Acid Base Chemistry Practice Test - Answer Key

 

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  1. A saturated solution of calcium hydroxide has a pH of 12.25.  What is the concentration of calcium ions in this solution?

    [Ca2+] = 8.9 x 10-3 M

     

     

  2. HCl gas in a 1.21-L cylinder at 0.870 atm and 28.0oC.  The volume of the solution is 750.0 mL.  Calculate the pH of this solution.

    pH = 1.25

     

     

  3. A 50.0 mL sample of 0.10 M HNO2 is titrated with 0.10 M NaOH.  Calculate the pH of the solution after 50.0 mL of NaOH have been added?
    (Ka = 4.0 x 10 -4) .

    pH = 8.05

    4.  

     

  4. For 100 mL of a buffer that is 0.50 M HOCl and 0.40 M NaOCl, what is the pH after 10.0 mL of 1.0 M NaOH is added? (Ka = 3.0 x 10-8)

    pH = 7.6

     

     

  5. A strong acid is added to water.  Which of the following is the strongest base in the system?
    1. HA
    2. H2O
    3. H3O+
    4. A–
  6. What initial concentration of HF (Ka = 7.2 x 10-4) has the same pH as that of a 0.068M solution of HCl?

    [HF] = 6.5 M

     

     

  7. A monoprotic weak acid, when dissolved in water, 0.92% dissociated and produces a solution with pH = 3.42.  Calculate Ka for the acid.

    Ka = 3.5 x 10-6

    8.  

     

  8. Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.200 M acetic acid to form a pH = 5.00 buffered solution. (Ka = 1.8 x 10-5)

    14.8 g CH3COOH

     

     

  9. Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.025 M HCl.

    pH = 3.68

     

     

  10. Determine whether the following salts are acidic, basic or neutral.
    1. HONH­3NO3 – basic
    2. LiN3– basic
    3. NaNO3– basic
    4. NH4ClO3 – acidic
    5. KC2H3O2 – basic
    6. NaCl – neutral
    7. CaHPO4 – basic

       

       

  11. If the following substance is dissolved in pure water, will the solution be acidic, basic or neutral?

    Solid sodium cyanide

                                                        NaCN – basic

     

     

  12. A 500 mL sample of an HF solution has a pH = 2.00.  What is the pH of the solution if 700 mL of water is added to the solution?  (Ka = 7.2 x 10 –4)

    pH = .18

    13.  

     

  13. Which of the following is a conjugate acid base pair?
    1. H2PO4- and PO43-
    2. HSO4- and SO32-
    3. HNO3 and NO3-
    4. HCl and NaOH
    5. None of these

       

       

  14. Calculate the pH of a 1.9 M solution of HNO3­.

    pH = –0.28

    15.  

     

  15. The pH of a 0.6 M solution of a weak acid id 4.00.  What percent of the acid is ionized?

    0.016%

     

     

  16. Calculate the pH of a 1.30M solution of NH­4Cl.
    Ka = 5.6 x 10 –10

    pH = 4.57

     

     

  17. Determine the concentration of –OH if the pH = 5.40.

    [–OH] = 2.5 x 10-9

    18.  

     

  18. A typical sample of vinegar has a pH of 3.00. Assuming that vinegar is only an aqueous solution of acetic acid (Ka = 1.8 x 10-5), calculate the mass of acetic acid in a 550 mL sample.

    1.87 g CH3COOH

     

     

  19. Calculate the pH for a 3.5 M solution of KNO2.  Ka = 4.0 x 10-4

    pH = 8.97

     

     

  20. Calculate the pH for a solution that contains 2.0 M HF (Ka= 7.2 x 10 -4),  2.0M HCN (Ka = 6.2 x 10 -10) and 2.0 M HOCl (Ka = 3.5 x 10-8).

    pH = 1.42

     

     

  21. Which of the following pieces of information is required to determine the strength of an acid?
    1. The concentration of the acid in solution.
    2. The Ka value of the acid.
    3. The number of acidic hydrogens in the acid.
    4. All of the above.
    5. a and b only.

     

     

  22. Calculate the pH of the solution obtained from the mixing of equal volumes of a solution of HCl with a pH = 2.1 and HNO3 with a pH = 1.6.

    pH = 1.78

     

     

  23. Calculate the pH of a solution after mixing 500 mL of HBr with a concentration of 1.21 M and 330 mL of a 1.60M solution of NaOH.

    pH = 1.03

     

     

  24. Determine the pH of a 2.4M solution of NaClO3.

    pH = 7.00

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