10. Consider the titration of 300.0 mL of 0.450 M NH3 (KB = 1.8 x 10) with 0.450 M HN03. At thestoichiometric point of this titration, the pH is:A) 4.80B) 2.70C) 4.95D) 4.74onE) 7.0011. 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 noitobnoeA) 0.67 molB) 1.07 molC) 0.20 molD) 1.00 E 10-13 molJm 0EIm 0aE) none of these13. A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mLof 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 Kasto H h Ovalue of HA?A) 3.2 x 10B) 1.8 x 106C) 0.57D) 1.1 x 106E) none of these

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Answered: 10. Consider the titration of 300.0 mL…

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

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

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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