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16 Nov 2019
Calculate the pH of a 0.500L of a 0.200 M NH^+_4 -0.200 M NH_3 buffer before and after the addition of 0.0050 mol NaOH. Assume the volume remains constant. Consider the titration of 100.0 ml of 0.016 M HOCl (K_a = 3.5 times 10^-8) with 0.040 M NaOH. Calculate the pH: a) After addition of 10.0 ml of 0.0400 M NaOH b) Halfway to the equivalence point c) At the equivalence point In a 0.15 M NH_3, the pH is 11.21 and the percent dissociation is 1.1%. Calculate the concentrations of all species present, the pH, and percent dissociation of ammonia in a solution that is 0.15 M in NH_3 and 0.45 M in NH_4 CI. Calculate the pH of 5.0 times 10^-5 M Ba(OH_2). Calculate the pH of 0.010 M Benzoic Acid at 25 degree C where K_a = 6.3 times 10^-5 at 25 degree C. Calculate the pH of a 0.050 M solution of CH_3 CO_2 Na where K_a = 1.8 times 10^-5 at 25 degree C.
Calculate the pH of a 0.500L of a 0.200 M NH^+_4 -0.200 M NH_3 buffer before and after the addition of 0.0050 mol NaOH. Assume the volume remains constant. Consider the titration of 100.0 ml of 0.016 M HOCl (K_a = 3.5 times 10^-8) with 0.040 M NaOH. Calculate the pH: a) After addition of 10.0 ml of 0.0400 M NaOH b) Halfway to the equivalence point c) At the equivalence point In a 0.15 M NH_3, the pH is 11.21 and the percent dissociation is 1.1%. Calculate the concentrations of all species present, the pH, and percent dissociation of ammonia in a solution that is 0.15 M in NH_3 and 0.45 M in NH_4 CI. Calculate the pH of 5.0 times 10^-5 M Ba(OH_2). Calculate the pH of 0.010 M Benzoic Acid at 25 degree C where K_a = 6.3 times 10^-5 at 25 degree C. Calculate the pH of a 0.050 M solution of CH_3 CO_2 Na where K_a = 1.8 times 10^-5 at 25 degree C.
Hubert KochLv2
11 Aug 2019