Answer e i.e 1.2M
If the pH of a solution of NH, is 11.67, what is the concentration of NH,...
Clicker What is the pH of a solution that contains 0.05 M NH, and 0.10 M NH Br? Ko (NH3) = 1.76 x 10-5, Hint: convert Ko to K, before using the equation A. 9.25 B. 8.94 C. 9.55 pH =pK, + log [base] D. 4.45 ([acid]) E. 10.97
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
IWCI. 5) What is the H30 pH values? (a) 0.00 concentration to the correct number of significant figures for solutions with the following (b) 7.00 (c) 2.63 (d) - 0.42 (e) 11.21 6) (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NH4Cl-NH; buffer that has a pH of 9.00? (The Kb for NH; is 1.8 x 10%)
QUESTION 6 What is the pH of a solution that has a H? concentration equal to 1.7 x 10-5 M? A) 4.77 B) 5.20 C) 0.22 D) 10.20 E) none of the above
6. Consider titration of 20.0 ml of 0.100 M NH, with 0.200 M HCl solution. Calculate the pH after the addition of the following volumes of HCl solution. The Koof NH, = 1.8 x 10 (4 pts each, 12 pts total) 100M NH3 00 L=.08 a. 0.00 ml NH3 + H20 OH- + NH4 ka 10m 5.56 x 10 10 1.8x10-S 100M TX +X X X 100M X=[oH ] = 1.34 X 10 - 3M pOH = -10 g (1.34...
What is the pH of a 0.14 M solution of methylammonium chloride, CH NH, CI? What is the concentration of methylamine in the solution? Ks (methylamine) - 4.4 x 10-4 pH- Concentration =
What is the concentration of hydroxide ions in pH= 5.0 solution? Select one: a. 1.6 x 10-5 M b. 5.0 x 10-5 M c. 3.2 x 10-9 M d. 2.3 x 10-8 M e. 1.0x 10-5 M Clear my choice ◄ Chem100 ProblemSet7
What is the pH of a solution at 25 oC if OH- concentration is 1 x 10-4 M? A. 10 B. 6 C. 4 D. None of the above
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...
A buffered solution containing dissolved aniline, CH NH, and aniline hydrochloride, CH-NH, CI, has a pH of 5.49. A. Determine the concentration of CGH NH; in the solution if the concentration of CoH_NH, is 0.290 M. The pKy of aniline is 9.13. [C,H,NH] = M B. Calculate the change in pH of the solution, ApH, if 0.358 g NaOH is added to the buffer for a final volume of 1.55 L. Assume that any contribution of NaOH to the volume...