Which 0.10 M solution would you expect to have the largest [H+]? Multiple Choice   HF              (Ka = 6.8 x 10-4)   HC2H3O2   (Ka = 1.8 x 10-5)   HC3H5O2   (Ka = 1.3 x 10-4)   HCN           (Ka = 4.9 x 10-10)   HCOOH     (Ka = 1.8 x 10-4)

Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?

Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric acid) b. HC2H3O2 (acetic acid) c. H2C5H6O4 (glutaric acid) d. HCN (cyanic acid)

Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?

8-45 Describe how you would prepare each of the following solutions (in each case, assume that the base is a solid). (a) 400.0 mL of 0.75 M NaOH (b) 1.0 L of 0.071 M Ba(OH)2 (c) 500.0 mL of 0.1 M KOH (d) 2.0 L of 0.3 M sodium acetate

8-41 What is the [OH-] and pOH of each solution? (a) 0.10 M KOH, (b) 0.10 M Na2CO3, (c) 0.10 M Na3PO4, (d) 0.10 M NaHCO3,

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.

The active ingredient formed by aspirin in the body is salicylic acid, C6H4OH(CO2H). The carboxyl group. (-CO2H) acts as a weak acid. The phenol group (an OH group bonded to an aromatic ring) also acts as an acid but a much weaker acid. List, in order of descending concentration, all of the ionic and molecular species present in a 0.001-M aqueous solution of C6H4OH(CO2H).

. Choose the answer that best completes the following statement and defend your answer. When 100.0 mL of water is added to 100.0 mI of 1.00 M HCI. a. the pH decreases because the solution is diluted. b. the pH does not change because water is neutral. c. the pH is doubled because the volume is now doubled. d the pH increases because the concentration of H decreases e. the solution is completely neutralized.

Which of the solutions listed below has the lowest pH? (a) 0.10 M HCl (b) 0.10 M NaOH (c) 2.5 105 M HNO3 (d) pure H2O