Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 15, Problem 15.48QE
Find [OH−] and the pH of the following solutions.
- (a) 0.25 g barium hydroxide, Ba(OH)2, dissolved in enough water to make 0.655 L of solution
- (b) A 3.00 L solution of KOH is prepared by diluting 300.0 mL 0.149 M KOH with water.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution.
(a) Show the reaction between HClO and OH–.
(b) What is the final volume after two solutions were mixed?
(c) What is the final molarity of HClO after the reaction with OH–?
(d) What is the pH after 20.0 mL of the NaOH solution is added? (Ka of HClO is 3.0*10–8)?
The sample of 25.0 mL of 0.0200 M NH3 is titrated with a 20.0 mL of 0.0150 M HCl solution.
(a) Show the reaction between NH3 and H+.
(b) What is the final volume after two solutions were mixed?
(c) What is the final molarity of NH3 after the reaction with H+?
(d) What is the pH after 20.0 mL of the HCl solution is added? (Ka of NH4+ is 5.6 x 10–10)
Hydrochloric acid is one of the common acids used in the laboratory. It is a very strong acid and react with many substances including metals.
(a) Why is hydrochloric acid classified as a strong acid?
(b) Write a chemical equation to represent its action on zinc
(c) What is observed when:
litmus paper is dipped in hydrochloric acid?
two drops of methyl orange is put in 20cm3 of 0.1M hydrochloric acid?
iii. Hydrochloric acid react with calcium carbonate
Chapter 15 Solutions
Chemistry: Principles and Practice
Ch. 15 - Prob. 15.1QECh. 15 - Can a compound be an Arrhenius base and not a...Ch. 15 - Water is not the only solvent that undergoes...Ch. 15 - Write two BrnstedLowry acid-base reactions and...Ch. 15 - Define pH and explain why pH, rather than...Ch. 15 - Prob. 15.6QECh. 15 - Prob. 15.7QECh. 15 - Prob. 15.8QECh. 15 - Prob. 15.9QECh. 15 - Prob. 15.10QE
Ch. 15 - Prob. 15.11QECh. 15 - Prob. 15.12QECh. 15 - Why have chemists not tabulated the fraction...Ch. 15 - Prob. 15.15QECh. 15 - Prob. 15.16QECh. 15 - Prob. 15.17QECh. 15 - Prob. 15.18QECh. 15 - Define oxyacid and give examples from among the...Ch. 15 - Prob. 15.20QECh. 15 - Prob. 15.21QECh. 15 - Prob. 15.22QECh. 15 - Prob. 15.23QECh. 15 - Prob. 15.24QECh. 15 - Prob. 15.25QECh. 15 - Write the formula and name for the conjugate acid...Ch. 15 - For each of the following reactions, identify the...Ch. 15 - Prob. 15.28QECh. 15 - Prob. 15.29QECh. 15 - Prob. 15.30QECh. 15 - Prob. 15.31QECh. 15 - Write an equation to describe the proton transfer...Ch. 15 - Prob. 15.33QECh. 15 - Determine the hydrogen ion or hydroxide ion...Ch. 15 - Prob. 15.35QECh. 15 - The hydroxide ion concentrations in wines actually...Ch. 15 - Prob. 15.37QECh. 15 - Prob. 15.38QECh. 15 - Prob. 15.39QECh. 15 - Prob. 15.40QECh. 15 - Prob. 15.41QECh. 15 - Prob. 15.42QECh. 15 - Prob. 15.43QECh. 15 - Prob. 15.44QECh. 15 - Prob. 15.45QECh. 15 - Prob. 15.46QECh. 15 - A saturated solution of milk of magnesia, Mg(OH)2,...Ch. 15 - Find [OH] and the pH of the following solutions....Ch. 15 - Write the chemical equation for the ionization of...Ch. 15 - Prob. 15.50QECh. 15 - Prob. 15.51QECh. 15 - Prob. 15.52QECh. 15 - Prob. 15.53QECh. 15 - Assuming that the conductivity of an acid solution...Ch. 15 - Prob. 15.55QECh. 15 - Prob. 15.56QECh. 15 - Prob. 15.57QECh. 15 - Prob. 15.58QECh. 15 - Prob. 15.59QECh. 15 - A 0.10 M solution of chloroacetic acid, ClCH2COOH,...Ch. 15 - Prob. 15.61QECh. 15 - Prob. 15.62QECh. 15 - Prob. 15.63QECh. 15 - Prob. 15.64QECh. 15 - Prob. 15.65QECh. 15 - Prob. 15.66QECh. 15 - Prob. 15.67QECh. 15 - Prob. 15.68QECh. 15 - Write the chemical equation for the ionization of...Ch. 15 - Prob. 15.70QECh. 15 - Hydrazine, N2H4, is weak base with Kb = 1.3 106....Ch. 15 - Prob. 15.72QECh. 15 - Prob. 15.73QECh. 15 - Prob. 15.74QECh. 15 - Calculate the [OH] and the pH of a 0.024 M...Ch. 15 - Prob. 15.76QECh. 15 - Prob. 15.77QECh. 15 - Prob. 15.78QECh. 15 - Prob. 15.79QECh. 15 - Prob. 15.80QECh. 15 - Find the value of Kb for the conjugate base of the...Ch. 15 - Consider sodium acrylate, NaC3H3O2. Ka for acrylic...Ch. 15 - Prob. 15.83QECh. 15 - Prob. 15.84QECh. 15 - Prob. 15.85QECh. 15 - Prob. 15.86QECh. 15 - Prob. 15.87QECh. 15 - Prob. 15.88QECh. 15 - Prob. 15.89QECh. 15 - Prob. 15.90QECh. 15 - Prob. 15.91QECh. 15 - Prob. 15.92QECh. 15 - Prob. 15.93QECh. 15 - Prob. 15.94QECh. 15 - Explain how to calculate the pH of a solution that...Ch. 15 - Prob. 15.96QECh. 15 - Prob. 15.97QECh. 15 - Prob. 15.98QECh. 15 - Hypofluorous acid, HOF, is known, but fluorous...Ch. 15 - Prob. 15.100QECh. 15 - Prob. 15.101QECh. 15 - Prob. 15.102QECh. 15 - Which of each pair of acids is stronger? Why? (a)...Ch. 15 - Prob. 15.104QECh. 15 - Prob. 15.105QECh. 15 - Prob. 15.106QECh. 15 - Prob. 15.107QECh. 15 - Prob. 15.108QECh. 15 - Prob. 15.109QECh. 15 - Prob. 15.110QECh. 15 - Prob. 15.111QECh. 15 - Prob. 15.112QECh. 15 - Prob. 15.113QECh. 15 - Prob. 15.114QECh. 15 - Prob. 15.115QECh. 15 - Prob. 15.116QECh. 15 - Prob. 15.117QECh. 15 - Prob. 15.118QECh. 15 - Prob. 15.119QECh. 15 - Prob. 15.120QECh. 15 - A solution is made by diluting 25.0 mL of...Ch. 15 - A Liquid HF undergoes an autoionization reaction:...Ch. 15 - Pure liquid ammonia ionizes in a manner similar to...Ch. 15 - Prob. 15.124QECh. 15 - Prob. 15.125QECh. 15 - Prob. 15.126QECh. 15 - Prob. 15.127QECh. 15 - Prob. 15.128QECh. 15 - An aqueous solution contains formic acid and...Ch. 15 - A solution is made by dissolving 15.0 g sodium...Ch. 15 - Calculate the pH of a solution prepared by adding...Ch. 15 - Prob. 15.132QECh. 15 - Prob. 15.133QECh. 15 - When perchloric acid ionizes, it makes the...Ch. 15 - Prob. 15.135QE
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
- What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.arrow_forwardAcids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forwardWhat is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water tomake 450. mL of solution? Assume that Ba(OH)2 dissociates completely in water to Ba2+ andOH¯ ions. What is the pH of the solution?arrow_forward
- 2. Barbituric acid, HC,H,N,O, a weak organic acid used to manufacture hypnotic drugs and some plastic, has a Ka of 9.8 x 10 An industrial process requires a 0.25 mol/L solution of Barbituric acid. (a) Calculate the H° and pH of the solution. (b) What is the percent ionization of the acid?arrow_forwarda) A solution is made by mixing 350 mL of .5 M hydrofluoric acid with 50 mL of 1.5 M KOH. Calculate the pH of the solution. (b) to the solution above is added 2.00 grams of sodium fluoride. What is the new pH? (c) to the solution from part (a) you add 75 mL of .5 M HCl. What is the new pH? (d) To the solution from part (a) you add 25 mL of .45 M KF, what is the new pHarrow_forwardWhen sodium fluoride (NaF) is added to an HF solution, what happens to the pH of the solution and why? (A) The pH will not change because NaF is an ionic compound that is neither acid nor base. (B) The pH will decrease because F– absorbs H+ and decreasing the H3O+(aq) concentration. (C) The pH will increase because F– absorbs H+ and decreasing the H3O+(aq) concentration. (D) The pH will not change because NaF is a neutral compound.arrow_forward
- 14) Calculate the following for the given aqueous solutions at 25.0 oC: a) The Molarity of a Ba(OH)2 solution whose pH = 13.85 b) The pH of a 5.48 x 10–8 M Ca(OH)2 solution. c) The [OH–] concentration of a Sr(OH)2 solution whose pH is 14.65. d) The pH of a 12.0 M HCl solution.arrow_forward(a) A solution is prepared by dissolving 0.23 mol of NaH(s) inenough water to form 2.8 L of solution. Calculate its pH.(b) The pH of some orange juice at 25°C is 2.85. Calculate[H3O+] and [OH2].arrow_forwardCalculate the pH of each of the following strong acid solutions. (a) 0.00813 M HBrO4 pH = (b) 0.443 g of HBr in 39.0 L of solution pH = (c) 25.0 mL of 6.80 M HBrO4 diluted to 2.00 L pH = (d) a mixture formed by adding 65.0 mL of 0.00719 M HBrO4 to 67.0 mL of 0.00254 M HBr pH =arrow_forward
- Calculate the pH of each of the following strong acid solutions. (a) 0.00577 M HCIO4 pH = (b) 0.523 g of Hl in 18.0 L of solution pH= (c) 27.0 mL of 8.90 M HCIO4 diluted to 1.90 LpH = (d) a mixture formed by adding 52.0 mL of 0.00627 M HCIO4 to 25.0 mL of 0.00315 M HI pH =arrow_forward4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂arrow_forwardCalculate the pH of each of the following strong acid solutions. (a) 0.00704 M HIO4 pH = (b) 0.696 g of HIO4 in 25.0 L of solution pH = X PH = (c) 70.0 mL of 8.00 M HIO4 diluted to 3.40 L X pH = X (d) a mixture formed by adding 16.0 mL of 0.00197 M HIO4 to 16.0 mL of 0.00284 M HIO4 Xarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral 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 Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: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
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY