Equilibrium Constants by stariya

VIEWS: 40 PAGES: 6

									IB CHEM II
Writing Acid and Base Equilibrium Constants                Name:


   1) Ammonia is a weak base. If the initial concentration of ammonia is 0.150 M and the equilibrium
      concentration of OH- is 1.6 x 10-3 M, calculate Kb for ammonia.




   2) Formic acid is a weak monoprotic acid. If the initial concentration of formic acid is 0.10 M and the
      equilibrium concentration of H3O+ is 4.2 x 10-3 M, calculate Ka for formic acid.




   3) Cyanic acid is a weak monoprotic acid. If the initial concentration of cyanic acid is 0.150 M and the
      equilibrium concentration of H3O+ is 4.8 x 10-2 M, calculate Ka for cyanic acid.




   4) Gallic acid is a weak monoprotic acid. If the initial concentration of gallic acid is 0.280 M and the
      equilibrium concentration of H3O+ is 3.3 x 10-3 M, calculate Ka for gallic acid.




   5) Trimethylamine is a weak base. If the initial concentration of trimethylamine is 0.390 M and the
      equilibrium concentration of OH- is 4.4 x 10-3 M, calculate Kb for trimethylamine.
6) Dipropylamine is a weak base. If the initial concentration of dipropylamine is 0.160 M and the
   equilibrium concentration of OH- is 0.012 M, calculate Kb for dipropylamine.




7) Uric acid is a weak acid. If the initial concentration of uric acid is 0.110 M and the equilibrium
   concentration of H3O+ is 3.4 x 10-2 M, calculate Ka for uric acid.




8) Butylamine is a weak base. If the initial concentration of butylamine is 0.230 M and the equilibrium
   concentration of OH- is 8.6 x 10-6 M, calculate Kb for butylamine.




9) A certain solution has [H3O+] = 5 x 10-9. Calculate the concentration of [OH-] and the pH of the
   solution




10) A certain solution has [OH-] = 4 x 10-3. Calculate the concentration of [H3O+] and the pH of the
    solution




11) A certain solution has [OH-] = 3 x 10-11. Calculate the concentration of [H3O+] and the pH of the
    solution
12) A certain solution has pH = 2.5. Calculate the pOH, the concentration of [H3O+] and the [OH-] of
    the solution




13) A certain solution has pOH = 2.0. Calculate the pH, the concentration of [H3O+] and the [OH-] of
    the solution




14) A certain solution has pOH = 9.3. Calculate the pH, the concentration of [H3O+] and the [OH-] of
    the solution




15) A certain solution has [H3O+] of 5 x 10-12 Calculate the [OH-] , the pH and the pOH, of the solution




16) What volume of 0.500 M hydrochloric acid is required to exactly neutralize 24.00 c m3 0.350 M
    NaOH?
17) What volume of 0.300 M NaOH solution is required to neutralize 32.5 c m3 of a 0.180 M HCl
    solution?




18) What is the concentration of a sodium hydroxide solution if 18.5 cm3 of it are exactly neutralized by
    25.0 cm3 of a 0.320 M hydrochloric acid solution?




19) Hydrochloric acid is neutralized by calcium hydroxide according to the following reaction:
       a. Ca(OH)2 (aq) + 2 HCl (aq)  CaCl2 (aq) + 2 H2O (l)


   What is the concentration of a calcium hydroxide solution if 12.0 cm3 are exactly neutralized by 5.00
   cm3 of 0.150 M HCl solution?




20) Phosphoric acid H3PO4 reacts with calcium hydroxide according to the following reaction.




21) What volume of 0.500 M hydrochloric acid is required to exactly neutralize 24.00 c m3 0.350 M
    NaOH?
22) What volume of 0.300 M NaOH solution is required to neutralize 32.5 c m3 of a 0.180 M HCl
    solution?




23) What is the concentration of a sodium hydroxide solution if 18.5 cm3 of it are exactly neutralized by
    25.0 cm3 of a 0.320 M hydrochloric acid solution?




24) Hydrochloric acid is neutralized by calcium hydroxide according to the following reaction:
       a. Ca(OH)2 (aq) + 2 HCl (aq)  CaCl2 (aq) + 2 H2O (l)
    What is the concentration of a calcium hydroxide solution if 12.0 cm3 are exactly neutralized by 5.00
    cm3 of 0.150 M HCl solution?




25) Phosphoric acid H3PO4 reacts with calcium hydroxide according to the following reaction. Calculate
    the concentration of a phosphoric acid solution if 35.0 cm3 of it is required to neutralize 20.0 cm3 of
    0.05 M calcium hydroxide solution
    2 H3PO4 + 3 Ca(OH)2  Ca3(PO4)2 + 3 H2O
26) What is the concentration of a sodium hydroxide solution if 43.20 grams of sodium hydroxide are
    dissolved in exactly 3.60 dm3 of solution? What is the concentration of a Phosphoric Acid solution if
    40.00 cm3 of the acid are exactly neutralized by 30.00 cm3 of the sodium hydroxide solution?




27) Acid spills are often neutralized with sodium carbonate. For example

       a. Na2CO3 (s) + 2 HCl (aq)  2 NaCl (aq) + CO2 (g) + H2O (l)

   An instructor dropped a 2.50 dm3 bottle of 12.0 M HCl on a cement floor. (Oops!) How much
   sodium carbonate would be required to neutralize it?




28) Calculate the concentration of a phosphoric acid solution if 35.0 cm3 of it is required to neutralize
    20.0 cm3 of 0.05 M calcium hydroxide solution




29) What is the concentration of a sodium hydroxide solution if 43.20 grams of sodium hydroxide are
    dissolved in exactly 3.60 dm3 of solution? What is the concentration of a Phosphoric Acid solution if
    40.00 cm3 of the acid are exactly neutralized by 30.00 cm3 of the sodium hydroxide solution?

								
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