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- 3. 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.What is [H3O+] in a solution obtained by dissolving 205 mL HCl(g), measured at and 23oC and 751 mmHg, in 4.25 L of aqueous solution? (R: 0,08206 L.atm/mol.K)Single choice.Ammonia can react as an acid or a base. a) What is the conjugate acid of ammonia? b) What is the conjugate base of ammonia? c) arist dit ons servbed as Complete the following acid-base reaction in which NH3(e) acts as both an acid and a base: OcH 6 HOONH3() + NH3() = OOH (d FOZH (s *АНИ (1 sqz ions to biosqu adtavið
- 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 + H2OWhich is the stronger acid, H2SO4 or H2SeO4? Why?What is [H3O+] in a solution obtained by dissolving 205 mL HCl(g), measured at and 23oC and 751 mmHg, in 4.25 L of aqueous solution? (R: 0,08206 L.atm/mol.K
- H2AO4 is a weak acid. What is [AO42 in a 0.30 M H2AO4 solution? [Ka1 = 6.2 x 10-; Ka2 = 5.2 x 10-10 OA21 x 10-5 M OB 5.2 x 10-7 M OC0.60 M OD 6.2 x 10-7 M OE 0.30 M OF 6.2 x 10-10 M OG5.2 x 10-10 MOf the hydrogen halides, only HF is a weak acid. Give a possibleexplanation.Fill in the left side of this equilibrium constant equation for the reaction of diethylmethylamine (C3H13N), a weak base, with water. D= K, olo
- Which of the following compounds will form a solution with water that slightly conducts electricity (dim light bulb)? O 0.01 M CH;COOH O 0.01 M CH3OH O 0.01 M CCI4 0.01 M NHẠNO3 O 0.01 M O2For 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 = 3.36Consider a weak acid "HA". What is the pH of a 0.957 mol L-1 solution of HA? The KA of HA is 7.09 x 10-7 .