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exam_3_practice_exam_questions

exam_3_practice_exam_questions - c for the reaction 5 A...

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1 This document contains extra practice problems involving equilibrium, acid/base, buffer, and titration calculations. The exam will also include short answer conceptual questions on these topics. 1. A 0.0560 g quantity of CH 3 COOH is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H + , CH 3 COO - and CH 3 COOH at equilibrium. K a =1.8 x 10 -5 . 2. A titration in conducted where exactly 500 mL of 0.167 M NaOH was titrated into 500 mL 0.100 M CH 3 COOH. Calculate the pH of the solution at this point in the titration. CH 3 COOH Ka=1.8 x 10 -5 .

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2 3. What is the pH at the equivalence point in the titration discussed in the previous question?
3 4. Consider the following equilibrium process at 700°C 2 H 2 (g) + S 2 (g) ÅÆ 2 H 2 S (g) Analysis shows that there are 2.50 moles of H 2 , 1.35 x 10 -5 moles of S 2 , and 8.70 moles of H 2 S present in a 12.0 L flask at equilibrium. Calculate the equilibrium constant K

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Unformatted text preview: c for the reaction. 5. A 2.50 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 28 percent of the NOCl had dissociated: 2 NOCl (g) ÅÆ 2 NO (g) + Cl 2 (g) Calculate the equilibrium constant K c for the reaction. 4 6. The concentration of HO-ions in a certain household ammonia cleaning solution is 0.0025 M. Calculate the concentration of H+ ions. Ammonia K b =1.8 x 10-5 7. Calculate the pH of a 0.15 M solution of CH 3 COONa. What is the percent ionization? K b =5.6 x 10-10 5 8. The pH of a 0.30 M solution of a weak base is 10.66. What is the K b of the base? 9. Calculate the pH of a buffer solution of 0.10 M Na 2 HPO 4 /0.15 M NaH 2 PO 4 ....
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exam_3_practice_exam_questions - c for the reaction 5 A...

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