Calculate the pOH of 390 mL of a 0.3 M aqueous solution of methylammonium chloride (CH3NH3Cl) at 25 °C given that the Kb of methylamine (CH3NH2) is 4.4×10-4.
8.42
3.35
3.56
2.13
8.04
Calculate the pOH of 390 mL of a 0.3 M aqueous solution of methylammonium chloride (CH3NH3Cl)...
Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. 1.61 8.75 5.25 12.39
What is the pOH of a solution of 0.125 M CH3NH2 and 0.130M CH3NH3CI CH3NH2 +H20 > CH3NH3Cl +OH Kb = 4.4 *10^-4
Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH2 tor (methylammonium chloride). Report answer to 2 decimal places. Kb CH3NH2) - 44 x 10-4 CH3NH2 (aq) + H200 + CH3NH3 (2) + OH(aq) Assuming equal initial concentrations of the given species, which of the following is the weakest acid in aqueous solution? O. HB Ky = 2.0 x 10-6 OB.HD K = 6.0 x 10-2 ОС: НЕ Kg = 4.0 x...
Question 7 of 9 How many moles of CH3NH3Cl need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for CH3NH2 is 4.4 * 10-4) to make a buffer with a pH of 11.60? mol C +/- 0 x 100
Consider a buffer solution which consists of methyl amine (CH3NH2) and methyl ammonium chloride (CH3NH3Cl). At what pH is this buffer solution most effective? (Kb = 4.4⋅10−4 for methyl amine)
Calculate the pH of a buffer solution that is 1.25 M CH3NH2 and 1.00 M CH3NH3Cl. Kb = 8.85 x 10-4 and what would happen after 35.0 mL of 0.45 M HNO3 is added to 250.0 mL of the buffer solution, what would the pH of the solution be after the HNO3(aq) is added?
Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...
10) The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl) in 1.00 L of 1.35 M methylamine (CH3NH2) is Kb for methylamine is 4.40 x 10-4. (Assume the final volume is 1.00 L.) The A) 11.03 B) 2.97 C) 3.75 D) 10.64 E) 10.25 11) A 25.0 mL sample of 0.723 M HCIO4 is titrated with a 0.27 M KOH solution. The H30+ concentration after the addition of 80.0 ml of KOH is M....
Determine the pH of a 0.10 M CH3NH3Cl solution. (Kb (CH3NH2) = 4.4 x 10-4) 2.18 11.82 5.82 8.17 3.36
Calculate the pH of a solution prepared by mixing equal volumes of 0.20 M methylamine (CH3NH2 Kb 3.7x 10-4) and 0.60 M CH3NH3Cl.