CHEMISTRY-TEXT
8th Edition
ISBN: 9780134856230
Author: Robinson
Publisher: PEARSON
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Chapter 16, Problem 16.30A
For the following Lewis acid— base reaction, draw electron-dot structures for the reactants and products, and use the curved arrow notation to represent the donation of a lone pair of electrons from the Lewis base to the Lewis acid.
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Chapter 16 Solutions
CHEMISTRY-TEXT
Ch. 16 - Write a balanced equation for the dissociation of...Ch. 16 - Write the reaction between the carbonate ion...Ch. 16 - Conceptual PRACTICE 15.3 For the following...Ch. 16 - Conceptual APPLY 15.4 For the following reactions...Ch. 16 - If you mix equal concentrations of reactants and...Ch. 16 - Conceptual APPLY 15.6 The following pictures...Ch. 16 - Which pair has the stronger acid listed first? H2S...Ch. 16 - Which acid is stronger, H3PO4orH3AsO4?Ch. 16 - PRACTICE 15.9 The concentration of H3O+ ions in...Ch. 16 - Calculate the pH of a sample of seawater that has...
Ch. 16 - During mining operations, the mineral pyrite...Ch. 16 - Calculate the concentrations of H3O+ and OH- in a...Ch. 16 - Calculate the pH of the following solutions: (a)...Ch. 16 - Calculate the pH of a solution prepared by...Ch. 16 - The following pictures represent aqueous solutions...Ch. 16 - Acetic acid, CH3CO2H, is the solute that gives...Ch. 16 - Wha concentration of formic acid will result in a...Ch. 16 - Calculate the pH and the concentration of all...Ch. 16 - Carbonated drinks are prepared by dissolving CO2...Ch. 16 - Calculate the pH and the concentrations of all...Ch. 16 - Lactated Ringers solution is given intravenously...Ch. 16 - Prob. 16.25PCh. 16 - The following pictures represent aqueous solutions...Ch. 16 - Predict whether a solution of 0.20 M NaNO2 is...Ch. 16 - Calculate the pH and percent dissociation of...Ch. 16 - Prob. 16.29PCh. 16 - For the following Lewis acid— base reaction, draw...Ch. 16 - What are the chemical formulas and names of the...Ch. 16 - What were the average pH ranges for rainfall in...Ch. 16 - Prob. 16.33PCh. 16 - (a) Natural or “unpolluted” rain has a pH of 5.6....Ch. 16 - Prob. 16.35PCh. 16 - Prob. 16.36PCh. 16 - Because sulfur and nitrogen oxides are the main...Ch. 16 - Prob. 16.38CPCh. 16 - The following pictures represent aqueous solutions...Ch. 16 - Locate sulfur, selenium, chlorine, and bromine in...Ch. 16 - Prob. 16.41CPCh. 16 - Prob. 16.42CPCh. 16 - The followign pictures represent solutions of...Ch. 16 - Prob. 16.44CPCh. 16 - Look at the electron-dot structures of the...Ch. 16 - Boric acid (H3BO3) is a weak monoprotic acid that...Ch. 16 - Prob. 16.47CPCh. 16 - Prob. 16.48SPCh. 16 - Which of the following can behave both as a...Ch. 16 - Give the formula for the conjugate base of each of...Ch. 16 - Give the formula for the conjugate acid of each of...Ch. 16 - For each of the following reactions, identify the...Ch. 16 - For each of the following reactions, identify the...Ch. 16 - Aqueous solutions of hydrogen sulfide contain...Ch. 16 - Prob. 16.55SPCh. 16 - Choose from the conjugate acid-base pairs...Ch. 16 - Prob. 16.57SPCh. 16 - Prob. 16.58SPCh. 16 - Prob. 16.59SPCh. 16 - Arrange each group of compounds in order of...Ch. 16 - Arrange each group of compounds in order of...Ch. 16 - Prob. 16.62SPCh. 16 - Identify the weakest acid in each of the following...Ch. 16 - Prob. 16.64SPCh. 16 - Identify the stronger base in each of the...Ch. 16 - Prob. 16.66SPCh. 16 - Prob. 16.67SPCh. 16 - The concentration of OH- in a sample of seawater...Ch. 16 - The concentration of OH- in human blood is...Ch. 16 - For each of the following solutions, calculate...Ch. 16 - For each of the following solutions, calculate...Ch. 16 - Water superheated under pressure to 200oC and 750...Ch. 16 - Water at 500oC and 250 atm is a supercritical...Ch. 16 - Calculate the pH to the correct number of...Ch. 16 - Calculate the pH to the correct number of...Ch. 16 - Calculate the H3O+ concentration to the correct...Ch. 16 - Calculate the H3O+ concentration to the correct...Ch. 16 - Prob. 16.78SPCh. 16 - Which of the indicators given in Figure 16.5,...Ch. 16 - Which of the following species behave a strong...Ch. 16 - Which of the following species behave as strong...Ch. 16 - Calculate the pH of the following solutions:...Ch. 16 - Calculate the pH of the following solutions: 0.48...Ch. 16 - Prob. 16.84SPCh. 16 - Calculate the pH of solutions prepared by: RAN (a)...Ch. 16 - How many grams of CaO should be dissolved in...Ch. 16 - Prob. 16.87SPCh. 16 - Look up the value of Ka in Appendix C for...Ch. 16 - Look up the value of Ka in Appendix C for...Ch. 16 - The pH of 0.040 M hypobromous acid (HOBr) is 5.05....Ch. 16 - Lactic acid (C3H6O3) , which occurs in sour milk...Ch. 16 - The pH of 0.050 M gallic acid, an acid found in...Ch. 16 - The pH of 0.040 M pyruvic acid, an acid found in...Ch. 16 - A vitamin C tablet containing 250 mg of ascorbic...Ch. 16 - Acetic acid (CH3COOH;Ka=1.810-5) has a...Ch. 16 - Acrylic acid (HC3H3O2) is used in the manufacture...Ch. 16 - Hippuric acid (HC9H8NO3) , found in horse urine,...Ch. 16 - Calculat the pH and the percent dissociation in...Ch. 16 - A typical aspirin tablet contains 324 mg of...Ch. 16 - Prob. 16.100SPCh. 16 - Calculate the percent dissociation of...Ch. 16 - Write balanced net ionic equations and the...Ch. 16 - Write balanced net ionic equations and the...Ch. 16 - Calculate the pH and the concentrations of all...Ch. 16 - Prob. 16.105SPCh. 16 - Prob. 16.106SPCh. 16 - Tartaric acid (C4H6O6) is a diprotic acid that...Ch. 16 - Like sulfuric acid, selenic acid (H2SeO4) is a...Ch. 16 - Calculate the concentrations of H3O+ and SO42- in...Ch. 16 - Prob. 16.110SPCh. 16 - Prob. 16.111SPCh. 16 - Write a balanced net ionic equation and the...Ch. 16 - Write a balanced net ionic equation and the...Ch. 16 - Styrchine (C21H22N2O2) , a deadly poison used for...Ch. 16 - What is the pH of 0.5 M ammonia (NH3)?(Kb=1.8105)Ch. 16 - Morphine (C17H19NO3), a narcotic used in...Ch. 16 - A 1.00103M solution of quinine, a drug used in...Ch. 16 - Oxycodone (C18H21NO4), a narcotic analgesic, is a...Ch. 16 - Morpholine (C4H9NO) is a weak organic base with...Ch. 16 - Using values of Kb in Appendix C, calculate values...Ch. 16 - Using values of Ka in Appendix C, calculate values...Ch. 16 - Prob. 16.122SPCh. 16 - Sodium benzoate (C6H5CO2Na) is used as a food...Ch. 16 - Write a balanced net ionic equation for the...Ch. 16 - Write a balanced net ioflk equation for the...Ch. 16 - Classify each of the following ions according to...Ch. 16 - Classify each of the following salt solutions as...Ch. 16 - Calculate the concentrations of all species...Ch. 16 - Prob. 16.129SPCh. 16 - Calculate Ka for the cation Kb for the anion in an...Ch. 16 - Classify each of the following salt solutions as...Ch. 16 - Prob. 16.132SPCh. 16 - Classify each of the following salt solutions as...Ch. 16 - Calculate the pH and the concentrations of all...Ch. 16 - Calculate the pH and the percent dissociation of...Ch. 16 - Prob. 16.136SPCh. 16 - Prob. 16.137SPCh. 16 - Prob. 16.138SPCh. 16 - For each of the following reactions, identify the...Ch. 16 - Prob. 16.140SPCh. 16 - For each of the Lewis acid—base reactions in...Ch. 16 - Prob. 16.142SPCh. 16 - Prob. 16.143SPCh. 16 - Prob. 16.144MPCh. 16 - Prob. 16.145MPCh. 16 - Prob. 16.146MPCh. 16 - Prob. 16.147MPCh. 16 - Normal rain has a pH of 5.6 due to dissolved...Ch. 16 - Sulfur dioxide is quite soluble in water:...Ch. 16 - Prob. 16.150MPCh. 16 - Acid and base behavior can be observed in solvents...Ch. 16 - Prob. 16.152MPCh. 16 - In the case of very weak acids, [H3O+] from the...Ch. 16 - Prob. 16.154MPCh. 16 - Prob. 16.155MPCh. 16 - Neutralization reactions involving either a strong...Ch. 16 - Prob. 16.157MPCh. 16 - Prob. 16.158MPCh. 16 - A 200.0 mL sample of 0.350 M acetic acid (CH3CO2H)...Ch. 16 - Prob. 16.160MP
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- In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()arrow_forwardIonization 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_forwardIn each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()arrow_forward
- Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forwardHydrazine, N2H4 (having the structure H2NNH2), and its derivatives have been used as rocket fuels. Draw the Lewis electron-dot formula for the hydrazine molecule. Describe the geometries expected about the nitrogen atoms in this molecule. Why would you expect hydrazine to be basic? Which substance, NH3 or N2H4, would you expect to be more basic? Why? Write the chemical equation in which hydrazine reacts with hydrochloric acids to form the salt N2H5Cl. Consider the positive ion of this salt. How does its basic character compare with that of NH3 and N2H4? Explain.arrow_forwardTable 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.arrow_forward
- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardWrite chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2CO3 (carbonic acid) b. H2C3H2O4 (malonic acid)arrow_forwardStudents are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2arrow_forward
- Write the base ionization constant expression for the ionization of each of the following bases. In each case, the nitrogen atom accepts the proton. a. CH3NH2 (methylamine) b. C2H5NH2 (ethylamine)arrow_forwardConsider 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_forwardUsing the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?arrow_forward
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