1. a.* Should the equivalent of 0.01 M AgBr [K [K, for Ag(NH.7x10]? 5x10 dissolve in 6MNH, b. Wha...
What mass of AgBr will dissolve in 500.0 mL of 5.50 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the reaction Ag⁺(aq) + 2NH₃(aq) ⇌ Ag(NH₃)₂⁺(aq) K = 1.7 × 10⁷
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O. 2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side...
Please help with solving Question 1 (A-C) Thank you! Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
17.6 Based on the information in Appendix D, calculate the pH and trimethylammonium ion concentration of a solution of trimethylamine, (CH3) 3N, 0.075 M, and trimethylammonium chloride, (CH3) 3NHCl, 0.10 M. CONSTANTS OF AQUEOUS BALANCE Кок LO X 107 3.0 X 10-12 X L6 X 10 12 Kat 18 X 105 5.6 X 10- 5.1 X 10-10 3 X 10 6.3 X 105 5.8 X 10 10 15 X Ls 43 X 10 14 X 1st 1 x 102 74...