A solution of 0.025 M NH OH (K a) Calculate Kb 1.11 x 10) (20 p!)...
A solution of 0.025 M NH2OH (Ka-1.11 x 10") (20 pt) a) Calculate Kb b) Calculate the [OH). [NH,OH) and (NH,OH'). c) Calculate the pH and POH of the solution. d) What is the pH of the solution if the solution was mixed with 0.78 M NH3OH"?
Kw 1.0 x 1014 Ks 6.6 X 10 for HF Kb 1.8 X 10 for NH 1. Calculate the [H'], [OHl, pH and pOH for 0.025 M HCl 2. Calculate the pH of 4.0 M hydrofluoric acid, HF. (over)
Calculate the pH of a 0.445 M NH, solution. NH, has a Kb = 1.8 x 10-5. pH = The K, of a weak monoprotic acid is 1.59 x 10-5. What is the pH of a 0.0808 M solution of this acid? pH =
Calculate the (OH) and the pH of a 0.023-M methylamine solution; Kb = 5.0 x 10". [OH-] =D pH =
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...
Calculate the following values for a 0.025 M solution of Hydrocyanic acid. Ka= 4.90 × 10^-10 [H3O+]eq [OH-]eq = pH = pOH = % Ionization =
NH, is a weak base (Kb = 1.8 x 10-M), so the salt NH, Cl acts as a weak acid. What is the pH of a solution that is 0.033 M in NH CI? pH = pH = {
Calculate the hydroxide concentration of a 0.024 M methylamine solution. Kb is 4.2 x 10-4 This problem has a second part in the problem below.... part 1 .What is the OH- concentration? B) Consider the same 0.024 M methylamine solution. Kb is 4.2 x 10-4 part 2 -- what is the pH?
10. Fill in each blánk with increases or decreases As K, increases, acid strength As Kb increases, base strength As pK, increases, acid strength As pKb increases, base strength As acid strength increases, conjugate base strength The stronger an acid, the the conjugate base. (stronger or weaker) HoCI NH4 11. a) Which is the HS stronger acid? stronger acid? stronger base? stronger base? HF pk-3.14 CH,OH pk, 10.0 b) Which is the c) Which is the d) Which is the...
7) Calculate the K, of butanoic acid (monoprotic) if a 0.025 M aqueous solution has a pH of 3.21 at 25°C 8) trans-cinnamic acid (C,H,O, monoprotic) has a K = 3.60 x 10-5 a. Calculate the pH of a 0.020 M aqueous solution of this acid. b. Calculate the percentage of acid dissociated (i.e., in the "A" form) in this solution using your calculations in (a). CHEM 120B-Activity #3 Acids and Bases Page 5