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Part A The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, Assuming each solution to be 0.10 mol L-1, rank the following aqueous solutions in order of decreasing pH. pH = -log[H3O+] In neutral solutions at 25 °C, [H3O+] = 10-7 mol L-1 and pH = 7. As [H30+] increases, pH decreases, so acidic solutions have a pH of less than seven. Basic solutions have a pH greater than seven. The hydroxide and hydronium ion concentrations are related by the ion-product constant of water, Kw , as follows: Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help K, = 1.0 x 10-14 = [H30+][OH-] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the Kw expression that pH + рОН — 14. HCI NaOH HOCI Ba(OH), N2H4 Highest pH Lowest pH

Part A The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, Assuming each solution to be 0.10 mol L-1, rank the following aqueous solutions in order of decreasing pH. pH = -log[H3O+] In neutral solutions at 25 °C, [H3O+] = 10-7 mol L-1 and pH = 7. As [H30+] increases, pH decreases, so acidic solutions have a pH of less than seven. Basic solutions have a pH greater than seven. The hydroxide and hydronium ion concentrations are related by the ion-product constant of water, Kw , as follows: Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help K, = 1.0 x 10-14 = [H30+][OH-] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the Kw expression that pH + рОН — 14. HCI NaOH HOCI Ba(OH), N2H4 Highest pH Lowest pH

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Part A The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, pH = -log[H3O+] In neutral solutions at 25 °C, [H30+] = 10-7 mol L-1 and pH = 7. As [H30+] increases, pH decreases, so acidic solutions have a pH of less than seven. Basic solutions have a pH greater than seven. The hydroxide and hydronium ion concentrations are related by the ion-product constant of water, Kw , as follows: Assuming each solution to be 0.10 mol L-1 , rank the following aqueous solutions in order of decreasing pH. Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help Kw = 1.0 x 10-14 = [H3O+][OH¯] In the same way as the pH, we can define the pOH as pOH = -log[OH¯]. It follows from the Kw expression that PH + pОН — 14. HCl NaOH HOCI Ba(OH)2 N2H4 Highest pH Lowest pH
Transcribed Image Text:Part A The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, pH = -log[H3O+] In neutral solutions at 25 °C, [H30+] = 10-7 mol L-1 and pH = 7. As [H30+] increases, pH decreases, so acidic solutions have a pH of less than seven. Basic solutions have a pH greater than seven. The hydroxide and hydronium ion concentrations are related by the ion-product constant of water, Kw , as follows: Assuming each solution to be 0.10 mol L-1 , rank the following aqueous solutions in order of decreasing pH. Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help Kw = 1.0 x 10-14 = [H3O+][OH¯] In the same way as the pH, we can define the pOH as pOH = -log[OH¯]. It follows from the Kw expression that PH + pОН — 14. HCl NaOH HOCI Ba(OH)2 N2H4 Highest pH Lowest pH
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