Calculate the pH of a 0080 M carbonic acid solution H 2 CO 3 aq that has the

Calculate the ph of a 0080 m carbonic acid solution h

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30) Calculate the pH of a 0.080 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1= 4.3 × 10-7and Ka2= 5.6 × 10-11. A) 1.10 B) 3.73 C) 6.37 D) 10.25 31) What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1= 1.3 × 10-4 and Ka2= 1.0 × 10-11? 32) If the pKa of HCHO2is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE? 33) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3. The Kbfor NH3is 1.8 × 10-5. 34) Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO. The Kafor HClO is 2.9 × 10-8. A) 5.99 B) 8.01 C) 7.54 D) 7.06 E) 6.46 35) A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Kafor HF is 3.5 × 10-4. 36) A 100.0 mL sample of 0.18 M HClO4is titrated with 0.27 M LiOH. Determine the pH of the solution before the addition of any LiOH. 37) A 100.0 mL sample of 0.18 M HClO4is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point). 38) A 100.0 mL sample of 0.180 M HClO4is titrated with 0.270 M LiOH. Determine the pH of the solution after the addition of 75.0 mL of LiOH. A) 12.1 B) 2.65 C) 11.35 D) 1.89 E) 13.06 39) Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp(AgBr) = 7.7 × 10-13. 40) Determine the molar solubility of AgBr in a solution containing 0.200 M NaBr. Ksp(AgBr) = 7.7 × 10-13. 41) Determine the molar solubility for Al(OH)3 in pure water. K sp for Al(OH) 3 = 1.3 x 10 -33 .
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  • Fall '09
  • pH, NH3

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