General, Organic, & Biological Chemistry
3rd Edition
ISBN: 9780073511245
Author: Janice Gorzynski Smith Dr.
Publisher: McGraw-Hill Education
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Chapter 9.6, Problem 9.22P
Convert each
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c.
d.
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Chapter 9 Solutions
General, Organic, & Biological Chemistry
Ch. 9.1 - Name each acid: (a)HF;(b)HNO3;(c)HCN.Ch. 9.1 - If the polyatomic anion C1O2- is called chlorite,...Ch. 9.1 - Which of the following species can be...Ch. 9.1 - Which of the following species can be...Ch. 9.1 - Classify each reactant as a Brønsted-Lowry acid or...Ch. 9.2 - Determine the conjugate acid of each species:...Ch. 9.2 - Determine the conjugate base of each species:...Ch. 9.2 - Draw the structure of the conjugate base of each...Ch. 9.2 - Label the acid and the base and the conjugate acid...Ch. 9.2 - Ammonia, NH3, is amphoteric. Draw the conjugate...
Ch. 9.2 - Prob. 9.11PCh. 9.3 - Diagrams represent three acids (HA) dissolved in...Ch. 9.3 - Label the stronger acid in each pair. Which acid...Ch. 9.3 - Are the reactants or products favored at...Ch. 9.3 - If lactic acid is similar in strength to acetic...Ch. 9.4 - Rank the acids in each group in order of...Ch. 9.4 - Use the acid dissociation constants in Table 9.3...Ch. 9.4 - Consider the weak acids, HCN and H2CO3. Which acid...Ch. 9.5 - Calculate the value of [OH-] from the given [H3O+]...Ch. 9.5 - Calculate the value of [H3O+] from the given [OH-]...Ch. 9.5 - Calculate the value of [H3O+] and [H3O-] in each...Ch. 9.6 - Convert each H3O+ concentration to a pH value. a....Ch. 9.6 - What H3O+ concentration corresponds to each pH...Ch. 9.6 - Prob. 9.24PCh. 9.6 - Convert each H3O+ concentration to a pH value....Ch. 9.6 - Prob. 9.26PCh. 9.7 - Write a balanced equation for each acid-base...Ch. 9.7 - Prob. 9.28PCh. 9.7 - The acid in acid rain is generally sulfuric acid...Ch. 9.7 - Write a balanced equation for the reaction of...Ch. 9.8 - Determine whether each salt forms an acidic,...Ch. 9.8 - Which of the following salts forms an aqueous...Ch. 9.9 - What is the molarity of an HCI solution if 25.5 mL...Ch. 9.9 - How many milliliters of 2.0MNaOH are needed to...Ch. 9.10 - Determine whether a solution containing each of...Ch. 9.10 - Consider a buffer prepared from the weak acid HCO3...Ch. 9.10 - Calculate the pH of a dihydrogen...Ch. 9.10 - What is the pH of a buffer that contains...Ch. 9 - Which of the following species can be...Ch. 9 - Which of the following species can be...Ch. 9 - Prob. 9.41PCh. 9 - Which of the following species can be...Ch. 9 - Prob. 9.43PCh. 9 - Draw the conjugate acid of each base. a. Br- b....Ch. 9 - Draw the conjugate base of each acid. HNO2 NH4+...Ch. 9 - Draw the conjugate base of each acid. H3O+ H2Se...Ch. 9 - Prob. 9.47PCh. 9 - Prob. 9.48PCh. 9 - Prob. 9.49PCh. 9 - Prob. 9.50PCh. 9 - Label the conjugate acid-base pairs in each...Ch. 9 - Label the conjugate acid-base pairs in each...Ch. 9 - Prob. 9.53PCh. 9 - Prob. 9.54PCh. 9 - Fill in the missing product in each acid-base...Ch. 9 - Fill in the missing product in each acid-base...Ch. 9 - Prob. 9.57PCh. 9 - Write the equation for the acid-base reaction that...Ch. 9 - Prob. 9.59PCh. 9 - Which diagram represents what happens when HCN...Ch. 9 - Prob. 9.61PCh. 9 - Prob. 9.62PCh. 9 - Prob. 9.63PCh. 9 - Use the data in and 9.2 and 9.3 to label the...Ch. 9 - Prob. 9.65PCh. 9 - Which acid, A or B, is stronger in each part? a. B...Ch. 9 - Fill in the missing terms (strong or weak) and...Ch. 9 - Fill in the missing terms (strong or weak) and...Ch. 9 - For each pair of acids: [1] Label the stronger...Ch. 9 - For each pair of acids: [1] Label the stronger...Ch. 9 - Prob. 9.71PCh. 9 - Prob. 9.72PCh. 9 - Prob. 9.73PCh. 9 - Label the acid in the reactants and the conjugate...Ch. 9 - Calculate the value of [OH-] from the given and...Ch. 9 - Calculate the value of [OH-] from the given [H3O+]...Ch. 9 - Calculate the value of [OH-] from the given [HO-]...Ch. 9 - Calculate the value of [H3O+] from the given [OH-]...Ch. 9 - Prob. 9.79PCh. 9 - Prob. 9.80PCh. 9 - Prob. 9.81PCh. 9 - Complete the following table with the needed...Ch. 9 - Prob. 9.83PCh. 9 - Prob. 9.84PCh. 9 - Prob. 9.85PCh. 9 - If pancreaticfluids have a pH of 8.2, calculate...Ch. 9 - Calculate the concentrations of H3O+ and OH in the...Ch. 9 - Prob. 9.88PCh. 9 - Prob. 9.89PCh. 9 - Prob. 9.90PCh. 9 - Prob. 9.91PCh. 9 - Prob. 9.92PCh. 9 - Write a balanced equation for each reaction. a....Ch. 9 - Prob. 9.94PCh. 9 - Prob. 9.95PCh. 9 - Prob. 9.96PCh. 9 - Prob. 9.97PCh. 9 - Prob. 9.98PCh. 9 - Prob. 9.99PCh. 9 - Prob. 9.100PCh. 9 - Whatisthe molarityofanaceticacid (CH3COOH)...Ch. 9 - What is the molarity of an H2SO4 solution if 18.5...Ch. 9 - How many milliliters of 1.0MNaOH solution are...Ch. 9 - How many milliliters of 2.0MNaOH solution are...Ch. 9 - Prob. 9.105PCh. 9 - Prob. 9.106PCh. 9 - Prob. 9.107PCh. 9 - Prob. 9.108PCh. 9 - Prob. 9.109PCh. 9 - Prob. 9.110PCh. 9 - Using the Ka values in Table9.6, calculate the pH...Ch. 9 - Using the Ka values in Table9.6, calculate the pH...Ch. 9 - Calculate the pH of an acetic acid/acetate buffer...Ch. 9 - Calculate the pH of a bicarbonate/carbonate buffer...Ch. 9 - Why is the pH of unpolluted rainwater lower than...Ch. 9 - Prob. 9.116PCh. 9 - Prob. 9.117PCh. 9 - A sample of rainwater has a pH of 4.18. Calculate...Ch. 9 - Prob. 9.119PCh. 9 - Prob. 9.120PCh. 9 - Prob. 9.121PCh. 9 - Prob. 9.122PCh. 9 - Prob. 9.123CPCh. 9 - Prob. 9.124CP
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- Unpolluted rain water has a pH of about 5.5. Acid rain has been shown to have a pH as low as 3.0. Calculate the [H+] ratio of acid rain to unpolluted rain.arrow_forwardFigure 14.3 shows the pH of some common solutions. How many times more acidic or basic is each of these compared with a neutral solution? (a) Black coffee (b) Household ammonia (c) Baking soda (d) Vinegararrow_forwardThe measured pH of a sample of seawater is 8.30. (a) Calculate the H3O+ concentration. (b) Is the sample acidic or basic?arrow_forward
- Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?arrow_forwardWhat is meant by “pH”? True or false: A strong acid always has a lower pH than a weak acid does. Explain.arrow_forward3. A solution has a pH of 10.54. What is the hydronium ion concentration? 2.9 × 10−11 M 2.7 × 10−5 M 10.54 M 3.5 × 1010 Marrow_forward
- Household ammonia is a solution of the weak base NH3 in water. List, in order of descending concentration, all of the ionic and molecular species present in a1-M aqueous solution of this base.arrow_forwardFigure 14.3 shows the pH of some common solutions. How many times more acidic or basic is each of these compared with a neutral solution? (a) Milk (b) Seawater (c) Blood (d) Battery acidarrow_forwardWhich of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH] > 1.0 X IO’7Marrow_forward
- Which of the solutions listed below has the lowest pH? (a) 0.10 M HCl (b) 0.10 M NaOH (c) 2.5 105 M HNO3 (d) pure H2Oarrow_forwardAcrylic acid (CH29CHCO2H) is a precursor for many important plastics. Ka for acrylic acid is 5.6 105. a. Calculate the pH of a 0.10-M solution of acrylic acid. b. Calculate the percent dissociation of a 0.10-M solution of acrylic acid. c. Calculate the pH of a 0.050-M solution of sodium acrylate (NaC3H3O2).arrow_forwardA 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000arrow_forward
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