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10. Consider the titration of 300.0 mL of 0.450 M NH3 (K, = 1.8 x 10) with 0.450 M HNO3. At the stoichiometric point of this titration, the pH is: A) 4.80 B) 2.70 C) 4.95 D) 4.74 E) 7.00

10. Consider the titration of 300.0 mL of 0.450 M NH3 (K, = 1.8 x 10) with 0.450 M HNO3. At the stoichiometric point of this titration, the pH is: A) 4.80 B) 2.70 C) 4.95 D) 4.74 E) 7.00

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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10. Consider the titration of 300.0 mL of 0.450 M NH3 (KB = 1.8 x 10) with 0.450 M HN03. At the stoichiometric point of this titration, the pH is: A) 4.80 B) 2.70 C) 4.95 D) 4.74 on E) 7.00 11. What quantity of NaOH(s) must be added to 2.00 L of 0.434 M HCI to achieve a pH of 13.00? (Assume no volume change.) su to noito bnoe A) 0.67 mol B) 1.07 mol C) 0.20 mol D) 1.00 E 10-13 mol Jm 0E Im 0a E) none of these 13. A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCI. The pH of the resulting solution is 4.7. Which of the following is true? A) At pH 4.7, half the conjugate base, A, has been converted to HA. B) The pKa of the acid is 4.7. C) The pka of the acid is less than 4.7. D) The pKa of the acid is greater than 4.7. E) More than one of the above is correct. 14. You have 75.0 ml of 0.11M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka sto H h O value of HA? A) 3.2 x 10 B) 1.8 x 106 C) 0.57 D) 1.1 x 106 E) none of these
Transcribed Image Text:10. Consider the titration of 300.0 mL of 0.450 M NH3 (KB = 1.8 x 10) with 0.450 M HN03. At the stoichiometric point of this titration, the pH is: A) 4.80 B) 2.70 C) 4.95 D) 4.74 on E) 7.00 11. What quantity of NaOH(s) must be added to 2.00 L of 0.434 M HCI to achieve a pH of 13.00? (Assume no volume change.) su to noito bnoe A) 0.67 mol B) 1.07 mol C) 0.20 mol D) 1.00 E 10-13 mol Jm 0E Im 0a E) none of these 13. A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCI. The pH of the resulting solution is 4.7. Which of the following is true? A) At pH 4.7, half the conjugate base, A, has been converted to HA. B) The pKa of the acid is 4.7. C) The pka of the acid is less than 4.7. D) The pKa of the acid is greater than 4.7. E) More than one of the above is correct. 14. You have 75.0 ml of 0.11M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka sto H h O value of HA? A) 3.2 x 10 B) 1.8 x 106 C) 0.57 D) 1.1 x 106 E) none of these
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