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 NH3(aq)/NH4+(aq) to behave as a buffer?
Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l) NH4+(aq) +...
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...
onsider the reaction of NH3 with water: NH3 + H2O ↔ NH4+ + OH- (Kb=Kw/Ka) and also NH4+ + H2O ↔ NH3 + H3O+ (Ka = 5.70×10-10) be sure to show all work including the ICE Tables. a) Find the pH of 50.00 mL of 0.200M NH3 after the addition of 45.00 mL of 0.200M HCl. b) Find the pH of 50.00 mL of 0.200M NH3 after the addition of 50.00 mL of 0.200M HCl. c) Find the pH of...
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2 k1? NH4+ + H2O -> H3O+ + NH3. ka = 5.6 x 10^-10 NO2- + H2O -> HNO2 + OH- kb =2.2 x 10^-11 2H2O -> H3O+ + OH- kw = 1.0 x10^-14 Write symbolic expression for equilibrium constants for each reaction. Derive expression for k1 in terms of ka, kb, and kw; find numerical value of k1.
The equlibrium constant for the equation NH3(aq) + H2O(l) ↔ NH4+(aq) + OH⁻(aq) is Kb= 1.8×10-5 at 25 ºC. Calculate ΔGºrxn at 25 ºC. a) -2.27 kj/mol b) 0 kj/mol c) 2.27 kj/mol d) 267 J/mol 27.1 kj/mol
NH4+(aq) + H2O (l) BLUE <--GREEN--> NH3(aq) + H3O+(aq) YELLOW NH4+ + H2O= Blue. NH3 + H3O = Yellow. Mix is green at equilibrium. Q: When adding sodium hydroxide solution, the color of the equilibrium mixture changed from green ---> yellow. a. In which direction did the equilibrium shift? (L) left or (R) right b. Explain answer to a. Which ion was added or removed from the equilibrium mixture?
1) Calculate the OH- concentration at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5). (a) 1 x10^(-14) M (b) 2.7 x10^(-3) M (c) 7.2 x10^(-6) M (d) None of the above 2) Which of the following pH values indicates the most basic solution? (a) pH=12 (b) pH=4 (c) pH=8 (d) pH=9 3) Which of the following pH values indicate the most acidic solution? ( (a) pH=11 (b) pH=2...
Calculate the concentration of OH- at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5)
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)...
Please show all your work for the problems! Exp Composition Total Vol pH 1 A few mL of 0.10M NH3 (unchanged) n/a 11.13 2 2.5mL 0.1M NH3 & 7.5mL H2O 10 ml 10.82 3 2.5mL 0.1M NH4Cl & 7.5mL H2O 10 ml 6.01 4 2.5mL 0.1M NH3 & 2.5mL 0.1M NH4Cl & 5mL H2O 10 ml 9.26 5 Take 1mL Solution #4 and add 9mL of water 10 ml 9.26 Solution 1. Use the concentration of NH3 and the measured...
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)