Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH...
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...
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...
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
Calculate the pH of a 0.400 M HNO2 solution. Report answer to 2 decimal places. Ka = 7.1 x 10-4 HNO2 (aq) + H20 (1) = NO2 (aq) + H30+ (aq) Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH3 (methylammonium chlorides Report answer to 2 decimal places. CHH) - 4.4 x 10-4 CH3NH2 (aq) + H200 - Chynas (aq) + OH" () 1. Questa
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate the equilibrium hydroxide ion concentration in a 0.95 M solution of the base. [OH-] = What are the pH and pOH of the solution?
7. (5 pts) Determine the pOH of a 0.227 M solution of the WB pyridine, CsHsN; K (CsH5N) = 1.7x10. a) 9.41 (Situation #3) b) 4.59 c) 9.39 d) 3.86 e) 4.71 8. (4 pts) Determine the Kcfor the conjugate acid CH NH3'; K, for the WB CH3NH2 = 4.4x104. a) 3.1x10-10 b) 6.8x10-11 c) 5.6x10-10 d) 2.3x103 e) 2.3x10-11 9. (5 pts) Determine the pH of a mixed solution where (HCIO2). = 0.15 M with K. - 1.1x102 and...
Calculate the PH and concentrations of CH3NH2 and CH3NH3+ in a 0.0445M Methylamine (CH3NH2) Calculate the pH and concentrations of CH3NH2 and CH3NH3 in a 0.0445 M methylamine (CH3NH2) solution. The Kb of CH3NH2-4.47 x10 Number pH11.520 Number CH,NH0.0409 Number CH, NH, |-| | 0.00446
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
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...