Quest. 4 (15 pts). Ammonia react with water as shown in the following equation: NH3(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...
15:15 When ammonia dissolves in water, make the following equilibrium in NH 3 (aq) + H2O (l) ⇌NH4 + (aq) + OH- (aq) Calculate hydroxidjon concentrationen in the solution formed when 0.10 moles of ammonia dissolved in water to a volume of 500 cm 3 at the temperature the reaction is är k = 1.8 × 10-5.
For the lonization of ammonia shown below, the mixture initially contains 0.500 M NH, (aq). Determine the equilibrium millimolar (mm) concentration of HO- if K. - 1.74 x 10-5. NH3 (aq) + H2O (liq) + NH4+ (aq) + OH- (aq) QUESTION 18 Calculate the concentration of sulfate (SO2-) in a 0.0500 M solution of Nasso, If K = 0.012 for the following reaction: HSO4- (aq) + H20 (lia) = H2O* (aq) + SO42- (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...
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,...
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.
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
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
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,...