General, Organic, & Biological Chemistry
3rd Edition
ISBN: 9780073511245
Author: Janice Gorzynski Smith Dr.
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 9, Problem 9.42P
Which of the following species can be Brønsted—Lowry acids?
a.
b.
c.
d.
e.
f.
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Chapter 9 Solutions
General, Organic, & Biological Chemistry
Ch. 9.1 - Name each acid: (a)HF;(b)HNO3;(c)HCN.Ch. 9.1 - If the polyatomic anion C1O2- is called chlorite,...Ch. 9.1 - Which of the following species can be...Ch. 9.1 - Which of the following species can be...Ch. 9.1 - Classify each reactant as a Brønsted-Lowry acid or...Ch. 9.2 - Determine the conjugate acid of each species:...Ch. 9.2 - Determine the conjugate base of each species:...Ch. 9.2 - Draw the structure of the conjugate base of each...Ch. 9.2 - Label the acid and the base and the conjugate acid...Ch. 9.2 - Ammonia, NH3, is amphoteric. Draw the conjugate...
Ch. 9.2 - Prob. 9.11PCh. 9.3 - Diagrams represent three acids (HA) dissolved in...Ch. 9.3 - Label the stronger acid in each pair. Which acid...Ch. 9.3 - Are the reactants or products favored at...Ch. 9.3 - If lactic acid is similar in strength to acetic...Ch. 9.4 - Rank the acids in each group in order of...Ch. 9.4 - Use the acid dissociation constants in Table 9.3...Ch. 9.4 - Consider the weak acids, HCN and H2CO3. Which acid...Ch. 9.5 - Calculate the value of [OH-] from the given [H3O+]...Ch. 9.5 - Calculate the value of [H3O+] from the given [OH-]...Ch. 9.5 - Calculate the value of [H3O+] and [H3O-] in each...Ch. 9.6 - Convert each H3O+ concentration to a pH value. a....Ch. 9.6 - What H3O+ concentration corresponds to each pH...Ch. 9.6 - Prob. 9.24PCh. 9.6 - Convert each H3O+ concentration to a pH value....Ch. 9.6 - Prob. 9.26PCh. 9.7 - Write a balanced equation for each acid-base...Ch. 9.7 - Prob. 9.28PCh. 9.7 - The acid in acid rain is generally sulfuric acid...Ch. 9.7 - Write a balanced equation for the reaction of...Ch. 9.8 - Determine whether each salt forms an acidic,...Ch. 9.8 - Which of the following salts forms an aqueous...Ch. 9.9 - What is the molarity of an HCI solution if 25.5 mL...Ch. 9.9 - How many milliliters of 2.0MNaOH are needed to...Ch. 9.10 - Determine whether a solution containing each of...Ch. 9.10 - Consider a buffer prepared from the weak acid HCO3...Ch. 9.10 - Calculate the pH of a dihydrogen...Ch. 9.10 - What is the pH of a buffer that contains...Ch. 9 - Which of the following species can be...Ch. 9 - Which of the following species can be...Ch. 9 - Prob. 9.41PCh. 9 - Which of the following species can be...Ch. 9 - Prob. 9.43PCh. 9 - Draw the conjugate acid of each base. a. Br- b....Ch. 9 - Draw the conjugate base of each acid. HNO2 NH4+...Ch. 9 - Draw the conjugate base of each acid. H3O+ H2Se...Ch. 9 - Prob. 9.47PCh. 9 - Prob. 9.48PCh. 9 - Prob. 9.49PCh. 9 - Prob. 9.50PCh. 9 - Label the conjugate acid-base pairs in each...Ch. 9 - Label the conjugate acid-base pairs in each...Ch. 9 - Prob. 9.53PCh. 9 - Prob. 9.54PCh. 9 - Fill in the missing product in each acid-base...Ch. 9 - Fill in the missing product in each acid-base...Ch. 9 - Prob. 9.57PCh. 9 - Write the equation for the acid-base reaction that...Ch. 9 - Prob. 9.59PCh. 9 - Which diagram represents what happens when HCN...Ch. 9 - Prob. 9.61PCh. 9 - Prob. 9.62PCh. 9 - Prob. 9.63PCh. 9 - Use the data in and 9.2 and 9.3 to label the...Ch. 9 - Prob. 9.65PCh. 9 - Which acid, A or B, is stronger in each part? a. B...Ch. 9 - Fill in the missing terms (strong or weak) and...Ch. 9 - Fill in the missing terms (strong or weak) and...Ch. 9 - For each pair of acids: [1] Label the stronger...Ch. 9 - For each pair of acids: [1] Label the stronger...Ch. 9 - Prob. 9.71PCh. 9 - Prob. 9.72PCh. 9 - Prob. 9.73PCh. 9 - Label the acid in the reactants and the conjugate...Ch. 9 - Calculate the value of [OH-] from the given and...Ch. 9 - Calculate the value of [OH-] from the given [H3O+]...Ch. 9 - Calculate the value of [OH-] from the given [HO-]...Ch. 9 - Calculate the value of [H3O+] from the given [OH-]...Ch. 9 - Prob. 9.79PCh. 9 - Prob. 9.80PCh. 9 - Prob. 9.81PCh. 9 - Complete the following table with the needed...Ch. 9 - Prob. 9.83PCh. 9 - Prob. 9.84PCh. 9 - Prob. 9.85PCh. 9 - If pancreaticfluids have a pH of 8.2, calculate...Ch. 9 - Calculate the concentrations of H3O+ and OH in the...Ch. 9 - Prob. 9.88PCh. 9 - Prob. 9.89PCh. 9 - Prob. 9.90PCh. 9 - Prob. 9.91PCh. 9 - Prob. 9.92PCh. 9 - Write a balanced equation for each reaction. a....Ch. 9 - Prob. 9.94PCh. 9 - Prob. 9.95PCh. 9 - Prob. 9.96PCh. 9 - Prob. 9.97PCh. 9 - Prob. 9.98PCh. 9 - Prob. 9.99PCh. 9 - Prob. 9.100PCh. 9 - Whatisthe molarityofanaceticacid (CH3COOH)...Ch. 9 - What is the molarity of an H2SO4 solution if 18.5...Ch. 9 - How many milliliters of 1.0MNaOH solution are...Ch. 9 - How many milliliters of 2.0MNaOH solution are...Ch. 9 - Prob. 9.105PCh. 9 - Prob. 9.106PCh. 9 - Prob. 9.107PCh. 9 - Prob. 9.108PCh. 9 - Prob. 9.109PCh. 9 - Prob. 9.110PCh. 9 - Using the Ka values in Table9.6, calculate the pH...Ch. 9 - Using the Ka values in Table9.6, calculate the pH...Ch. 9 - Calculate the pH of an acetic acid/acetate buffer...Ch. 9 - Calculate the pH of a bicarbonate/carbonate buffer...Ch. 9 - Why is the pH of unpolluted rainwater lower than...Ch. 9 - Prob. 9.116PCh. 9 - Prob. 9.117PCh. 9 - A sample of rainwater has a pH of 4.18. Calculate...Ch. 9 - Prob. 9.119PCh. 9 - Prob. 9.120PCh. 9 - Prob. 9.121PCh. 9 - Prob. 9.122PCh. 9 - Prob. 9.123CPCh. 9 - Prob. 9.124CP
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- Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.arrow_forwardAccording to the Brønsted-Lowry theory, which of the following would you expect to act as an acid? Which as a base? Both acid and base? (a) CHO2- (b) NH4+ (c) HSO3-arrow_forwardClassify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous solution. a. HNO2 b. HNO3 c. CH3NH2 d. NaOH e. NH3 f. HF g. h. Ca(OH)2 i. H2SO4arrow_forward
- Which of each pair of acids is stronger? Why? (a) HClO3, HClO4 (b) H2S, H2Searrow_forwardWhich of the following substances are acids in terms of the Arrhenius concept? Which are bases? Show the acid or base character by using chemical equations. a P4O10 b Na2O c N2H4 d H2Tearrow_forwardWrite the reaction and the corresponding Kb equilibrium expression for each of the following substances acting as bases in water. a. NH3 b. C5H5Narrow_forward
- Write equations that show H2PO4- acting both as an acid and as a base.arrow_forwardWhich of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH] > 1.0 X IO’7Marrow_forwardUsing your results from Exercise 133, place the species in each of the following groups in order of increasing base strength. a. OH, SH, SeH b. NH3, PH3 c. NH3, HONH2arrow_forward
- Determine whether aqueous solutions of the following salts are acidic, basic, or neutral: (a) Al(NO3)3. (b) RbI. (c) KHCO2. (d) CH3NH3Brarrow_forwardTo measure the relative strengths of bases stronger than OH, it is necessary to choose a solvent that is a weaker acid than water. One such solvent is liquid ammonia. (a) Write a chemical equation for the autoionization of ammonia. (b) What is the strongest acid and base that can exist in liquid ammonia? (c) Will a solution of HCI in liquid ammonia be a strong electrical conductor, a weak conductor, or a nonconductor? (d) Oxide ion (O2) is a stronger base than the amide ion (NH2). Write an equation for the reaction of O2 with NH3 in liquid ammonia. Will the equilibrium favor products or reactants?arrow_forward12.63 For each of the following reactions, indicate the Bronsted-Lowrv acids and bases. What are the conjugate acid-base pairs? CN’(aq) + H2O(€) «=* HCN(aq) + OH’(aq) HCO}-(aq) + H,o+(aq) +* H2CO,(aq) + H,O(€) (C) CH,CtX)H(aq) + HS~(aq)i=i CH}COO"(aq) + H2S(aq)arrow_forward
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