Given the solution 0.50 M NH3 (aq) with Kb = 1.75 * 10-5, calculate the pH using an I.C.E. table
The solution is given below-
The approximation we made is viable only if less than 10% or 15%
base is ionized,This criterion is arbitrary one as it applies only
if Kb is smaller than about 0.01 C i.e smaller than about when
C=0.01M,
at C=0.1M
and so on.The error introduced under these conditions is less than
5%.So it is quite a good approximation rather than to solve a
hectic quadratic equation.
Given the solution 0.50 M NH3 (aq) with Kb = 1.75 * 10-5, calculate the pH...
the Kb of ammonia (NH3) at 25.0 C is 1.75 x 10-5. Calculate the pH of a 0.0321 M aqueous solution of NH4Cl
Calculate the pH of a 500.0 mL solution that is 0.30 M NH3 and 0.50 M NH4Br. For NH3, Kb = 1.76 × 10-5 .
What is the pH of a 1.0028 M ammonia solution given that Kb =
1.80E-5?
NH3 (aq) + H2O (l) --> OH1- (aq) + NH41+ (aq)
What is the pH of a 1.0028 M ammonia solution given that Kb = 1.80E-5? NH3 (aq) + H20 (1) --> OH1- (aq) + NH41+ (aq)
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...
Find the pH of the following : 0.50 M solution of a base with a Kb = 1.75 x 10-4
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.
Calculate the pH of a 0.401 M solution of NH4Br (Kb of NH3 = 1.8 x 10-5). Enter pH to 2 decimal places.
find pH when a 500.0 mL solution has 0.30 M NH3 and 0.50 M NH4Br. For NH3, Kb = 1.76 × 10-5 .
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).
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200 M of NH4Cl(aq). The Kb of NH3(aq) is 18 x 10-5. Consult Textbook Numerical Answer pH b) Calculate the change in pH when 6.00 mL of 100 M HCl is added to 100.0 mL of the buffer solution. Numerical Answer: c) Calculate the change in pH when 6.00 mL of o.100 M NaOH is added to 100.0 mL of the buffer solution. Numerical Answer: