![Calculate [H3O^+] for each pH value using the formula [H3O^+] = 10^-pH.](/_next/image?url=https%3A%2F%2Fohijasnjvprzodcmxltt.supabase.co%2Fstorage%2Fv1%2Fobject%2Fpublic%2Fwhatsapp-images%2F1774544337444-deda6757fe1a2b49.png&w=3840&q=75)
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here are the solutions for Exercise 3.10: 1. Which solution has a higher [H_3O^+] concentration, one with pH=5, or with pH=8? Step 1: Calculate [H_3O^+] for each pH value using the formula [H_3O^+] = 10^-pH. For pH=5: [H_3O^+] = 10^-5 M For pH=8: [H_3O^+] = 10^-8 M Step 2: Compare the concentrations. Since 10^-5 > 10^-8, the solution with pH=5 has a higher [H_3O^+] concentration. Answer: The solution with pH=5 has a higher [H_3O^+] concentration. 2. Which solution has the higher OH^- concentration? Step 1: Calculate pOH for each pH value using the formula pOH = 14 - pH. For pH=5: pOH = 14 - 5 = 9 For pH=8: pOH = 14 - 8 = 6 Step 2: Calculate [OH^-] for each pOH value using the formula [OH^-] = 10^-pOH. For pOH=9: [OH^-] = 10^-9 M For pOH=6: [OH^-] = 10^-6 M Step 3: Compare the concentrations. Since 10^-6 > 10^-9, the solution with pH=8 has a higher [OH^-] concentration. Answer: The solution with pH=8 has a higher [OH^-] concentration. 3. Give the pH and pOH for each solution with the following concentrations: a) [H_3O^+] = 1.0 × 10^-3 Step 1: Calculate pH using the formula pH = -[H_3O^+]. pH = -(1.0 × 10^-3) = 3.0 Step 2: Calculate pOH using the formula pOH = 14 - pH. pOH = 14 - 3.0 = 11.0 Answer: pH = 3.0, pOH = 11.0 b) [OH^-] = 1.0 × 10^-9 M Step 1: Calculate pOH using the formula pOH = -[OH^-]. pOH = -(1.0 × 10^-9) = 9.0 Step 2: Calculate pH using the formula pH = 14 - pOH. pH = 14 - 9.0 = 5.0 Answer: pH = 5.0, pOH = 9.0 4. Give the hydroxide ion concentrations of solutions with the following values of pH: a) pH 13.0 Step 1: Calculate pOH using the formula pOH = 14 - pH. pOH = 14 - 13.0 = 1.0 Step 2: Calculate [OH^-] using the formula [OH^-] = 10^-pOH. [OH^-] = 10^-1.0 M = 0.1 M Answer: [OH^-] = 0.1 M b) pH 3.0 Step 1: Calculate pOH using the formula pOH = 14 - pH. pOH = 14 - 3.0 = 11.0 Step 2: Calculate [OH^-] using the formula [OH^-] = 10^-pOH. [OH^-] = 10^-11.0 M Answer: [OH^-] = 10^-11.0 M c) pH 8.0 Step 1: Calculate pOH using the formula pOH = 14 - pH. pOH = 14 - 8.0 = 6.0 Step 2: Calculate [OH^-] using the formula [OH^-] = 10^-pOH. [OH^-] = 10^-6.0 M Answer: [OH^-] = 10^-6.0 M 5. Which of the solutions is most acidic? Which is most basic? (Referring to the solutions from part 4: pH 13.0, pH 3.0, pH 8.0) • Acidity increases as pH decreases. The lowest pH among 13.0, 3.0, and 8.0 is 3.0. • Basicity increases as pH increases. The highest pH among 13.0, 3.0, and 8.0 is 13.0. Answer: The solution with pH=3.0 is most acidic. The solution with pH=13.0 is most basic.