Introduction to Chemistry, Special Edition
6th Edition
ISBN: 9781337035934
Author: Cracolice/Peters
Publisher: Cengage Learning
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Chapter 18, Problem 17PE
Interpretation Introduction
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The ratio
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A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C₆H₅NH₃⁺ in the solution. The value of Kb for C₆H₅NH₂ is 3.8 × 10⁻¹⁰.
Also what is the original concentration of C₆H₅NH₃⁺ ?
Calculate the pH of each of the following buffered solutions.
Ka(HC, HgO,)= 1.8 × 10 5
1.0.19 M acetic acid/0.29 M sodium acetate
pH =
2. 0.29 M acetic acid/0.19 M sodium acetate
pH =
3. 0.060 M acetic acid/0.21 M sodium acetate
pH =
4. 0.21 M acetic acid/0.060 M sodium acetate
pH =
Visited
Consider the reaction below. What is the effect on the concentration of ammonia (NH3 ), water (H20) hydroxide ion
(OH"), and ammonium ion (NH+) if OH is added to the reaction?
NH3 (aq) + H2O (1) = NH4* (aq) + OH (aq) K-1.8x1Q-5
The concentration of NH3
The concentration of OH-
The concentration of NHA+
The concentration of H2
increases
decreases
does not change
Chapter 18 Solutions
Introduction to Chemistry, Special Edition
Ch. 18 - Prob. 1ECh. 18 - Prob. 2ECh. 18 - Prob. 3ECh. 18 - Prob. 4ECh. 18 - Prob. 5ECh. 18 - Prob. 6ECh. 18 - Prob. 7ECh. 18 - Prob. 8ECh. 18 - Prob. 9ECh. 18 - Prob. 10E
Ch. 18 - Prob. 11ECh. 18 - Prob. 12ECh. 18 - Prob. 13ECh. 18 - Prob. 14ECh. 18 - Prob. 15ECh. 18 - Prob. 16ECh. 18 - Prob. 17ECh. 18 - Prob. 18ECh. 18 - Prob. 19ECh. 18 - Prob. 20ECh. 18 - Prob. 21ECh. 18 - Prob. 22ECh. 18 - Prob. 23ECh. 18 - Prob. 24ECh. 18 - Prob. 25ECh. 18 - Consider the following system at equilibrium at...Ch. 18 - Prob. 27ECh. 18 - Prob. 28ECh. 18 - Prob. 29ECh. 18 - Prob. 30ECh. 18 - Prob. 31ECh. 18 - Prob. 32ECh. 18 - Prob. 33ECh. 18 - Prob. 34ECh. 18 - Which direction of the equilibrium...Ch. 18 - Prob. 36ECh. 18 - Prob. 37ECh. 18 - Prob. 38ECh. 18 - Prob. 39ECh. 18 - Consider the following system at equilibrium at...Ch. 18 - Prob. 41ECh. 18 - Prob. 42ECh. 18 - Prob. 43ECh. 18 - Prob. 44ECh. 18 - Prob. 45ECh. 18 - Prob. 46ECh. 18 - Prob. 47ECh. 18 - Prob. 48ECh. 18 - Prob. 49ECh. 18 - Prob. 50ECh. 18 - The equilibrium between nitrogen monoxide, oxygen,...Ch. 18 - The equilibrium constant expression for a given...Ch. 18 - Prob. 53ECh. 18 - For the following system, K=4.86105 at 298K:...Ch. 18 - Prob. 55ECh. 18 - Prob. 56ECh. 18 - Prob. 57ECh. 18 - Question 57 and 58: In Chapter 9, we discussed how...Ch. 18 - Prob. 59ECh. 18 - A student measures the molar solubility of...Ch. 18 - Prob. 61ECh. 18 - Prob. 62ECh. 18 - Find the moles per liter and grams per 100mL...Ch. 18 - Prob. 64ECh. 18 - Prob. 65ECh. 18 - Prob. 66ECh. 18 - Prob. 67ECh. 18 - Ksp for silver hydroxide is 2.0108. Calculate the...Ch. 18 - Prob. 69ECh. 18 - Prob. 70ECh. 18 - Prob. 71ECh. 18 - Prob. 72ECh. 18 - Prob. 73ECh. 18 - Prob. 74ECh. 18 - Prob. 75ECh. 18 - Prob. 76ECh. 18 - Prob. 77ECh. 18 - Prob. 78ECh. 18 - Prob. 79ECh. 18 - Classify each of the following statements as true...Ch. 18 - Prob. 81ECh. 18 - Prob. 82ECh. 18 - Prob. 83ECh. 18 - Prob. 84ECh. 18 - Prob. 85ECh. 18 - Prob. 86ECh. 18 - Prob. 87ECh. 18 - Prob. 88ECh. 18 - Prob. 89ECh. 18 - Prob. 90ECh. 18 - Hard water has a high concentration of calcium and...Ch. 18 - Prob. 18.1TCCh. 18 - Prob. 18.3TCCh. 18 - a What happens to a reaction rate as temperature...Ch. 18 - Prob. 18.5TCCh. 18 - Write a brief description of the relationships...Ch. 18 - Prob. 2CLECh. 18 - Prob. 3CLECh. 18 - Prob. 4CLECh. 18 - Prob. 5CLECh. 18 - Prob. 1PECh. 18 - Prob. 2PECh. 18 - Prob. 3PECh. 18 - Prob. 4PECh. 18 - Prob. 5PECh. 18 - Prob. 6PECh. 18 - Prob. 7PECh. 18 - Prob. 8PECh. 18 - Prob. 9PECh. 18 - Prob. 10PECh. 18 - Prob. 11PECh. 18 - Prob. 12PECh. 18 - What is the molar solubility of calcium fluoride...Ch. 18 - Prob. 14PECh. 18 - Prob. 15PECh. 18 - Prob. 16PECh. 18 - Prob. 17PECh. 18 - Prob. 18PECh. 18 - Prob. 19PE
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- Briefly describe how a buffer solution can control the pH of a solution when strong acid is added and when strong base is added. Use NH3/NH4Cl as an example of a buffer and HCl and NaOH as the strong acid and strong base.arrow_forwardFor 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_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forward
- Write 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_forwardThe concentration of acetylcholine (a neurotransmitter) in a sample can be determined from the pH changes that accompany its hydrolysis. When the sample is incubated with the enzyme acetylcholinesterase, acetylcholine is converted to choline and acetic acid, which dissociates to yield acetate and a hydrogen ion. CНз CHз Нао — сHz— CH "N— снз но-сн— сH,-"N-CH; + CH;— с-о+ н* CH3-C-0- сHз CHз Choline Acetylcholine Acetate In a typical analysis, 11 mL of an aqueous solution containing an unknown amount of acetylcholine had a pH of 7.70. When incubated with acetylcholinesterase, the pH of the solution decreased to 6.89. Assuming there was no buffer in the assay mixture, determine the number of moles of acetylcholine in the 11 mL sample.arrow_forwardA buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C₆H₅NH₃⁺ in the solution. The value of Kb for C₆H₅NH₂ is 3.8 × 10⁻¹⁰. Let x equal the original concentration of C₆H₅NH₃⁺ in the water. Based on the values given, set up an ice table to determine the unknown. Based on the ice table, set up the expression of Kb in order to determine the unknown. Do not simplify or combine terms. Based on the ice table and kb expression, determine the original concentration of C₆H₅NH₃⁺.arrow_forward
- You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.arrow_forwardWhat is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride? K, (methylamine) = 4.4 × 10-4arrow_forwardWhich of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M sodium nitrite 0.31 M ammonium bromide + 0.31 M ammonia 0.29 M hydroiodic acid + 0.23 M potassium iodide 0.16 M potassium fluoride + 0.21 M hydrofluoric acid O 0.39 M acetic acid + 0.25 M potassium acetatearrow_forward
- 1) Write the equilibrium constant expression for the dissociation of acetic acid 2) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? 3) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from number 2?arrow_forwardWhich of the following aqueous solutions are good buffer systems? O 0.14 M hypochlorous acid + 0.18 M potassium hypochlorite D0.29 M ammonium bromide + 0.32 M ammonia O 0.37 M nitrous acid + 0.25 M sodium nitrite O 0.17 M sodium cyanide + 0.28 M hydrocyanic acid D0.30 M hydroiodic acid + 0.17 M potassium iodidearrow_forwardC6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C,H,NH2COO, in a 8.0 x 10-2 M solution of the acid. The value of Ka is 2.2 x 10-5. Concentration of hydronium ion = | м Concentration of para-aminobenzoate ion =|| |мarrow_forward
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