Listen What is the pH of a solution containing a proton (hydronium ion) concentration of 2.7 x 109 M? Is the solution acidic, basic, or neutral? What is the pOH and what is the hydroxde ion concentration (i.e., [OH]) of this solution?

Write equations that show H2PO4- acting both as an acid and as a base.

You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.

Write a formula for the conjugate base formed when each of the following behaves as a Brnsted acid: a. HSO3 b. HPO42 c. HClO3 d. CH3NH3+ e. H2C2O4

For which of the following solutions must we consider the ionization of water when calculating the pH or pOH? (a) 3108M HNO3. (b) 0.10 g HCl in 1.0 L of solution. (c) 0.00080 g NaOH in 0.50 L of solution. (d) 1107M Ca(OH)2. (e) 0.0245 M KNO3

Solution A has a pH of 2.0. Solution B has a pH of 5.0 Which solution is more acidic? Based on the H+ ion concentrations in the two solutions, how many times more acidic?

Which of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH] > 1.0 X IO’7M

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.

Use Table 14.3 to help order the following acids from strongest to weakest HNO3,H2O,NH4+,C5H5NH+

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