4/15 HW – Acid/Base Review

 

42.       According the Arrhenius, what are the characteristics of acids and bases?

 

43.       How do hydronium ions form? Why do they form in aqueous acid solution?

 

45.       For each of the following reactions, label the acid, base, conjugate acid, and conjugate base.

            a.         NH3 (g) +        H3O+ (aq) à   NH4+ (aq) +     H2O (l)

 

            b.         CH3OH (l) +   NH2- (aq) à    CH3O- (aq) +   NH3 (g)

                       

            c.         OH- (aq) +       H3O+ (aq) à   H2O (l) +         H2O (l)

                       

            d.         NH2- (aq) +      H2O (l) à       NH3 (g) +        OH- (aq)

                       

 

46.       How do binary acids and ternary acids differ?

 

49.       What element is always present in binary acids? What two elements are usually present in ternary acids?

           

54.       Why do we call an aqueous solution of HCl strong and a solution of acetic acid weak?

 

55.       In writing net ionic equations, why are insoluble salts not written as ions?

           

60.       Name the following acids.

            a.         HI

b.                  H2TeO3

c.                   H2Se

d.                  HIO3

 

61.       Write formulas for the following acids.

            a.         phosphorous acid

b.         hydrotelluric acid

c.                   periodic acid

d.                  iodic acid

e.                   hydrochloric acid

 

70.       Give the names and formulas of the salts obtained from complete neutralization reactions between the following acid-base pairs.

            a.         sodium hydroxide + phosphoric acid

b.                  potassium hydroxide + boric acid, H3BO3

c.                   cadmium hydroxide + hydrobromic acid

d.                  lithium hydroxide + silicic acid, H4SiO4

e.                   barium hydroxide + sulfurous acid

 

71.       Reduce the following complete equations to net ionic form.

            a.         6 Cr(NO3)2 + 3 CuSO4 à 3 Cu + 4 Cr(NO3)3 + Cr2(SO4)3

b.                  H2SO4 à H2O + SO3

c.                   P4O10 + 6 H2O à 4 H3PO4

d.                  4 CuCNS + 7 KIO3 + 14 HCl à 4 HCN + 4 CuSO4 + 7 ICl + 7 KCl + 5 H2O

 

35.       What is the hydronium ion concentration of a solution in which the hydroxide ion concentration is 2.77 x 10-10 M? What is the pH of the solution?

           

36.       Determine the hydroxide ion concentration in a solution whose hydronium ion concentration is 4.49 x 10-9 M. What is the pH of this solution?

 

37.       What is the pH of 0.0001 M NaOH?

 

38.       What is the pH of freshly pressed apple juice, if the H3O+ concentration is 1.74 x 10-4 M?

 

39.       What kinds of compounds function as indicators?

 

41.       What volume of 0.196 M LiOH is required to neutralize 25.0 cm3 of 0.413 M HBr?

LiOH + HBr à HOH + LiBr

 

46.       Find the hydroxide ion concentration of a solution with a pOH of 6.13.

 

47.       Using Figure 24.6, calculate pOH for each of the following:

            a.         stomach contents

b.                  beer

c.                   pumpkin pulp

d.                  saliva

e.                   eggs

f.                   bile

 

48.       Calculate the [OH-] for lemon juice, pH = 2.3, and baking soda solution, pH = 8.5.

 

57.       What is a titration? Why is a standard solution necessary for a titration?