38-What is the [H3O+] for a solution with a [OH-] = 4.8 x 10^-2 M? a- 2.1 x10^-13 M b-1.0 x 10^-14 M c-2.0 x 10^-12 M d- 1.32 M e-12.68 M

Draw a curve similar to that shown in Figure 14.23 for a series of solutions of NH3. Plot [OH-] on the vertical axis and the total concentration of NH3 (both ionized and nonionized NH3 molecules) on the horizontal axis. Let the total concentration of NH3 vary from 11010M to 1102M.

Calculate the concentration of all solute species in each of the following solutions of acids or bases. Assume that the ionization of water can be neglected, and show that the change in the initial concentrations can be neglected, Ionization constants can be found in Appendix H and Appendix I. (a) 0.0092 M HCIO, a weak acid. (b) 0.0784 M C6H5NH2, a weak base. (c) 0.0810 M HCN, a weak acid. (d) 0.11 M (CH3)3N, a weak base. (e) 0.120 M Fe(H2O)62+ a weak acid, Ka=1.6107

Write a balanced chemical equation for the dissociation in water of each of the salts listed in Problem 10-131. a. NaCl b. Mg(NO3)2 c. K2S d. NH4CN

8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate (c) KOH (d) Ammonia (e) Water

Consider the following six beakers. All have 100 mL of aqueous 0.1 M solutions of the following compounds: beaker A has HI beaker B has HNO2 beaker C has NaOH beaker D has Ba(OH)2 beaker E has NH4Cl beaker F has C2H5NH2 Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more Information required). (a) The pH in beaker A the pH in beaker B. (b) The pH in beaker C the pH in beaker D. (c) The % ionization in beaker A the % ionization in beaker C. (d) The pH in beaker B the pH in beaker E. (e) The pH in beaker E the pH in beaker F. (f) The pH in beaker C the pH in beaker F.

Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.

A solution has a [OH1-] = 4.20 x 10-4 M. Use the self ionization constant of water (Kw) to find the [H3O1+]. Note: Kw = 1.00 x 10-14 answer choices [H3O1+] = 1.28 x 10-7 M [H3O1+] = 2.27 x 10-4 M [H3O1+] = 2.56 x 10-3 M [H3O1+] = 2.38 x 10-11 M [H3O1+] = 3.03 x 10-13 M

Indicate whether each of the following solutions is acidic, basic or neutral: a) [H3O+] = 1.7 x 10-11 Mb) [H3O+] = 6.8 x 10-5 Mc) [OH-] = 5.9 x 10-8 Md) [OH-] = 1.0 x 10-7 Me) [OH-] = 7.5 x 10-3 M

Calculate the [OH-] of each aqueous solution with the following [H3O+], and then identify the solution as acidic, basic or neutral: a) [H3O+] = 9.1 x 10-10 Mb) [H3O+] = 6.4 x 10-7 Mc) [H3O+] = 4.3 x 10-4 Md) [H3O+] = 7.0 x 10-8 Me) [H3O+] = 2.1 x 10-3 M