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 aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2...
This question pertains to the pH of a weak acid/weak base salt combo. For an aq solution of NH4NO2, these are the combinations of reactions that are possible. (1) NH4+(aq) + NO21-(aq) ⇆ NH3(aq) + HNO2(aq)____________K1 = ? (2) NH4+(aq) + H2O(l) ⇆ H3O+(aq) + NH3(aq)_______________Ka = 5.6 x 10-10 (3) NO21- + H2O(l) ⇆ HNO2(aq) + OH-(aq)_________________Kb = 2.2 x 10-11 (4) 2H2O(l) ⇆ H3O+(aq) + OH-(aq)_________________________Kw =1.0 x 10-14 Write the symbolic expression for the equilibrium constants...
PART A is already solved. It is provided for context for you :) PART A: If you have a initial conc. 0.10M NH4NO2, make an ICE table, solve for concentration of NH4+, NO2-, NH3 and HNO2.K1 value is 1.23e-6 NH4+NO2<=>NH3+HNO2 [NH4] and [NO2] both are 9.99e-2 M [NH3] and [HNO2] were found to be 1.11e^-4 M PART B (the part I need help with): Using the values you found in part A (conc. of NH4 and NH3), find the value...
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...
12. The pK, for NH4 is 9.26. This expression refers to which of the following reactions? A. NH4+ (aq) + OH(aq) + NH3(aq) + H2O(aq) B. NH4+ (aq) + H2O(l) NH3(aq) + H30+(aq) C. H3O+(aq) + OH(aq) → 2H2O(1) D. NH3(aq) + H30+(aq) NH4+ (aq) + H2O(l) E. NH3(aq) + H2O(1) NH4+ (aq) + OH (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...
Aqueous solutions of ammonia (NH3) and hydrogen cyanide (HCN) react to produce ammonium cyanide, (NH4CN) according to the following equilibrium reaction. NH3(aq) + HCN(aq) = NH4+ (aq) + CN (aq) Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (Kw - 1.01 x 10-14) NH4+ Ka = 5.6 x 10-10 HCN ka = 4.0 x 10-10 reaction is product favored, K<1 reaction is neither reactant nor product favored reaction is product favored, K>1 reaction...
Aqueous solutions of ammonia (NH3) and hydrogen cyanide (HCN) react to produce ammonium cyanide, (NH4CN) according to the following equilibrium reaction. NH3(aq) + HCN(aq) = NH4+ (aq) + CN (aq) Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (Kw = 1.01 x 10-14) NH4* Ka = 5.6 x 10-10 HCN Ka = 4.0 x 10-10 reaction is reactant favors, K> 1 O reaction is reactant favors, K <1 O reaction is product favored,...
Consider the following reaction: HNO2 (aq) + HPO42-(aq) ⇌ NO2-(aq) + H2PO4-(aq) a.)Identify the Brønsted-Lowry acids and bases in the forward reaction b.)State the conjugate pairs for the above reaction. Be specific. Identify the acids and bases in the following reactions and identify the conjugate pairs. HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq) CH3NH2(aq) + H2O(l) ⇌ OH-(aq) + CH3NH3+(aq) HCO3-(aq) + HSO4-(aq) ⇌ H2CO3(aq) + SO42-(aq) Complete the following reactions: ____________(aq) + Br-(aq) ⇌ NH3(aq) + HBr(aq) CH3COOH(aq) +...
A. Answer the following questions considering the 4 aqueous solutions below. Each contains 100.0 mL of the following solutions: Solution A = 0.10 M HBr Solution B = 0.10 M HNO2 Solution C = 0.10 M NaOH Solution D = 0.10 M NH3 Fill in the blanks with GT (greater than), ET (for less than) or EQ (for equal to). 1. ________ pH of A pH of B. 2. ________ pH of B ____________ 1. 3. ________ pH of C...
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)...