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Q: NH3 contains no OH- ions, and yet its aqueous solutions are basic. Explain why?
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Q: 6. Identify the Lewis acid and Lewis base in the reaction: Co*(aq) + 6NH3(aq) Co(NH;)* (aq)
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- For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.363. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.Based on the Lewis structures of the reactants and product of the following equation, identify the Lewis acid and the Lewis base in it: CO, + OH → HCO, =c=0: + :0-H H-0- O: O Lewis acid: CO,; Lewis base: HCO, O Lewis acid: OH; Lewis base: CO, O Lewis acid: CO; Lewis base: OH-
- 6. Identify the Lewis acid and Lewis base in the reaction: Co³* (aq) + 6NH;(aq) = Co(NH;);*(aq)Calculate the pH of 0.400 M solution of ascorbic acid, HC6H;O6. (Ka of ascorbic acid = 6.80 x 105)Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin itcauses the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of methemoglobin whichcannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base.C6H5NH2 (aq) + H2O (ℓ) ⇋ C6H5NH3+ (aq) + OH- (aq)a. When you measure the concentrations of the ionized substances you find them to be:[C6H5NH2] = 0.234 mol/L [C6H5NH3+] = 2.8 x 10-5 mol/L [OH-]= 2.8 x 10-5 mol/LIf the Kb is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (rightor left) to reach equilibrium? Explain. b. At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L [C6H5NH3+] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 mol/LIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when…
- Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions. (a) CsBr; (b) Al(NO3)3; (c) KCN; (d) CH3NH3Cl3. For the following acid - base reaction, (a) predict the products; (b) identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base; (c) use curved arrows to show the flow of electron pairs in the reaction. CH3 CH2C-OH + NaNHawhats the base and acid of this reaction CsF + SF4 → Cs+[SF5]–
- Rank the following acids in order of increasing strength: (a) HClO4, H3PO4, H2SO4; (b) H3PO4, H3AsO4, H3SbO4; (c) HOF, HOCl, HOBr, HOI; (d) HOCl, HClO2, HClO3, HClO4; (e) CH3CO2H, CF3CO2H, CCl3CO4H;Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2O9) a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; + H;O* H¿CO; + H2O (aqueous solution) b) Phenol (HC&H50) is a weak acid (Ka= 1.5 x 10*). Write the equilibrium chemical equation, equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol. 10) Blood is mainly buffered by HCO; /H2CO; (H2CO3, Carbonic Acid, K= 4.4x10 -") buffer system. Calculate the pH of human blood for a carbonic acid concentration of 0.091M and HCO; concentration of 1.00M.