Questions for General, Organic, and Biological Chemistry Structures of Life, 5th Edition - Chapter (11)

General, Organic, and Biological Chemistry Fifth Edition Karen Timberlake Acids and Bases Chapter 11 Clicker Questions Chapter 11 – Acids and Bases Has a sour taste Neutralizes bases Produces H+ ions in water Is named potassium hydroxide 1. All except which of the following are characteristic of an acid? Chapter 11 – Acids and Bases Has a sour taste Neutralizes bases Produces H+ ions in water Is named potassium hydroxide 1. All except which of the following are characteristic of an acid? Chapter 11 – Acids and Bases Has a bitter taste Feels slippery Produces H+ ions in water Is used in drain cleaners 2. All except which of the following are characteristic of a base? Chapter 11 – Acids and Bases Has a bitter taste Feels slippery Produces H+ ions in water Is used in drain cleaners 2. All except which of the following are characteristic of a base? Chapter 11 – Acids and Bases H2O, because it accepts an H+ H2O, because it donates an H+ HNO3, because it accepts an H+ HNO3, because it donates an H+ Identify the acid in the following equation and explain why it is the acid. H2O + HNO3 ? H3O+ + NO3– Chapter 11 – Acids and Bases Identify the acid in the following equation and explain why it is the acid. H2O + HNO3 ? H3O+ + NO3– H2O, because it accepts an H+ H2O, because it donates an H+ HNO3, because it accepts an H+ HNO3, because it donates an H+ Chapter 11 – Acids and Bases 4. The conjugate acid of H2PO4– is ______. H3PO4 H2PO4– H2PO4 PO4–3 Chapter 11 – Acids and Bases 4. The conjugate acid of H2PO4– is ______. H3PO4 H2PO4– H2PO4 PO4–3 Chapter 11 – Acids and Bases 5. The conjugate base of HPO4–2 is ______. H3PO4 H2PO4– H2PO4 PO4–3 Chapter 11 – Acids and Bases 5. The conjugate base of HPO4–2 is ______. H3PO4 H2PO4– H2PO4 PO4–3 Chapter 11 – Acids and Bases Identify the acid on the left side of the following equation and identify its conjugate base on the right side. H2CO3(aq) + H2O(l) H3O+ (aq) + HCO3–(aq) H2CO3 is the acid; HCO3– is the conjugate base. H2CO3 is the acid; H3O+ is the conjugate base. H2O is the acid; HCO3– is the conjugate base. H2O is the acid; H3O+ is the conjugate base. Chapter 11 – Acids and Bases H2CO3 is the acid; HCO3– is the conjugate base. H2CO3 is the acid; H3O+ is the conjugate base. H2O is the acid; HCO3– is the conjugate base. H2O is the acid; H3O+ is the conjugate base. Identify the acid on the left side of the following equation and identify its conjugate base on the right side. H2CO3(aq) + H2O(l) H3O+ (aq) + HCO3–(aq) Chapter 11 – Acids and Bases Which of the following is not considered a strong acid? HI HF HCl HBr Chapter 11 – Acids and Bases Which of the following is not considered a strong acid? HI HF HCl HBr Chapter 11 – Acids and Bases In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH–? [H3O+] is less than [OH–]. [H3O+] is greater than [OH–]. They are equal. There is not enough information to tell. Chapter 11 – Acids and Bases [H3O+] is less than [OH–]. [H3O+] is greater than [OH–]. They are equal. There is not enough information to tell. In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH–? Chapter 11 – Acids and Bases An unknown solution has an [H3O+] of 3.8 × 10–9 M. Calculate the [OH–] and determine whether the solution is acidic or basic. [OH–] = 2.6 × 10–6 and is acidic [OH–] = 2.6 × 10–6 and is basic [OH–] = 3.8 × 105 and is acidic [OH–] = 3.8 × 105 and is basic Chapter 11 – Acids and Bases [OH–] = 2.6 × 10–6 and is acidic [OH–] = 2.6 × 10–6 and is basic [OH–] = 3.8 × 105 and is acidic [OH–] = 3.8 × 105 and is basic An unknown solution has an [H3O+] of 3.8 × 10–9 M. Calculate the [OH–] and determine whether the solution is acidic or basic. Chapter 11 – Acids and Bases blood, pH 7.38 shampoo, pH 5.7 soda, pH 3.2 vinegar, pH 2.8 All of the following are acidic solutions except _____. Chapter 11 – Acids and Bases blood, pH 7.38 shampoo, pH 5.7 soda, pH 3.2 vinegar, pH 2.8 All of the following are acidic solutions except _____. Chapter 11 – Acids and Bases 11. What is the pH of a 0.001 M solution of HCl? –3 –11 3 11 Chapter 11 – Acids and Bases –3 –11 3 11 11. What is the pH of a 0.001 M solution of HCl? Chapter 11 – Acids and Bases What is the pH of a 0.001 M solution of NaOH? –3 –11 3 11 Chapter 11 – Acids and Bases –3 –11 3 11 What is the pH of a 0.001 M solution of NaOH? Chapter 11 – Acids and Bases What is the pH of a 0.04 M KOH solution? 3.9 9.6 10.4 12.6 Chapter 11 – Acids and Bases 3.9 9.6 10.4 12.6 What is the pH of a 0.04 M KOH solution? Chapter 11 – Acids and Bases 14. What is the [H3O+] of a solution at pH 3.5? 0.00167 8.84 × 10–3 3.16 × 10–4 6.0 × 10–4 Chapter 11 – Acids and Bases 0.00167 8.84 × 10–3 3.16 × 10–4 6.0 × 10–4 14. What is the [H3O+] of a solution at pH 3.5? Chapter 11 – Acids and Bases [H3O+] = 2.0 × 10–5 and [OH–] = 5.0 × 10–10 [H3O+] = 5.0 × 10–10 and [OH–] = 2.0 × 10–5 [H3O+] = 2.0 × 10–10 and [OH–] = 5.0 × 10–5 [H3O+] = 5.0 × 10–5 and [OH–] = 2.0 × 10–10 What are the [H3O+] and [OH–] of a solution whose pH = 4.7? Chapter 11 – Acids and Bases [H3O+] = 2.0 × 10–5 and [OH–] = 5.0 × 10–10 [H3O+] = 5.0 × 10–10 and [OH–] = 2.0 × 10–5 [H3O+] = 2.0 × 10–10 and [OH–] = 5.0 × 10–5 [H3O+] = 5.0 × 10–5 and [OH–] = 2.0 × 10–10 What are the [H3O+] and [OH–] of a solution whose pH = 4.7? Chapter 11 – Acids and Bases 0.150 M 0.167 M 0.230 M 0.333 M A student titrated 15.0 mL of an unknown acid solution with 25.0 mL of a 0.100 M KOH solution. What is the molarity of the unknown acid? Chapter 11 – Acids and Bases 0.150 M 0.167 M 0.230 M 0.333 M A student titrated 15.0 mL of an unknown acid solution with 25.0 mL of a 0.100 M KOH solution. What is the molarity of the unknown acid? Chapter 11 – Acids and Bases HCl and NaCl NaOH and H2O HCN and NaCN HNO3 and NaOH Which of the following pairs can be used to make a buffer solution? Chapter 11 – Acids and Bases HCl and NaCl NaOH and H2O HCN and NaCN HNO3 and NaOH Which of the following pairs can be used to make a buffer solution? Chapter 11 – Acids and Bases 3.58 3.93 10.07 10.42 The Ka for formic acid, HCOOH, is 1.77 × 10–4. What is the pH of a buffer made from 2.0 M HCOOH and 3.0 M COOH–? Chapter 11 – Acids and Bases 3.58 3.93 10.07 10.42 The Ka for formic acid, HCOOH, is 1.77 × 10–4. What is the pH of a buffer made from 2.0 M HCOOH and 3.0 M COOH–? Chapter 11 – Acids and Bases During stress or trauma, a person can start to hyperventilate. The person might breathe into a paper bag to avoid fainting. Which of the following describes the changes that occur in the blood pH during hyperventilation? The CO2 level in the blood decreases, H2CO3 decreases, H3O+ decreases, and the blood pH decreases. The CO2 level in the blood increases, H2CO3 increases, H3O+ increases, and the blood pH increases. The CO2 level in the blood decreases, H2CO3 decreases, H3O+ decreases, and the blood pH increases. The CO2 level in the blood increases, H2CO3 increases, H3O+ increases, and the blood pH decreases. Chapter 11 – Acids and Bases The CO2 level in the blood decreases, H2CO3 decreases, H3O+ decreases, and the blood pH decreases. The CO2 level in the blood increases, H2CO3 increases, H3O+ increases, and the blood pH increases. The CO2 level in the blood decreases, H2CO3 decreases, H3O+ decreases, and the blood pH increases. The CO2 level in the blood increases, H2CO3 increases, H3O+ increases, and the blood pH decreases. During stress or trauma, a person can start to hyperventilate. The person might breathe into a paper bag to avoid fainting. Which of the following describes the changes that occur in the blood pH during hyperventilation?