Determine the ammonia concentration of an aqueous solution that
has a pH of 11.30. The equation for the dissociation of
NH3 (Kb = 1.8 × 10-5) is
below:
Determine the ammonia concentration of an aqueous solution that
has a pH of 11.30. The equation for the dissociation of
NH3 (Kb = 1.8 × 10-5) is
below:
a)9.0 × 10-3 mol L-1 |
b)2.7 mol L-1 |
c)0.22 mol L-1 |
d)2.0 × 10-3 mol L-1 |
Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation...
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
An aqueous solution of ammonia is prepared (ammonia is weak base). How can we achieve the condition where [NH4+] = [NH3]? NH3 (aq) + H2O (l)-----OH– (aq) + NH4+(aq) A) By decreasing the pH. B) By increasing the pH. C) By heating the solution. D) By diluting the solution with water. E) By concentrating the solution.
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for the ammonia is EQ1: NH3(aq + H2O(l) ßà NH4+(aq) Kb=1.8x10-5 The bismuth(III) ion is precipitated out of the solution as Bi(OH)3. The equilibrium involved is related to the one provided below: EQ2: Bi(OH)3(s) ßà Bi3+(aq) +3OH(aq)- Ksp =3.2x10-40 Manipulate EQ 1 and 2 to solve for the net equation, EQ3: EQ3 (net): 3H2O+ Bi3+(aq) +3NH3(aq) ßàBi(OH)-(s) +3NH4+(aq) Write the mass law expression for the...
The pH of an ammonia, NH3, solution is 9.50. The Kb for ammonia is 1.78 x 10-5?a. Write the balanced chemical equation for the reaction of ammonia with water. b. Write the term for the Kc for this reaction. c. What is the concentration in mol L-1 of ammonia added to water to make this solution at pH 9.5?
What is the pH of 6.0 M aqueous solution of NH3 (ammonia). It's Kb = 1.8 x 10-5.
Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) Kb = 1.77 x 10-5 and Ka = 5.65 x 10-10 a) Calculate the pH of the 0.030 M NH3 solution (Use a labeled ICE table) b) Calculate the pH of the solution at the equivalent point (when equal amount of acid is added. Assume the volume doubles). (Use a labeled ICE table) c) Over which pH range (actual numbers) do you expect...
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)
An aqueous solution of 0.23 M ammonia (NH3) has a pOH of 2.70. Determine the base-dissociation constant (Kb) of ammonia.
Quest. 4 (15 pts). Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l) NH4+(aq) + OH(aq) Kb = 1.77 x 10-4 and Ka = 5.65 x 10-10 a) Calculate the pH of the 0.030 M NH solution (Use a labeled ICE table) b) Calculate the pH of the solution at the equivalent point (when equal amount on added. Assume the volume doubles). (Use a labeled ICE table) c) Over which pH range (actual numbers) do you...
please answer both questions QUESTION 8 The compound ammonia, NH3, is a weak base when dissolved in water. Which of the following is the correct equation for the reaction of ammonia in water? a NH3(aq) + H20(0) NH4(aq) + OH(aq) NH3(aq) + OH(aq) NH2 (aq) + H20(0) NH3(aq) + H20(1) -NH2 (aq) + H30*(aq) NH3(aq) + H200) NH2 (aq) + H30(aq) NH3(aq) + H30aq) NH4+ (aq) + H20(0) QUESTION 9 What is the pH of a solution that is 0.17...