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).
Part A: Calculate the pH of 0.61 M NH3 (Kb=1.8×10−5). Part B: Calculate the concentrations of...
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+] = ?,?,?,?
Calculate the pH and percent dissociation of 0.25 M NH3, Kb = 1.8 × 10^–5
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.
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
38. A buffer solution is 0.40 M NH3 and 0.60 M NHACI. Kb for NH3 is 1.8 x 10-5 a) Calculate the pH for the buffer system. b) Calculate the pH of the solution after adding 0.00600 moles of NaOH to 400.0 mL of the buffer. c) Calculate the pH of the solution after adding 0.050 moles of HCl to 600.0 mL of the buffer.
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
Part A Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. pH of 0.500 M ammonia solution is 11.48 What is the percent ionization of ammonia at this concentration? Express your answer with the appropriate units.
Calculate the PH of a 0.36 M aqueous solution of NH4NO3. Kb of NH3= 1.8 x10^-5. Please show your work; I know how to do a normal problem but I am confused because the Kb is only for NH3, not the whole thing. Thanks!
Ammonia, NH3, is a weak base with a Kb value of 1.8×10^−5. Part A What is the pH of a 0.370 M ammonia solution? Part B What is the percent ionization of ammonia at this concentration?
Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. Part A What is the pH of a 8.50×10−2 M ammonia solution? Part B What is the percent ionization of ammonia at this concentration?