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A: pH = - log[H3O+] = - log(6.330×10-5) =5-log(6.330) = 4.20
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Determine the pH of a 0.16M NH3 where kb = 2.4 x 10-6
follow the format:
a) [OH-] in 0.16M NH3
b) pOH
c) pH
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- Calculate the molar concentration of OH- in a 0.075 M solution of ethylamine 1C2H5NH2; Kb = 6.4 * 10-42. Calculate the pH of this solution.(b) What is the pH of 0.39 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 10-4.)THE X IS SMALL APPROXIMATION The initial concentration and Ka of several weak acid (HA) solutions are listed. For which solution is the x is small approximation least likely to work in finding the pH? (a) initial [HA]=0.100 M; Ka=1.0*10-5 (b) initial [HA]=1.00 M; Ka=1.0*10-6 (c) initial [HA]=0.0100 M; Ka=1.0*10-3 (d) initial [HA]=1.0 M; Ka=1.5*10-3
- Q2-3:(a) Given that Kb for ammonia is 1.8 X 10 -5 and that for methylamine is 4.4 X 10 -4, which is the stronger base? (b) which is the stronger acid ,the ammonium ion or the methylammonium ion ? (c) calculate the Ka for NH,* and CH;NH;* + Q2-4: A particular sample of vinegar has a pH of 2.90, assuming that the vinegar contains only acetic acid (Ka acetic acid in vinegar . 1.8 X 10 -5), calculate the concentration of Q2-5: Calculate the molar concentration of OH-ions in an 0.85M solution of hypobromite ion , BrO- (Kp 4.0X10-6) .what the pH value of this solution?The equilibrium constant, K, for a neutralization reaction can be symbolized as Kn- Determine K, at 25 °C for the reaction NH, (aq) + HB1O(aq) = NH†(aq) + BrO¯(aq) using Kw, and the K, and K, values from the ionization constant tables. Kn ||Abbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2 in each of the following solutions: (a) 0.100 M H2M; (b) 0.100 M NaHM; (c) 0.100 M Na2M. For (b), use the approximation 3HM24 < 0.100 M.
- + 2) HA is a weak acid. HA is dissociated to H and A in water. At equilibria, if the pH of the solution is 3.24, then what is the concentration of A. [A [H*] At what condition, pH = pka? 3) pH = pKa + logDetermine the pka of an acid whose concentration is 0.100M and pH is 2.86.Calculate the concentration of the following weak acids. 2) a) ethanoic acid with pH 4.53 (Ka = 1.74 x 10° mol dm) b) pentanoic acid with pH 3.56 (pK, = 4.86) -5
- Calculate the PH of 0.15 molesdm-3 of benzoic acid (c6h5COOh) Ka of benzoic acid = 6.3x10-5(a) Calculate [OH-] of a 4.40×10-1 M aqueous solution of triethylamine ((C2H5)3N, Kb = 4.0×10-4). (b)Calculate the pH of the above solution.(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .