Question

STUDY CHECK 10.6 What is the [H3O+] of an ammonia cleaning solution with [OH-] = 4.0 x 10^-4 M? Is the solution acidic, basic, or neutral? ANSWER [H3O+] = 2.5 x 10^-11 M, basic PRACTICE PROBLEMS 10.5 Dissociation of Water LEARNING GOAL Use the water dissociation expression to calculate the [H3O+] and [OH-] in an aqueous solution. 10.25 Why are the concentrations of H3O+ and OH- equal in pure water? 10.26 What is the meaning and value of Kw? 10.27 In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH-? 10.28 If a base is added to pure water, why does the [H3O+] decrease? 10.29 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 2.0 x 10^-5 M b. [H3O+] = 1.4 x 10^-9 M c. [OH-] = 8.0 x 10^-3 M d. [OH-] = 3.5 x 10^-10 M 10.30 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 6.0 x 10^-12 M b. [H3O+] = 1.4 x 10^-4 M c. [OH-] = 5.0 x 10^-12 M d. [OH-] = 4.5 x 10^-2 M Clinical Applications 10.31 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. coffee, 1.0 x 10^-5 M b. soap, 1.0 x 10^-8 M c. cleanser, 5.0 x 10^-10 M d. lemon juice, 2.5 x 10^-2 M 10.32 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. oven cleaner, 1.0 x 10^-12 M b. milk of magnesia, 1.0 x 10^-9 M c. aspirin, 6.0 x 10^-4 M d. pancreatic juice, 4.0 x 10^-9 M 10.33 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. stomach acid, 2.5 x 10^-13 M b. urine, 2.0 x 10^-9 M c. orange juice, 5.0 x 10^-11 M d. bile, 2.5 x 10^-6 M 10.34 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. baking soda, 1.0 x 10^-6 M b. blood, 2.5 x 10^-7 M c. milk, 4.0 x 10^-7 M d. bleach, 2.1 x 10^-3 M 10.6 The pH Scale LEARNING GOAL Calculate the pH of a solution from [H3O+]; given the pH, calculate [H3O+]. The proper level of acidity is necessary to evaluate the functioning of the lungs and kidneys, to control bacterial growth in foods, and to prevent the growth of pests in food crops. In the environment, the acidity, or pH, of rain, water, and soil can have significant effects. When rain becomes too acidic, it can dissolve aluminum from soil, which is toxic to many plants and fish.

          STUDY CHECK 10.6 What is the [H3O+] of an ammonia cleaning solution with [OH-] = 4.0 x 10^-4 M? Is the solution acidic, basic, or neutral? ANSWER [H3O+] = 2.5 x 10^-11 M, basic PRACTICE PROBLEMS 10.5 Dissociation of Water LEARNING GOAL Use the water dissociation expression to calculate the [H3O+] and [OH-] in an aqueous solution. 10.25 Why are the concentrations of H3O+ and OH- equal in pure water? 10.26 What is the meaning and value of Kw? 10.27 In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH-? 10.28 If a base is added to pure water, why does the [H3O+] decrease? 10.29 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 2.0 x 10^-5 M b. [H3O+] = 1.4 x 10^-9 M c. [OH-] = 8.0 x 10^-3 M d. [OH-] = 3.5 x 10^-10 M 10.30 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 6.0 x 10^-12 M b. [H3O+] = 1.4 x 10^-4 M c. [OH-] = 5.0 x 10^-12 M d. [OH-] = 4.5 x 10^-2 M Clinical Applications 10.31 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. coffee, 1.0 x 10^-5 M b. soap, 1.0 x 10^-8 M c. cleanser, 5.0 x 10^-10 M d. lemon juice, 2.5 x 10^-2 M 10.32 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. oven cleaner, 1.0 x 10^-12 M b. milk of magnesia, 1.0 x 10^-9 M c. aspirin, 6.0 x 10^-4 M d. pancreatic juice, 4.0 x 10^-9 M 10.33 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. stomach acid, 2.5 x 10^-13 M b. urine, 2.0 x 10^-9 M c. orange juice, 5.0 x 10^-11 M d. bile, 2.5 x 10^-6 M 10.34 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. baking soda, 1.0 x 10^-6 M b. blood, 2.5 x 10^-7 M c. milk, 4.0 x 10^-7 M d. bleach, 2.1 x 10^-3 M 10.6 The pH Scale LEARNING GOAL Calculate the pH of a solution from [H3O+]; given the pH, calculate [H3O+]. The proper level of acidity is necessary to evaluate the functioning of the lungs and kidneys, to control bacterial growth in foods, and to prevent the growth of pests in food crops. In the environment, the acidity, or pH, of rain, water, and soil can have significant effects. When rain becomes too acidic, it can dissolve aluminum from soil, which is toxic to many plants and fish.

STUDY CHECK 10.6 What is the [H3O+] of an ammonia cleaning solution with [OH-] = 4.0 x 10^-4 M? Is the solution acidic, basic, or neutral? ANSWER [H3O+] = 2.5 x 10^-11 M, basic PRACTICE PROBLEMS 10.5 Dissociation of Water LEARNING GOAL Use the water dissociation expression to calculate the [H3O+] and [OH-] in an aqueous solution. 10.25 Why are the concentrations of H3O+ and OH- equal in pure water? 10.26 What is the meaning and value of Kw? 10.27 In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH-? 10.28 If a base is added to pure water, why does the [H3O+] decrease? 10.29 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 2.0 x 10^-5 M b. [H3O+] = 1.4 x 10^-9 M c. [OH-] = 8.0 x 10^-3 M d. [OH-] = 3.5 x 10^-10 M 10.30 Indicate whether each of the following solutions is acidic, basic, or neutral: a. [H3O+] = 6.0 x 10^-12 M b. [H3O+] = 1.4 x 10^-4 M c. [OH-] = 5.0 x 10^-12 M d. [OH-] = 4.5 x 10^-2 M Clinical Applications 10.31 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. coffee, 1.0 x 10^-5 M b. soap, 1.0 x 10^-8 M c. cleanser, 5.0 x 10^-10 M d. lemon juice, 2.5 x 10^-2 M 10.32 Calculate the [OH-] of each aqueous solution with the following [H3O+]: a. oven cleaner, 1.0 x 10^-12 M b. milk of magnesia, 1.0 x 10^-9 M c. aspirin, 6.0 x 10^-4 M d. pancreatic juice, 4.0 x 10^-9 M 10.33 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. stomach acid, 2.5 x 10^-13 M b. urine, 2.0 x 10^-9 M c. orange juice, 5.0 x 10^-11 M d. bile, 2.5 x 10^-6 M 10.34 Calculate the [H3O+] of each aqueous solution with the following [OH-]: a. baking soda, 1.0 x 10^-6 M b. blood, 2.5 x 10^-7 M c. milk, 4.0 x 10^-7 M d. bleach, 2.1 x 10^-3 M 10.6 The pH Scale LEARNING GOAL Calculate the pH of a solution from [H3O+]; given the pH, calculate [H3O+]. The proper level of acidity is necessary to evaluate the functioning of the lungs and kidneys, to control bacterial growth in foods, and to prevent the growth of pests in food crops. In the environment, the acidity, or pH, of rain, water, and soil can have significant effects. When rain becomes too acidic, it can dissolve aluminum from soil, which is toxic to many plants and fish.

Added by Gemayrole A.

Question

Please give Ace some feedback