Part A ) Calculate the pH of 0.20 M NH3 (Kb=1.8×10−5).
Express your answer using two decimal places.
Part B) Calculate the concentrations of all species present in 0.20 M NH3 (Kb=1.8×10−5).
Express your answers using two significant figures separated by commas. Enter the concentrations of the species in the order listed below.
[NH4+],[NH3],[OH−],[H3O+] = ?,?,?,?
if you have any doubts about the answer please mention in the comments please do rate the answer.
Part A ) Calculate the pH of 0.20 M NH3 (Kb=1.8×10−5). Express your answer using two...
Part A Calculate the pH in 1.26 M CH3CO2H. Part B Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 1.26 M CH3CO2H. Express your answers using two significant figures separated by commas. Enter your answers in order listed in the question. Part C Calculate the pH in 9.50×10−2 M CH3CO2H. Part D Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 9.50×10−2 M CH3CO2H. Express your answers using two significant figures...
Part A: Calculate the pH of 0.61 M NH3 (Kb=1.8×10−5). Part B: Calculate the concentrations of all species present in 0.61 M NH3 (Kb=1.8×10−5).
Determine the pH for the following solutions: Part A [OH-] = 2.7x10-7M Express your answer using two decimal places. ANSWER: pH = Part B H3O+] = 4.7x10-3M Express your answer using two decimal places. ANSWER: pH = Part C [H3O+] = 2x10-4M Express your answer using one decimal place. ANSWER: pH = Part D [OH-] = 8.0x10-9 M Express your answer using two decimal places. ANSWER: pH = Problem 10.92 Calculate the [H3O+] and [OH-] for a solution with the...
Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C.
Part A 0.19 M NaOH Express your answer using two significant figures. Enter your answers numerically separated by commas. 30 AZ OO ? [OH-], H0+] - 5.3 • 10-14 Submit Previous Answers Request Answer Part B Express your answer to two decimal places. Enter your answers numerically separated by commas. © A ¢ O 2 ? pH. pOH = Submit Request Answer Part 2 Part C 1.4x10-3M Ca(OH), er using two significant figures. Enter your answers numerically shparated by commas....
Titrations Part A A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 19.0 mL of HNO3. Express your answer numerically. Part B A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 23.0 mL of NaOH. Express your answer numerically.
180Q2 Calculate the concentrations of all species present (H2CO3, HCO−3, CO2−3, H3O+ and OH−) in 0.019 M H2CO3. pH is 4.04 Express your answers using two significant figures. Enter your answers numerically separated by commas.
For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH. A) 1.6×10−3 M Ca(OH)2 Express your answer using two significant figures. (OH-), (H3O+) Enter your answers numerically separated by commas. pH, pOH. Express your answer to two decimal places. Enter your answers numerically separated by commas. B) 4.9×10−4 M Sr(OH)2 Express your answer using two significant figures. Enter your answers numerically separated by commas: pH, pOH. Express your answer to two decimal places. Enter your answers numerically...
Calculate the concentration of all species (listed below) in a 0.470 M solution of H2SO3. Express your answer using two significant figures. Enter your answers numerically separated by commas. Species: H2SO3], [H2SO3], [HSO−3], [SO2−3], [H3O+], [OH−]
Calculate the pH of the following buffer system. 0.500 M NH3 ( Kb=1.8×10^(-5) ) 0.500 M NH4 Br A. 4.74 B. 9.26 C. 7.00 D.0.30 E. 13.70 I got 4.74