The [H3O+] in a cabernet sauvignon wine is 5.9 x 10-4 M. What is the (-OH)...
The (H+] in a cabernet wine is 3.8 x 10-4 M. What is the [OH-] in this wine? Show Work on Scratch Paper! 3.8 x 10-4 M 1.0 x 10-10 M 3.8 x 10-18 M 2.6 x 10-11 M 1.0 x 10-14 M
If [H3O+] = 2.65x10–4 M, what is [OH–]? If [H3O+] = 2.65x10–4 M, what is [OH–]? a. 2.65 x 10–18 M b. 2.65 x 1010 M c. 2.65 x 10–4 M d. 3.77 x 10–11 M
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2. Which species is the conjugate base of HPO 2-? Refresher of Acid/Base Equilibria, Ka, and pK., and buffer solutions: 1. The (H30') in a cabernet Sauvignon wine is 5.9 x 10 M. What is the (-OH) in this wine? 2. The pH of a lime is 1.90. What is the [H30*]? 3. What is the pH of a cleaning solution with a [H3O+] =...
If the [OH–] of a solution is 1.5 × 10–4 M, the [H3O+] is ... (use parethesis to help) A. 1.2 x 10-2 B. 1.0 x 10-7 C. 1.5 x 10-3 D. 6.3 x 10-6 M E. 6.7 x 10-11 M
a) Calcuate the pH of a solution with [H3O+] = 6.54 x 10-3 M b) Calcuate the pOH of a solution with [H3O+] = 8.5 x 10-9 M c) A solution has a pH = 2.420, what is the [OH-]? d) A solution has a pOH = 1.0, what is the [OH-]? e) Calcuate the pH of a solution with [OH-] = 5.9 x 10-6 M
1. 2.0 x 10-9 M H3O+ 2. 1.0 x 10-7 M OH¯ 3. 5.2 x 10-6 M H3O+ 4. 3.1 x 10-10 M OH¯ Which of these is characteristic of a basic solution?
A student makes a solution of 1.00 X 10^-7 M NaOH at 298K. Which of the following is NOT true for this solution at 25C? a) [OH-] > 1.0 X 10^-7 b) [OH-][H3O+] = 1.0 X 10^-14 c) [OH-] > [H3O] d) [OH-] = 1.0 X 10^-7 e) [OH-]/[H3O+]>1 Explain why!! Please
Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]= M Solution B:[H3O+]=8.91×10−9 M Solution B: [OH−]= M Solution C:[H3O+]=7.61×10−4 M Solution C: [OH−]= M Which of these solutions are basic at 25 °C? A:[OH−]=2.59×10−7 M B:[H3O+]=8.91×10−9 M
Calculate the pH of each solution given the following [H3O+] or [OH−] values. a)[H3O+] = 4.0×10−4 M Express your answer using two decimal places. b)[H3O+] = 8.0×10−9 M c)[OH−] = 7.0×10−5 M d)[OH−] = 4.5×10−11 M e)[H3O+] = 8.0×10−8 M f)[OH−] = 8.6×10−4 M
Calculate the concentration of H3O for an aqueous solution with a pH of 6.20. A) 6.3 x 10-7 M E) 4.0 x 10 M 1. B) 1.6 x 10 M C) 1.0x 10-14 M D) 6.20 x 1014 M 2. The pH of a 0.010 M aqueous solution of Ca(OH)2 is A) 11.70 B) 12.00 C) 12.30 E) 1.70 D) 12.60 alution with a nH of 9.60. for an aqueous solution with a pH of 9.60. C) 1.5 x 10-5...