Calculate the concentration of OH- at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5)
Calculate the concentration of OH- at equilibrium in the following reaction: NH3 (aq) + H2O (l)...
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 OH- concentration at equilibrium in the following reaction: NH3 (aq) + H20 (1) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5) (1 point) O 1x10^(-14) M O2.7 x10^(-3) M O 7.2 x10^(-6) M O None of the above Question 15 Which of the following pH values indicates the most basic solution? (1 point)* O pH=12 O pH=4 O pH=8 O pH=9
13&14 please! Question 13 Write the equilibrium expression for the following reaction. HCIO4 (aq) -> H+ (aq) + CIO4- (aq) (1 point) * O Ka = ([H +][C104-1)/(HC104) O Ka = [H +)/(HC104] O ka = [H+][C104-1 O None of the above Question 14 Calculate the OH- concentration at equilibrium in the following reaction: NH3 (aq) + H2O (1) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5) (1 point)* O 1x10^(-14) M O2.7 x10^(-3) M O 7.2 x10^(-6)...
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
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...
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.
List the ∆Hºf for the species of the following ionic net equations: NH4+(aq)+ OH-(aq)→H2O(l)+NH3(g) and H+(aq)+OH-(aq)→H2O(l) (sodium hydroxide+ammonium chloride) (sodium hydroxide+hydrochloric acid).
Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) = NH4+ (aq) + OH- (aq) Check all that apply. H2O/NH3 NH4+/NH3 H2O/OH NH4+/OH- Submit Request Answer Part B OH(aq) + HF(aq) = H20(1)+F- (aq) Check all that apply. H2O/F- H20/OH HF/F- HF/OH
Question 10 Which of the following IS a strong acid (1 point ) * H2SO4 HCN HF NH3 Question 11 Write the equilibrium expression for a simple acid ionization. (HA (aq) -> H+ + A-) (1 point ) * Ka = ([H+][A-])/[HA] Ka = [H+]/[HA] Ka = [H+][A-] None of the above Question 12 Write the equilibrium expression for the following reaction. HF (aq) -> H+ (aq) + F- (aq) (1 point ) * Ka = ([H+][F-])/[HA] Ka = [H+]/[HA]...
For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq) Drag the appropriate stresses to their respective bins. Adding NH4+(aq) Adding NH3(g) Adding OH-(aq) Removing NH4+(aq) Removing OH-(aq) Shifts in the direction of the reactants: Shift in the direction of the products: