EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 117QP
Interpretation Introduction
Interpretation:
The reaction taking place when
Concept Introduction:
A molecule or ion capable of losing a proton is known as an acid. An acid that partially dissociates into its ions in water or an aqueous solution is known as a weak acid whereas a strong acid fully dissociates into its ions in an aqueous solution or water.
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Write the equation for dissolving Hydrochloric acid in water (include water). Identify base, acid, conjugate acid, and conjugate base. Describe where the equilibrium lies and why.
Hydrogen selenide (H2Se) reacts with water according to the following equation.
H2Se + H2O → SeH– + H3O+
Can you identify the acid, base, conjugate acid, and conjugate base in this reaction? Use patterns in the periodic table to explain why the substances you identified acted as the acid and the base in this reaction.
Hydrochloric acid is used for removing rust from iron or steel before it is processed for other uses.
5.07 g of HCl(g) is dissolved in water to make a 220 mL solution.
Calculate the pH of the solution.
Do not show your work. Record only your final answer with the correct number of significant digits. Remember, pH does not have units!
Use the following information to complete the statement below.
Solution Information Provided
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[H3O+ (aq)] = 5.5 x 10-¹2 mol/L
pOH = 11.92
pH = 3.8
[OH (aq)] = 7.45 x 10-³ mol/L
The four solutions in order from least basic to most basic are
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Chapter 13 Solutions
EBK INTRODUCTION TO CHEMISTRY
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)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_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_forward
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- Write a balanced chemical equation to represent each of the following acidbase neutralization reactions. a. HCl and LiOH b. HNO3 and Ba(OH)2 c. H2SO4 and NaOH d. KOH and H3PO4arrow_forwardWhat is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?arrow_forwardWrite a balanced chemical equation to represent each of the following acidbase neutralization reactions. a. HCl and NaOH b. HNO3 and KOH c. H2SO4 and LiOH d. Ba(OH)2 and H3PO4arrow_forward
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