21)
use:
pH = -log [H+]
12.26 = -log [H+]
[H+] = 5.495*10^-13 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(5.495*10^-13)
[OH-] = 1.82*10^-2 M
SO,
Mol of NaOH = [NaOH] * volume in L
= 1.82*10^-2 M * 1 L
= 1.82*10^-2 mol
Answer: 1.82*10^-2 mol
22)
Given:
[H+] = 0.045 M
use:
pH = -log [H+]
= -log (4.5*10^-2)
= 1.35
Answer: 1.35
23)
[OH-] > 1.0
POH = -log [OH-]
pOH will be less than 0
So,
pH will be greater than 14 since pH + pOH = 14
B is correct
C is correct
Answer: e
explain 21,22,23 UTILIT In this solution is a. 2.6 x 10-1° M b. 3.8 x 10...
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
SOLUTION CONDITION pH = 4.60 pOH = 5.60 (OH) = 4.5 x 10-6 M H) = 4.5 x 10-'M 1. The pH of Solution B is a. 10.61 b. 8.40 c. 7.98 d. 6.66 e. none of these 2. The pOH of Solution A is a. 9.40 b. 8.40 c. 7.88 d. 5.66 e. none of these 3. The pH of Solution Cis a. 12.61 b. 8.65 c. 7.98 d. 6.66 e. none of these 4. The pH of Solution...
WILSPILUIS SUSITIU 41722 Tourse o 25 1650 TocontentId = Question Completion Status: QUESTION 15 Calculate the pH of 0.026 M HC104. a. 1.59 b. 12.41 c. None of these d. 0.026 Oe. 7.00 Caps Lock is on QUESTION 16 Calculate the pH of a 0.045 M HCl solution a. 1.23 b. none of these c.12.65 d. 1.35 e. 12.29
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...
QUESTION A solution has [OH ]=59x 10-4 M. The pH of this solution is a. 5.39 b. 1.69 10-11 c 3.23 d. None of these e. 10.77 Caps Lock is on QUESTION 7 A solution has a pH of 3.99. The pOH of this solution is a. 3.99 b.4.09 c. 10.01 d. none of these e. 9.91
Calculate the pH and pOH of 1.2 x 10-3 M HCl solution. Calculate pH, pOH and [OH-] of 0.1 M HNO3 solution. If a solution X has pH = 5, which of the following is true: Solution X is neutral. H3O+ ion concentration is higher than OH- concentration. c. OH- ion concentration is higher than H3O+ concentration.
13) A 0.0035 M aqueous solution of a particular compound has pOH 11.54. The compound is a) a weak base b) a weak acid c) a strong base a strong acid e) a salt 14) In basic solution, a) [H30'> [OH] b) [H30 ]- [OH1 [Hs0)< [OH] d) (OH]<7.00 e) [OH] =OM 15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBro, at 25°C is 4.17. What is the value of K for HBro? a2.0 x 10...
explain 10,11,12 e. The answer depends on the volumes of the respective sululus. 10. A solution has [OH]=3.0 x10-'M. The [H] in this solution is a. 1.0M b. 3.0 x 107 M c. 1.0 x 10 M d. 3.3 x 108 M e. none of these 11. Calculate the [OH) in a solution that has a pH of 3.76. a. 5.8 x 10 M b. 1.0x 10 M c. 1.7x10+ M d. 2.7 x 10-4 M e. none of these...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
alculate the pH of a 0.543 M NH, solution. NH, has a Ky = 1.8 x 10 pH = Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral 0 pH = 4.59 pH=9.54 (H+) = 10x 10-7 pOH = 11.67 pOH = 4.94 (H+) - 3.7x 10-2 [H*) = 6.8 x 10- pOH = 7.00 [OH-] = 2.2 x 10- [OH-] = 5,5 x 10" Answer Bank Vhat...