For the ionization of ammonia shown below, the mixture initially contains 0.500 M NH3 (aq). Determine the equilibrium millimolar (mM) concentration of HO− if Kc = 1.74 × 10−5.
NH3 (aq) + H2O (liq) ⇌ NH4+ (aq) + OH− (aq)
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For the ionization of ammonia shown below, the mixture initially contains 0.500 M NH3 (aq). Determine...
For the lonization of ammonia shown below, the mixture initially contains 0.500 M NH, (aq). Determine the equilibrium millimolar (mm) concentration of HO- if K. - 1.74 x 10-5. NH3 (aq) + H2O (liq) + NH4+ (aq) + OH- (aq) QUESTION 18 Calculate the concentration of sulfate (SO2-) in a 0.0500 M solution of Nasso, If K = 0.012 for the following reaction: HSO4- (aq) + H20 (lia) = H2O* (aq) + SO42- (aq)
4. (3pts) Suppose an aqueous solution initially contains one mole of hydrochloric acid and one mole of ammonia. Which of the following statements best describes the solution once it comes to equilibrium? A. The solution is neutral because the ammonia neutralizes the hydrochloric acid. B. The solution is highly acidic due to the ionization: HCl (aq) + H+ (aq) + CI+ (aq) C. The solution is slightly acidic due to the equilibrium: NH4+ (aq) = NH3 (aq) + H+ (aq)...
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...
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...
Given the equilibrium constants for the equilibria, 2 NH4+(aq) + 2 H2O(ª) 2 NH3(aq) + 2 H3O+(aq); Kc = CH3COOH(aq) + H2O(ª) CH3COO−(aq) + H3O+(aq); Kc = determine Kc for the following equilibrium. CH3COOH(aq) + NH3(aq) CH3COO−(aq) + NH4+(aq) a. 3.08 × 104 b. 9.96 × 10-15 c. 3.25 × 10-5 d. 1.75 × 10-5 e. 1.00 × 1014
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
NH3(aq) + H20(1) = NH4+(aq) + OH-(aq) NH3(aq)...
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C? Express your answer using two significant figures.
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 M CO and 0.150 M H2O. What will be the equilibrium concentration of [CO2]? What will be the equilibrium concentration of [H2]?
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....
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...