Student Solutions Manual for Ebbing/Gammon's General Chemistry
11th Edition
ISBN: 9781305886780
Author: Darrell Ebbing; Steven D. Gammon
Publisher: Cengage Learning US
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 15, Problem 15.23QP
Interpretation Introduction
Interpretation:
What ion is produced by the addition of
Concept introduction:
Lewis theory:
Lewis acid: A species which can form a covalent bond by accepting electron pairs for the species is said to be Lewis acid.
Lewis base: A species which can form a covalent bond by donating electron pairs for the species is said to be Lewis base.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
A scientist is comparing two lakes. She finds that water samples from Lake X have a pH of 3.50 and water samples from Lake Y have a pH
of 5.50.
Therefore, it can be said that Lake X has a hydronium ion concentration that is
times greater than Lake Y.
Consider the following data on some weak acids and weak bases:
name
K₂
formula
HNO₂ 4.5 x 104
acetic acid HCH,CO₂ 1.8x105
acid
nitrous acid
solution
0.1 M HONHYBT
0.1 M KBr
Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to
the solution that will have the next lowest pH, and so on.
0.1 M KCH₂CO₂
0.1 M C₂H₂NHCI
PH
choose one
choose one
choose one
base
choose one
K
name
formula
hydroxylamine HONH₂ 1.1 x 107
pyridine
CH₂N 1.7×10
Calculate the pH and pOH of the following solutions (see
Appendix 11 of your textbook for pKa values):
1. 0.01 M HBr
2. 0.00005 M HBr
3. 0.00002 МКОН
4. 0.01 M CH,COOH
5. 0.00001 M CH,COOH
6. 0.01 M HIO,
7. 0.01 M pyridine
Calculate the pH of the following solutions:
1. 0.01 M NAHS
2. 0.005 M NaН.РО,
3. 0.005 M Na,HPO,
4. 0.005 M Na PO,
5. 0.1 ΜΝΗ,CN
Calculate the pH of the following buffer solutions:
1. 1.7 g/L of NH, and 5.35 g/L of NH,Cl.
2. 50 mL of 1 M CH,COONA and 1 L 0.1 M CH,COOH.
3. 50 mL of 1 M NaOH and 1 L 0.1 M CH,COOH.
4. 10 mL 0.1 H,PO, + 25 mL 0.1 NaOH
5. 10 mL 0.1 H,PO, + 25 mL 0.1 Na,PO,
6. A buffer solution pH=5.00 contains 0.01 M CH,COOH.
Calculate the concentration of sodium acetate it contains.
7. What weight of NH,Cl should be added to 1 L of 0.1 M
NH, solution to get pH=9.00?
Chapter 15 Solutions
Student Solutions Manual for Ebbing/Gammon's General Chemistry
Ch. 15.2 - For the reaction H2CO3(aq)+CN(aq)HCN(aq)+HCO3(aq)...Ch. 15.2 - Prob. 15.1CCCh. 15.3 - Identify the Lewis acid and the Lewis base in each...Ch. 15.4 - Prob. 15.3ECh. 15.4 - Prob. 15.2CCCh. 15.5 - Which member of each of the following pairs is the...Ch. 15.7 - A solution of barium hydroxide at 25C is 0.125 M...Ch. 15.7 - Prob. 15.6ECh. 15.7 - Rank the following solutions from most acidic to...Ch. 15.8 - What is the pH of a sample of gastric juice...
Ch. 15.8 - A saturated solution of calcium hydroxide has a...Ch. 15.8 - A brand of carbonated beverage has a pH of 3.16....Ch. 15.8 - A 0.010 M solution of ammonia, NH3, has a pH of...Ch. 15.8 - Prob. 15.4CCCh. 15 - Which of the following are strong acids? Which are...Ch. 15 - Describe any thermochemical (heat of reaction)...Ch. 15 - Prob. 15.3QPCh. 15 - Prob. 15.4QPCh. 15 - Write an equation in which H2PO3 acts as an acid...Ch. 15 - Describe four ways in which the BrnstedLowry...Ch. 15 - Prob. 15.7QPCh. 15 - Explain why an acidbase reaction favors the weaker...Ch. 15 - Give two important factors that determine the...Ch. 15 - Prob. 15.10QPCh. 15 - Prob. 15.11QPCh. 15 - Prob. 15.12QPCh. 15 - Prob. 15.13QPCh. 15 - Prob. 15.14QPCh. 15 - The conjugate base of hydrofluoric acid dissolved...Ch. 15 - In the following reaction, identify the Lewis...Ch. 15 - Calculate the hydronium-ion concentration at 25C...Ch. 15 - The pH of a solution is 9.55 at 25C What is the...Ch. 15 - Acids You make a solution by dissolving 0.0010 mol...Ch. 15 - Strong Acids, Weak Acids, and pH Two 0.10-mol...Ch. 15 - Prob. 15.21QPCh. 15 - Prob. 15.22QPCh. 15 - Prob. 15.23QPCh. 15 - Compare the structures of HNO2 and H2CO3. Which...Ch. 15 - Prob. 15.25QPCh. 15 - Prob. 15.26QPCh. 15 - A strong monoprotic acid, with the molecular...Ch. 15 - A weak acid, HA, is dissolved in water. Which one...Ch. 15 - Write the balanced reaction of hydroxide ion with...Ch. 15 - Write the balanced reaction of hypobromous acid,...Ch. 15 - Give the conjugate base to each of the following...Ch. 15 - Give the conjugate base to each of the following...Ch. 15 - Give the conjugate acid to each of the following...Ch. 15 - Give the conjugate acid to each of the following...Ch. 15 - For the following reactions, label each species as...Ch. 15 - For the following reactions, label each species as...Ch. 15 - The following shows ball-and-stick models of the...Ch. 15 - The following shows ball-and-stick models of the...Ch. 15 - Complete each of the following equations. Then...Ch. 15 - Complete each of the following equations. Then...Ch. 15 - In the following reactions, identify each reactant...Ch. 15 - In the following reactions, label each reactant as...Ch. 15 - Natural gas frequently contains hydrogen sulfide,...Ch. 15 - Coal and other fossil fuels usually contain sulfur...Ch. 15 - Complete the following equation. Using Table 15.2,...Ch. 15 - Complete the following equation. Using Table 15.2,...Ch. 15 - Use Table 15.2 to decide whether the species on...Ch. 15 - Use Table 15.2 to decide whether the species on...Ch. 15 - Prob. 15.49QPCh. 15 - In the following reaction of tetrafluoroboric...Ch. 15 - For each of the following pairs, give the stronger...Ch. 15 - Order each of the following pairs by acid...Ch. 15 - What are the concentrations of H3O+ and OH in each...Ch. 15 - What are the concentrations of H3O+ and OH in each...Ch. 15 - A solution of hydrochloric acid is 0.059 M HCl....Ch. 15 - A solution is 0.030 M HNO3 (nitric acid). What is...Ch. 15 - What are the hydronium-ion and the hydroxide-ion...Ch. 15 - A saturated solution of magnesium hydroxide is 3.2...Ch. 15 - The following are solution concentrations....Ch. 15 - The following are solution concentrations....Ch. 15 - A shampoo solution at 25C has a hydroxide-ion...Ch. 15 - An antiseptic solution at 25C has a hydroxide-ion...Ch. 15 - Which of the following pH values indicate an...Ch. 15 - Which of the following pH values indicate an...Ch. 15 - For each of the following, state whether the...Ch. 15 - Prob. 15.66QPCh. 15 - Obtain the pH corresponding to the following...Ch. 15 - Obtain the pH corresponding to the following...Ch. 15 - A sample of vinegar has a hydronium-ion...Ch. 15 - Some lemon juice has a hydronium-ion concentration...Ch. 15 - Obtain the pH corresponding to the following...Ch. 15 - Obtain the pH corresponding to the following...Ch. 15 - A solution of washing soda (sodium carbonate,...Ch. 15 - A solution of lye (sodium hydroxide, NaOH) has a...Ch. 15 - The pH of a cup of coffee (at 25C) was found to be...Ch. 15 - A wine was tested for acidity, and its pH was...Ch. 15 - A detergent solution has a pH of 11.80 at 25C....Ch. 15 - Morphine is a narcotic that is used to relieve...Ch. 15 - A 1.00-L aqueous solution contained 5.80 g of...Ch. 15 - A 1.00-L aqueous solution contained 6.78 g of...Ch. 15 - A certain sample of rainwater gives a yellow color...Ch. 15 - A drop of thymol blue gave a yellow color with a...Ch. 15 - Identify each of the following as an acid or a...Ch. 15 - Which of the following substances are acids in...Ch. 15 - Write a reaction for each of the following in...Ch. 15 - Write a reaction for each of the following in...Ch. 15 - Prob. 15.87QPCh. 15 - Prob. 15.88QPCh. 15 - Prob. 15.89QPCh. 15 - Prob. 15.90QPCh. 15 - Prob. 15.91QPCh. 15 - List the following compounds in order of...Ch. 15 - A solution is 0.18 M KOH. What are the...Ch. 15 - A solution is 0.25 M Sr(OH)2. What are the...Ch. 15 - Prob. 15.95QPCh. 15 - A sample of lemon juice has a hydronium-ion...Ch. 15 - Prob. 15.97QPCh. 15 - A sample of grape juice has a pH of 4.15. What is...Ch. 15 - A 4.640-g sample of a mixture of sodium hydrogen...Ch. 15 - A 2.500-g sample of a mixture of sodium carbonate...Ch. 15 - Prob. 15.101QPCh. 15 - The dihydrogen phosphate ion has the ability to...Ch. 15 - Prob. 15.103QPCh. 15 - Prob. 15.104QPCh. 15 - Prob. 15.105QPCh. 15 - Show how methylamine, CH3NH2, is a BrnstedLowry...Ch. 15 - Prob. 15.107QPCh. 15 - Prob. 15.108QPCh. 15 - Prob. 15.109QPCh. 15 - Prob. 15.110QPCh. 15 - Prob. 15.111QPCh. 15 - Hydrazine, N2H4 (having the structure H2NNH2), and...Ch. 15 - Prob. 15.113QPCh. 15 - Liquid ammonia undergoes autoionization similar to...Ch. 15 - Ethanol (ethyl alcohol), CH3CH2OH, can act as a...Ch. 15 - Ethanol, CH3CH2OH, can undergo auto-ionization....Ch. 15 - Aluminum chloride, AlCl3, reacts with...Ch. 15 - Consider each of the following pairs of compounds,...Ch. 15 - Arrange each of the following in order of...Ch. 15 - The following is a table of some of the oxoacids...Ch. 15 - Suppose you have 557 mL of 0.0300 M HCl, and you...Ch. 15 - Prob. 15.122QPCh. 15 - You want to make up 3.00 L of aqueous hydrochloric...Ch. 15 - Prob. 15.124QPCh. 15 - Prob. 15.125QPCh. 15 - Pure liquid ammonia ionizes in a way similar to...Ch. 15 - A solution contains 4.25g of ammonia per 250.0 mL...Ch. 15 - A solution contains 0.675 g of ethylamine,...Ch. 15 - Prob. 15.129QPCh. 15 - Hypophosphorous acid, H3PO2, and phosphoric acid,...Ch. 15 - Boron trifluoride, BF3, and ammonia, NH3, react to...Ch. 15 - Boron trifluoride, BF3, and diethyl ether,...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Follow the directions of Question 19 for the following acids: (a) hypochlorous acid (b) formic acid, HCHO2 (c) acetic acid, HC2H3O2 (d) hydrobromic acid (e) sulfurous acidarrow_forwardIron in drinking water is removed by precipitation of the Fe3+ ion by reaction with NaOH to produce iron(III) hydroxide. Write the balanced chemical equation and the net ionic equation for this reaction.arrow_forward4. Suppose you had a sample of Hydrobromic acid that had a molarity of 0.1 and you had 42 ml of it. If you added 20 ml of 0.15 M NaOH, what is the pH of the resulting solution? NaOH + HBr -> NaBr H2Oarrow_forward
- KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP– . HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g mol and at 25 °C has a pKa of 5.4.arrow_forwardFor each of the following pairs of substances • Classify each of the substances. • Compare their approximate pH levels. • Compare their ability to conduct electricity. • Compare their relative hydronium or hydroxide concentration. Comparison of 1.0 mol/L LIOH(aq) and 1.0 mol/L HOCI(aq) • LIOH(aq) is classified as a • HOCI(aq) is classified as a • HOCI(aq) has a + pH than LIOH(aq) has. . нос(ag) is a + electrical conductor than LIOH(aq) is. LIOH(aq) has a : [OH (aq)] than HOCI(aq) has. Comparison of 1.0 mol/L HCN(aq) and 1.0 mol/L KF(aq) • KF(aq) is classified as a • HCN(aq) is classified as a • HCN(aq) has a : pH than KF(aq) has. • HCN(aq) is a + electrical conductor than KF(ag) is. • HCN(aq) has a + [H30+(aq)] than KF(aq) has.arrow_forwardThe CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of H2CO3/HCO3− is required to obtain a pH of 7.40, the pH of blood? (Assume that the Ka of H2CO3 is 4.4 ✕ 10−8.)arrow_forward
- If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.arrow_forwardA laboratory technician wants to determine the aspirin content of a headache pill by acid-base titration. Aspirin has a Ka of 3.0 x 10−4. If the pill is dissolved in water to give a solution about 0.015 M, what is the pH of this solution? (Neglect dilution effects.) If the solution in the problem above is then titrated against KOH solution, what will be the pH at the stoichiometric point.arrow_forwardHydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.arrow_forward
- The acidity of a solution is measured by its pH. If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 158 times greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 3.4, determine the pH of Solution A. Report your answer to one decimal place. Solution A has pH equal to Number (Report to the nearest 0.1)arrow_forwardThe following assertions apply to acid A and base B. • When acid A interacts with a strong base and base B reacts with a strong acid, neutral salts are generated.• The Ka of Acid A is greater than that of HClO2.• The pH of a 2.13 x 10–3 M solution of base B is 11.6. Which among the choices below is most likely? a. Acid A is HClO and base B is NaOH. b. Acid A is HBrO4 and base B is KOH. c. Acid A is HClO4 and base B is Ba(OH)2. d. Acid A is HBrO2 and base B is Sr(OH)2.arrow_forwardCalculate the hydrogen ion concentration in mol/L for solutions with the following pH values: (a) 2.42, (b) 11.21, (c) 6.96, (d) 15.00.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY