the stronger base: NF3...Ch. 16 - Prob. 16.139QPCh. 16 - The ion product of D20 is 1.35 1015 at 25C. (a)...Ch. 16 - Prob. 16.141QPCh. 16 - Prob. 16.142QPCh. 16 - Prob. 16.143QPCh. 16 - Prob. 16.144QPCh. 16 - Prob. 16.145QPCh. 16 - When the concentration of a strong acid is not...Ch. 16 - Calculate the pH of a 2.00 M NH4CN solution.Ch. 16 - Prob. 16.148QPCh. 16 - Prob. 16.149QPCh. 16 - Prob. 16.150QPCh. 16 - Prob. 16.151QPCh. 16 - Hydrocyanic acid (HCN) is a weak acid and a deadly...Ch. 16 - How many grams of NaCN would you need to dissolve...Ch. 16 - Prob. 16.154QPCh. 16 - Calculate the pH of a 1-L solution containing...Ch. 16 - Prob. 16.156QPCh. 16 - You are given two beakers, one containing an...Ch. 16 - Use Le Chteliers principle to predict the effect...Ch. 16 - A 0.400 M formic acid (HCOOH) solution freezes at...Ch. 16 - The disagreeable odor of fish is mainly due to...Ch. 16 - Prob. 16.161QPCh. 16 - Prob. 16.162QPCh. 16 - Both the amide ion (NH2) and the nitride ion (N3)...Ch. 16 - When carbon dioxide is bubbled through a clear...Ch. 16 - Explain the action of smelling salt, which is...Ch. 16 - About half of the hydrochloric acid produced...Ch. 16 - Which of the following does not represent a Lewis...Ch. 16 - Determine whether each of the following statements...Ch. 16 - How many milliliters of a strong monoprotic acid...Ch. 16 - Hemoglobin (Hb) is a blood protein that is...Ch. 16 - Prob. 16.171QPCh. 16 - Calculate the pH of a solution that is 1.00 M HCN...Ch. 16 - Tooth enamel is largely hydroxyapatite...Ch. 16 - Prob. 16.174QPCh. 16 - Prob. 16.175QPCh. 16 - Prob. 16.176QPCh. 16 - Sulfuric acid (H2SO4) accounts for as much as 80...Ch. 16 - A 1-87-g sample of Mg reacts with 80.0 mL of a HCl...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - Determine pH at the equivalence point in the...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - Determine pH at the equivalence point in the...
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- Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.arrow_forward12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’arrow_forwardAcids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forward
- Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardWrite chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forward
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