# pH of solution

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4.) Determine the concentrations of hydronium and hydroxide ions in 0.0403 M aqueous sodium hydroxide. Kw = 1.0E-14.

A.) Hydronium ion concentration?(answer in M)

B.) Hydroxide ion concentration?(answer in M)

6.) Concentrated aqueous HClO4 has a concentration of 14.8 M. Calculate the concentrations of all ions present in a solution prepared by pipetting 8.04 mL of concentrated HClO4 into a 1000. mL volumetric flask and filling to the mark.

A.) Hydronium ion concentration? (answer in M)

B.) Perchlorate ion concentration?(answer in M)

C.) Hydroxide ion concentration? Kw = 1.0E-14. (answer in M)

8.) Calculate the concentrations of hydronium and hydroxide ions in a solution prepared by dissolving 0.307 g of solid NaOH in enough water to make 225 mL of solution. Kw = 1.0E-14.

A.) Hydronium ion concentration?(answer in M)

B.) Hydroxide ion concentration?(answer in M)

10.) Convert each of the following H3O+ concentrations to pH.

A.) 1.65 M

B.) 2.84 µM

C.) 0.0245 M

D.) 0.000526

12.) Convert each of the following OH- concentrations to pH.

A.) 2.0 M

B.) 2.8 µM

C.) 0.038M

D.) 00064M

14.) Convert each of the following pH values to a hydronium ion concentration.

A.) 1.33 (answer in M)

B.) 3.31 (answer in M)

C.) 9.88 (answer in M)

D.) 11.16 (answer in M)

16.) Convert each of the following pH values to a hydroxide ion concentration. Kw = 1.0E-14.

A.) 1.11 (answer in M)

B.) 3.63 (answer in M)

C.) 9.31 (answer in M)

D.) 11.03 (answer in M)

18.) Calculate the pH of a 0.055 M solution of the following compounds

A.) NH3. Kb(NH3) = 1.7E-5.

B.) HClO. Ka(HClO) = 4.0E-8.

C.) HCN. Ka(HCN) = 6.2E-10.

24.) What is the percent ionization of a 0.0477 M aqueous solution of cyanic acid, HCNO (Ka = 3.5E-4)? (answer in %)

28.) Determine the percent ionization of a solution of boric acid that is 66 mM (Ka = 5.4 × 10-10). (answer in %)

34.) For each weak acid, identify its conjugate base. For each weak base, identify its conjugate acid. For ions, put the charge in parentheses, if the charge is more than one, put the multiple first, then the sign. No phase is needed for this question.

A.) NH3

B.) HCLO

C.) HCN

44.) List the following in order of increasing pH of their 0.25 M solutions: NH4Cl, MgCl2, HCl, NaOCl, C6H5NH3Cl and NaClO2. (See Appendix E for K values.)

58.) Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.669 M solution of N2H4.

60.) The addictive painkiller morphine, C17H19NO3, is the principal molecule in the milky jiuce that exudes from unripe poppy seed capsules. Calculate the pH of a 0.0232 M solution of morphine, given that Kb = 7.9E-7.

(look up chemical formula)(internet?)

62.) The pH of a 0.0429 M solution of a weak acid is 2.752. What is the Ka of the acid?

64.) The pH of a 0.0366 M solution of a weak acid is 2.477. What is the percent ionization of the acid?

68.) What is the pH of a 0.0565 M solution of NH4Cl?

74.) What is Keq for the following reaction: HPO42-(aq) + H3O+(aq) --> H2PO4-(aq) + H2O(l)

Some possibly useful equilibrium constants are: 6.9E-3, 6.2E-8, and 4.8E-13, for the Ka1, Ka2, and Ka3 of phosphoric acid.

#### Solution Summary

The solution is comprised of detailed explanations on the topic of pH of the solutions, concentrations of ions, etc.