onsider the reaction of NH3 with water: NH3 + H2O ↔ NH4+ + OH- (Kb=Kw/Ka) and...
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 50.00 mL of 0.200M NH3 after the addition of 55.00 mL of 0.200M HCl.
Homework Answers
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onsider the reaction of NH3 with water:
NH3 + H2O ↔ NH4+ + OH- (Kb=Kw/Ka)
and...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF)...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2...
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...
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) +...
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...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
What is the pH of NH4C2H3O2 given information below? HC2H3O2⇌H+ + C2H3O2- Ka=1.76*10^-5 pKa=4.75 NH3+H2O⇌NH4+ +...
What is the pH of NH4C2H3O2 given information below? HC2H3O2⇌H+ + C2H3O2- Ka=1.76*10^-5 pKa=4.75 NH3+H2O⇌NH4+ + OH- Kb=1.79*10^-5 pKb=4.75 Assume initial concentration of NH4C2H3O2 is 0.100 M Use quadratic formula if necessary
Quest. 4 (15 pts). Ammonia react with water as shown in the following equation: NH3(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...
A) A 75.0mL- volume of 0.200M NH3 (Kb= 1.8*10^-50 is titrated with 0.500HNO3. Calculate the pH after the addition of 1...
A) A 75.0mL- volume of 0.200M NH3 (Kb= 1.8*10^-50 is titrated with 0.500HNO3. Calculate the pH after the addition of 17.0mL of HNO3 . B) A 52.0mL- volume of 0.35M CH3COOH(Ka-1.8*10^-5) is titrated with 0.40M NaOH. Calculate the pH after the addition of 33.0mL of NaOH. Thank you!!!!
Calculate Ka for 1 M NaCH3COO pH = 9.37 H+ = 4.203 X 10^-10 OH- =...
Calculate Ka for 1 M NaCH3COO pH = 9.37 H+ = 4.203 X 10^-10 OH- = 2.402 X 10^-5 CH3COO- = 1.00 X 10^0 CH3COOH = 2.402 X 10^-5 ________________ Calculate Ka using the formula Kw = Ka X Kb and the appropriate equilibrium constant for 1 M NaCH3COO. NaCH3COO ---> Na+ (neutral) + CH3COO-. Is the conjugate base for CH3COOH. CH3COOH Ka1 = 1.8 X 10^-5 ______________________ Calculate Ka for 1 M NH4Cl pH = 4.26 H+ = 2.336...
calculate the pH when 50.0 mL of 0.4 M NH3 is mixed with 5.00 mL of 0.8 M HCl. ( The ka of ammonia is 1.77 x10^-5.)...
calculate the pH when 50.0 mL of 0.4 M NH3 is mixed with 5.00 mL of 0.8 M HCl. ( The ka of ammonia is 1.77 x10^-5.) KaKb=Kw (Ka)(Kb)=1.00 x 10^-14
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
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...
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