Which of the following statements is true concerning a 0.50 M hydrozine N2H4 solution of 30.0 ml titrated with 0.50 M HCI solution. Kb( N2H4 ) = 1.7 x 10-6. Note that the conjugate acid of N2H4 is N2H5*. a. Before titration, [OH" ] > [N2H4 ] in the 0.50 M N2H4 solution. b. After adding 5.00 ml HCl into the 0.50 M N2H4 solution, (N2H5*)>[N2H4] in the solution. OC. After adding 15.0 mL HCI into the 0.50 M N2H4 solution, [ N2H5* ] = [ N2H4] in the solution. d. After adding 25.0 ml HCI into the 0.50 M N2H4 solution, [N2H5*) < [ N2H4] in the solution. e. After adding 30.0 mL HCI into the 0.50 M N2H4 solution, [ H30*] = [OH" ] in the solution.

35 A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K² of bases at 25 °C tables for additional information. a Part 1 of 4 0.00 mL Added, pH = Part 2 of 4 10.0 mL Added, pH = x10 X x10 X

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Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH1) was added to 1.000 L of the buffer solution. The new concentrations are [HC2H3O2] = 0.4900 M and [C2H3021] = 0.7100 M. The Ką = 1.60 x 105. %3D %3D everything is based upon the acid dissolving in water: HC2H3O2 + H20 C2H3O21 + H3O*1 [ Ка solve for [H30*l] then put in the numbers Ka [ [H30*1] = [H3O*1] = pH = - log a. H30*1 b. Он1 c. H2C6H606 d. HC6H6O61 е. HSO31 f. SO3? -2 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS1 I. s2 m. HX n. X-1 О. 1 р. 2 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 х 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 х. 5.5 х 10-2 у. О.7000 z. 1.60 x 10-5 аа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957