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 |
Given the equilibrium constants for the equilibria, 2 NH4+(aq) + 2 H2O(ª) 2 NH3(aq) + 2...
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?
For which of the following reactions will the reactants be favored at equilibrium? NH3(aq) + H30+ (aq) = NH4+ (aq) + H20(1) CO32- (aq) + H30+ (aq) = HCO3(aq) + H2O(1) CH3COOH(aq) + OH(aq) = CH3COO" (aq) + H2O(1) HSO3- (aq) + H3O+ (aq) =H2SO3(aq) + H2O(1) CIOA" (aq) + H3PO4(aq) = HCIO4(aq) + H2PO4" (aq)
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.
For the reaction NH3(aq) + H+ (aq) ⇋ NH4 + (aq), at 20°C the equilibrium concentrations were as follows: [NH3] = 2 x 10-4 M; [H+ ] = 2 x 10-4 M; and [NH4 + ] = 18 M. Calculate the equilibrium constant for the reaction.
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)
Consider these two equilibria with their respective equilibrium constants: (1) (2) PbCl2 ()Pb2+ (aq)2CI- (aq) Pbf2 (s) РЬ2+ (aq) + 2 F-(aq) K 1.7x 10-5 K-37x10-8 Which equilibrium will produce more Pb2+ions in solution? B) (2) D) cannot determine with provided information C) both (1) and (2) will produce the same amount
1. Given the two equilibria below, Ag(NH3)2(aq) = Agt(aq) + 2NH3(aq); Kd = 5.9 x 10-8 AgBr(s) Ag+(aq) + Br" (aq); Ksp = 5 x 10-13 what is K, for the following equilibrium? AgBr(s) + 2NH3(aq) = Ag(NH3)2(aq) + Br" (aq) a. 3 x 10-20 b.2.7 x 100 c. 7.2 x 10-11 d. 8.5 x 10-6 e. 1.2 x 105
Calculate the concentration of OH- at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5)
Given the following equilibrium equations and their corresponding equilibrium constants: 2CO2 (g)+H2O(g)⇌2O2 (g)+CH2CO(g) Kc=6.1x108 CH4(g)+2O2(g)⇌CO2 (g)+2H2O(g) Kc=1.2x1014 Find Kc for the reaction: CH4(g) + CO2(g) ⇌ CH2CO (g) + H2O (g) 2 of 5 .. .........e following equilibrium equations and their corresponding equilibrium constants: 2 CO2 (g) + H20 (g) – 202 (g) + CH2CO (g) Kc = 6.1 x 108 CH2(g) + 2 O2(g) - CO2 (g) + 2 H2O(g) Kc = 1.2 x 1014 Find Kc for the...
All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+, NH3 CH3COOH, CH3COO- H3O+, OH- HPO42-, PO43- The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid? Group of answer choices 4.7 x 10-5 4.1 x 10-7 3.4 x 105 2.4 x 10-4 1.3 x 10-5 You have 250.0 mL of a 0.56 M solution of NaCH3COO. How many milliliters of a 0.50...