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The (H+] in a cabernet wine is 3.8 x 10-4 M. What is the [OH-] in...
The [H3O+] in a cabernet sauvignon wine is 5.9 x 10-4 M. What is the (-OH) in this wine? O A) 1.0 x 10-7 M-OH O B) 5.9 x 10-4 M -OH OC) 1.0 x 10-14 M-OH OD) 1.7 x 10-11 M -OH E) 5.9 x 10-18 M OH
What is the hydronium-ion concentration of a 0.0038 M Ba(OH)2 solution? A) 7.6 x 10–3 M B) 3.8 x 10–3 M C) 1.3 x 10–12 M D) 2.6 x 10–12 M E) 1.0 x 10–7 M
D l Question 1 If the H concentration in a solution is 2.6 x 10-7 M, what is the OH concentration? e 3.8 x 108 M O 2.6 x 10-7 M 2.6 x 10.21 M 40 x 107 M 8.1 x 10 10 M Question 2 1 pts
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
A 0.050 M solution of a weak monoprotic acid, HA, has [H3O+] = 3.8 x 10-5. What is the value of Ka for this acid? 2.6 x 10-11 2.9 x 10-8 7.5 x 10-3 7.0 x 10-8 7.0 x 10-7
explain 21,22,23 UTILIT In this solution is a. 2.6 x 10-1° M b. 3.8 x 10 M c. 9.58 d. 4.42 e. none of these 21. How many moles of pure NaOH must be used to prepare 1.0 L of a solution that has pH = 12.26? a. 8.2 x 10-16 mol b. 0.018 mol c. 5.5 x 10-13 mol d. 1.74 mol e. none of these 22. Calculate the pH of a 0.045 M HCl solution. K a. 1.23...
I got an answer of about 8.4 x 10^-8, however, that's not an answer choice, so I'm not sure what I'm doing wrong. Help please! The hypothetical weak acid H2A ionizes as shown below. H2A + H+ + HA K1 = 1.0 x 10-7 HA- + H+ + A2- K2 = 5.0 x 10-11 Calculate the [A2-) in a 0.20 M aqueous solution of H2A. 1. 4.6 x 10-13 M 2. 5.8 x 10-14 M 3. 3.8 x 10-18 M...
The pH of a lime is 7.5 What is the [H+]? Show Work on Scratch Paper! O 3.2 x 10-8 MH+ 3.2 x 1012 MH O 7.5 x 10-14 MH+ O 7.5 x 10-1 MH+ O 7.5 MH+
Which of the following is most acidic? A. A solution with [H,0+] = 1.0 x 10-10 B. A solution with [H,0+] = 1.0 x 10-5 C. A solution with [OH-] = 1.0 x 10-10 D. A solution with [OH-] = 1.0 x 10-5 E. A solution with a pH of 5. Question 5 Which of the following is most basic? A. CA solution with [H,0+] = 1.0 x 10-10 B. A solution with [H0+] = 1.0 x 10-5 C. A...
[References] Calculate (OH") (H+), and the pH of 0.37 M solutions of each of the following amines (K for aniline is 3.8 x 10-20 K, for methylamine is 4.38 x 10-4) a aniline M [OH"]= [H+] - M pH- b. methylamine [OH-]- M (H+) - M pH