Show ALL work and explain, please.
Show ALL work and explain, please. P-4) Hydrazine, N2Ha, is a weak base with a ko...
Hydrazine, N2H4, is a weak base that reacts in water to form hydrazinium ion. In an aqueous solution containing 0.150 M hydrazine, what would be the pH? For this problem, provide the following: Write the chemical equation that describes this solution, include phase symbols and any charges: Kb value and determine if the S.A. is valid. Construct the ICE table and solve for x Solve for the pHs.
Calculate pH of a weak base solution. Please box answers! Thank you! Tutored Practice Problem 16.4.5 G S GRASS Calculate the pH of a weak base solution ([B]o > 100Ko). Close Problem Calculate the pH of a 0.286 M aqueous solution of hydroxylamine (NH,OH, Kb - 9.1x10') and the equilibrium concentrations of the weak base and its conjugate acid. PH (NH3OH)equilibrium [NH3OH lequilibrium - Check & Submit Answer Show Approach
1. The weak base hydrazine, N2H4, has a Kb = 1.7 x 10-6. What is the percent ionization of a 0.15 M solution? 2. Hydrofluoric Acid has a Ka of 6.8 x 10-4. Calculate the [H+] in 0.25 M HF: 3. What is the pH of a 0.050 M solution of Acetic Acid, HC2H3O2? 4. A solution has a pOH of 10.25. Calculate the [H+].
Calculate pH of a weak base solution. Please box answers! Thank you! Close Problem Tutored Practice Problem 16.4.6 cm STOWARRANTIE Calculate the pH of a weak base solution (quadratic equation). Calculate the pH of a 0.0304 M aqueous solution of methylamine (CHANH. K. - 4.2x10*) and the equilibrium concentrations of the weak base and its conjugate acid PH [CH3NH2lequilibrium [CH3NH3 Jequilibrium - Check & Submnt Answer Show Approach
please give an explanation/ show work! thank you! For the diprotic weak acid H2A, Kal =2.0 x 10- and Ko e =8.6 x 10 What is the pH of a 0.0750 M solution of H,A? pH What are the equilibrium concentrations of H,A and A in this solution? H,A] = [A21=
a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ...
Instructions: Complete all the problems in this assignment Show all your work and submit a PDF with your answers through Husky CT for your lab section. Please e-mail me if you have an issues with the submission. Activity #1 Calculate the pH for the following acidic solutions 1. Calculate the pH and pOH for the following solutions: a. 0.200 M HNO3 b. 0.200 M H2SO4 2. Calculate the equilibrium concentration for [H], [A-], and [HA], the pH and pOH for...
Find the nominal concentrations of the weak acid or base in each of the following aqueous solutions: (a) HClO, pH = 4.6; (b) hydrazine, NH2NH2, pH = 10.2 The percentage ionization of benzoic acid in a 0.110 mol·L–1 solution is 2.4%. What is the pH of the solution and the pKa of benzoic acid?
please show work neatly and explain! 8) Calculate the molar solubility of Fe(OH)3 (Ko= 4.0 10-38 ) in the following (9 points): b) a solution buffered at a pH = 5.0 c) a solution buffered at a pH = 11.0
Please Show All Work! Also please ignore my answers written. Given the following data, Base Ko NH3 1.8 x 10-5 CH3NH2 5.0 x 10-4 C6H6NH, 4.2 x 10-10 Calculate the pH of 0.39 M solutions of 1. NH4NO3 pH = 9.255 2. CH3NH; NO3 pH = 10.69 3. CH NH3NO3 pH = 4.623