Chemistry: The Central Science (14th Edition)
14th Edition
ISBN: 9780134414232
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
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Textbook Question
Chapter 16.6, Problem 16.12.2PE
Practice Exercise 2
The Ka for niacin (Sample Exercise 16.10) is 1.5 X 10-5. What is the pH of a 0.010 M solution of niacin?
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Homework:
Answer the following:
Determine the pH level of a solution that has 0.02372 M of Formic acid, given that the Ka of formic acid is equal to 1.400 x 10-4
What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
(Answer is not 11.16)
Baseline Question: Calculate the pH of a 5.6x10-9M HCl aqueous solution. ANS: pH=6.99
Commentary: Since I know HCl is a strong acid and ionization is 100%, I thought I could find pH as -log(5.6x10-9), however my teacher said that was incorrect . She did a Kw=[OH-][H3O+] to find x. Use image below to see my work. The answer to the question is pH= 6.99.
Actual Question:I want to know why we had to do an ICE table and find "x" (another H3O concentration) instead of -log(5.6x10-9).
Chapter 16 Solutions
Chemistry: The Central Science (14th Edition)
Ch. 16.2 - Practice Exercise 1 Consider the following...Ch. 16.2 - Prob. 16.1.2PECh. 16.2 - Prob. 16.2.1PECh. 16.2 - Practice Exercise 2 When lithium oxide (Li2O) is...Ch. 16.2 - Based on information in Figure 16.4, place the...Ch. 16.2 - Practice Exercise 2 For each reaction, use Figure...Ch. 16.3 - Practice Exercise 1 In a certain acidic solution...Ch. 16.3 - Practice Exercise 2 Indicate whether solutions...Ch. 16.3 - Prob. 16.5.1PECh. 16.3 - Prob. 16.5.2PE
Ch. 16.4 - Practice Exercise 1 A solution at 250C has [OH-] =...Ch. 16.4 - Practice Exercise 2 In a sample of lemon juice,...Ch. 16.4 - Practice Exercise 1 A solution at 25° C has pOH =...Ch. 16.4 - Prob. 16.7.2PECh. 16.5 - Practice Exercise 1 Order the following three...Ch. 16.5 - Prob. 16.8.2PECh. 16.5 - Practice Exercise 1 Order the following three...Ch. 16.5 - Prob. 16.9.2PECh. 16.6 - Prob. 16.10.1PECh. 16.6 - Practice Exercise 2 Niacin, one of the B vitamins,...Ch. 16.6 - Prob. 16.11.1PECh. 16.6 - Practice Exercise 2 A 0.020 M solution of niacin...Ch. 16.6 - Practice Exercise 1 What is the pH of a 0.40 M...Ch. 16.6 - Practice Exercise 2 The Ka for niacin (Sample...Ch. 16.6 - Prob. 16.13.1PECh. 16.6 - Prob. 16.13.2PECh. 16.6 - Practice Exercise 1 What is the pH of a 0.28 M...Ch. 16.6 - Practice Exercise 2 Calculate the pH of a 0.020 M...Ch. 16.7 - Prob. 16.15.1PECh. 16.7 - Practice Exercise 2 Which of the following...Ch. 16.7 - Prob. 16.16.1PECh. 16.7 - Practice Exercise 2 What is the morality of an...Ch. 16.8 - Practice Exercise 1 By using information from...Ch. 16.8 - Practice Exercise 2 Based on information in...Ch. 16.9 - Prob. 16.18.1PECh. 16.9 - Prob. 16.18.2PECh. 16.9 - Practice Exercise 1 How many of the following...Ch. 16.9 - Practice Exercise 2 Predict whether the...Ch. 16.10 - Prob. 16.20.1PECh. 16.10 - In each pair, choose the compound that gives the...Ch. 16 - Prob. 1DECh. 16 - a. Identify the Br ted-Lowry acid and base in the...Ch. 16 - Prob. 2ECh. 16 - Prob. 3ECh. 16 - Prob. 4ECh. 16 - 16.5 The following diagrams represent aqueous...Ch. 16 - Prob. 6ECh. 16 - Which of these statements about how the percent...Ch. 16 - 16.8 Each of the three molecules shown here...Ch. 16 - Prob. 9ECh. 16 - Which of the following diagrams best represent an...Ch. 16 - Prob. 11ECh. 16 - Prob. 12ECh. 16 - Prob. 13ECh. 16 - 16.14 Which of the following statements is...Ch. 16 - Prob. 15ECh. 16 - Prob. 16ECh. 16 - Identify the Bronsted-Lowry acid and the...Ch. 16 - Prob. 18ECh. 16 - Prob. 19ECh. 16 - Prob. 20ECh. 16 - Prob. 21ECh. 16 - Prob. 22ECh. 16 - Prob. 23ECh. 16 - Prob. 24ECh. 16 - Prob. 25ECh. 16 - Prob. 26ECh. 16 - Prob. 27ECh. 16 - Prob. 28ECh. 16 - 16.29 Calcualte [H +] for each of the following...Ch. 16 - Prob. 30ECh. 16 - 16.31 At the freezing point of water (0 o C), K10...Ch. 16 - Prob. 32ECh. 16 - Prob. 33ECh. 16 - Prob. 34ECh. 16 - 16.35 Complete the following table by calculating...Ch. 16 - Prob. 36ECh. 16 - Prob. 37ECh. 16 - 16.38 Carbon dioxide in the atmosphere dissolves...Ch. 16 - Prob. 39ECh. 16 - Prob. 40ECh. 16 - Prob. 41ECh. 16 - Prob. 42ECh. 16 - Prob. 43ECh. 16 - Prob. 44ECh. 16 - Prob. 45ECh. 16 - Prob. 46ECh. 16 - Prob. 47ECh. 16 - Prob. 48ECh. 16 - Prob. 49ECh. 16 - write the chemical equation and the Ka expression...Ch. 16 - Prob. 51ECh. 16 - Prob. 52ECh. 16 - Prob. 53ECh. 16 - Prob. 54ECh. 16 - Prob. 55ECh. 16 - Prob. 56ECh. 16 - Prob. 57ECh. 16 - Prob. 58ECh. 16 - Calculate the pH of each of the following solution...Ch. 16 - Prob. 60ECh. 16 - Prob. 61ECh. 16 - Prob. 62ECh. 16 - Calculate the percent ionization of hydrazoic acid...Ch. 16 - 16.64 Calculate the percent ionization of...Ch. 16 - Prob. 65ECh. 16 - Prob. 66ECh. 16 - Prob. 67ECh. 16 - 16.68 The hypochlorite ion, CIO- , acts as a weak...Ch. 16 - Prob. 69ECh. 16 - Prob. 70ECh. 16 - Calculate the molar concentration of OH- in a...Ch. 16 - 16.72 Calculate the molar concentration of OH- in...Ch. 16 - Prob. 73ECh. 16 - Prob. 74ECh. 16 - Prob. 75ECh. 16 - Prob. 76ECh. 16 - a. Given that Ka for acetic acid is 1.8 10-5 and...Ch. 16 - 16.78
a. Given that Kb for ammonia is 1.8 X 10 -5...Ch. 16 - Prob. 79ECh. 16 - Prob. 80ECh. 16 - Prob. 81ECh. 16 - Pyridinium bromide (C5H5NHBr) is a strong...Ch. 16 - Prob. 83ECh. 16 - Prob. 84ECh. 16 - Prob. 85ECh. 16 - 16.86 An unknown salt is either KBr, NH4 C1, KCN,...Ch. 16 - Prob. 87ECh. 16 - Prob. 88ECh. 16 - 16.89 Based on their compositions and structures...Ch. 16 - Prob. 90ECh. 16 - 16.91 Indicate whether each of the following...Ch. 16 - Prob. 92ECh. 16 - Prob. 93ECh. 16 - Prob. 94ECh. 16 - Prob. 95ECh. 16 - Prob. 96ECh. 16 - Prob. 97ECh. 16 - Prob. 98ECh. 16 - Prob. 99AECh. 16 - Prob. 100AECh. 16 - Prob. 101AECh. 16 - Prob. 102AECh. 16 - Prob. 103AECh. 16 - Prob. 104AECh. 16 - Benzoic acid (C6H5COOH) and aniline (C6H5NH2) are...Ch. 16 - Prob. 106AECh. 16 - Prob. 107AECh. 16 - Prob. 108AECh. 16 - Butyric acid is responsible for the foul smell of...Ch. 16 - Prob. 110AECh. 16 - Prob. 111AECh. 16 - Prob. 112AECh. 16 - 1S.113 Many moderately large organic molecules...Ch. 16 - Prob. 114AECh. 16 - Prob. 115AECh. 16 - Prob. 116IECh. 16 - Prob. 117IECh. 16 - Prob. 118IECh. 16 - Prob. 119IECh. 16 - 16.120 At 50 oC, the ion-product constant for H2...Ch. 16 - Prob. 121IECh. 16 - Prob. 122IECh. 16 - Prob. 123IECh. 16 - Prob. 124IECh. 16 - Prob. 125IECh. 16 - Prob. 126IE
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- Exercise 16.2 Calculate [H+] in a solution in which [OH]=2.0102M. Is this solution acidic, neutral, or basic?arrow_forwardThe pH of an aqueous solution at 25.0 °C is 7.85. What is the molarity of OH- in this solution? Input answer in exponential form, example, if the answer is 5.72x10-8, enter as 5.72e-8.arrow_forwardITTL/ What is the pH of 92.9 mL of a solution which is 0.29 M in NaCN and 0.61 M in HCN? For HCN use K₂ = 4.9x10-10. Your Answer:arrow_forward
- What is the pH of 0.175 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 × 10−4.) ( please type answer note write by hend )arrow_forwardWhat are the concentrations of hydrogen ion and acetate ion in a solution of 0.10 M acetic acid, HC2H3O2? What is the pH of the solution? What is the degree of ionization? See Table 16.1 for the value of Ka.arrow_forwardAt 55°C aniline, CH NH₂, has a Kb = 8.2 *10-1⁰ What is the pH of a 0.035M solution in water? (Please type answer)arrow_forward
- Example 2What is the pH of the solution that results when 0.093 g of Mg(OH)2 Ksp = 7.1 × 10–12 is mixed with(a) 75.0 mL of 0.0500 M HCl?(b) 100.0 mL of 0.0500 M HCl?(c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?arrow_forwardWhat is the hydroxide ion concentration of a Ca(OH)2 solution that has a pH of 10.40? Please help with this chemistry question.arrow_forwardStatement 1: A 0.10 M solution of a weak acid has a [H3O+] of 0.10 M. Statement 2: A 0.10 M solution of a weak base has a [H3O+] that is greater than [HB+] which in the two statements is correct and which is incorrect?arrow_forward
- Learning Check Determine the pH of a 0.1M solution of the salt NaF basic due to F- Kb=Kw/Ka UNIVERSITY x² / 0.1 = 2.87e-11 I C F- 0.1M -X + H₂O → OH- + HF (aq) aq. E (0.1-x)≈ 0.1 N/A -X • N/A pOH=? 0 +x X 16.3. Salt solutions are not neutral if the ions are weak acids or bases pH=? 0 +xarrow_forwardThe ionization constant for water (Kw) is 5.9 × 10–14 at 50 °C. What is the [H3O+], [OH–], pH, and pOH for pure water at 50 °C? Question 30 options: a) [H3O+] = 2.4 x 10-7 M [OH–] = 2.4 x 10-7 M pH = 6.61 pOH = 6.61 b) [H3O+] = 6.5x 10-7 M [OH–] = 0.1 x 10-7 M pH = 5.01 pOH = 8.05 c) [H3O+] = 5.3 x 10-7 M [OH–] = 2.8 x 10-7 M pH = 1.82 pOH = 7.45 d) [H3O+] = 1.7 x 10-7 M [OH–] = 1.7 x 10-7 M pH = 6.77 pOH = 6.77arrow_forwardHELPP NOWWWW Equation :#H +MAVA=MBVB #OH- Question 1) what is the concentration of a unknown Mg (OH)2 solution if it took an average of 15.4mL of .100M HCL solution to neutralize 10.0 mL of the Mg (OH)2 solution Question 2) what is the concentration of an unknown LiOH solution if it took an average of 25.4mL of .100 HNO3 solution to neutralize 20.0mL of the LiOH solutionarrow_forward
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