Conditions: A. Titration of 20-mL 0.05 M HF with 0.10 M NaOH B. Titration of 20-mL 0.05 M KF with 0.10 M HCI I. pH at EP in A II. pH at EP in B the quantity in I is greater the quantity in II is greater the two quantities are equal the relationship cannot be determined due to insufficient information

Conditions: A. Titration of 20-mL 0.05 M HF with 0.10 M NaOH B. Titration of 20-mL 0.05 M KF with 0.10 M HCI I. pH at EP in A II. pH at EP in B the quantity in I is greater the quantity in II is greater the two quantities are equal the relationship cannot be determined due to insufficient information

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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A 50.00-mL solution of 0.0400 M nitrous acid ( K a = 4.5 × 10 –4) is titrated with 20.00 mL of a 0.100 M solution of NaOH as the titrant. What is the pH of at the equivalence point? ( K w = 1.00 × 10 –14) a. 7.59 b. 11.45 c. 7.14 d. 7.90 e. 7.80 f. None of the above
Consider the titration curve describing the titration of a strong acid by addition of a strong base. Which of the following statements is incorrect? a. The equivalence point is at pH = 7.0. b. The pH is lower at the end of the titration than at the beginning. c. The pH increases rapidly around the equivalence point. d. At the equivalence point, the only species present are water and a neutral salt. e. The pH does not increase very rapidly at the beginning of the titration.
2. Calculate the pH at each stage in the titration for the addition of 0.110 M HCL to 35.0 mL of 0.105 M NAOH. a. Initiallyb. after the addition of 5.00mL of acid c. after the addition of a further 5.00mL of acid (10.00mL total of acid)d. at the equivalence point.e. after the addition of 5.00 of acid beyond the equivalence point.f. after the addition of 10.0mL of acid beyond the equivalence pointg. on graph paper draw the curve of pH vs mL of acid. First plot, the points from a through f and then sketch the curve.
Which of the following solutions is a good buffer system? A. A solution that is 0.10 M HC2H3O2 and 0.10 M LİC2H3O2 B. A solution that is 0.10 M HF and 0.10M NaC2H3O2 C. A solution that is 0.10 M HCI and 0.10 M NH4* D.A solution that is 0.10 M NaOH and 0.10 M KOH E. None of the above are buffer systems.
Which plot accurately represents the titration between 50.0 mL unknown HNO2 concentration and 0.15 M NaOH? А. В. Base (mL) Base (mL) C. D. Base (mL) Base (mL) Graph A Graph B Graph D Graph C Hd
A buffer is prepared by adding 20.0g of sodium acetate to 500mL of a 0.150 M acetic acid solution. Determine the pH of the buffer. a. 4.74 b. 6.32 c. 5.26 d. 4.23
Which of the following, when mixed, would NOT result in a buffer solution? а. 10 mL of 0.1M HCI and 20 mL of 0.1 M NH3 O b. 10 mL of 0.1 M HCI and 20 mL of 0.1 M NaC2H3O2 C. 10 mL of 0.1 M NaOH and 20 mL of 0.1 M potassium cyanide, KCN d. 10 mL of 0.1 M NaOH and 20 mL 0.1 M HF e. 10 mL of 0.1 M acetic acid, HC2H3O2, and 10 mL of 0.1 M sodium acetate, NaC2H3O2
Moving to another question will save this response. uestion 5 In the titration of 0.100 M HNO3 with the titrant 0.100 M KOH, what species are present at any point after KOH has been added but before the equivalence point? a. KOH only b. KNOJ only c. HNOJ and KNO d. HNO3 only e. HNO3 and KOH
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67. Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. a. the initial pH b. the volume of added base required to reach the equivalence point c. the pH at 10.0 ml of added base
A 50 mL solution of 0.08 M KCN (aq) is titrated with 0.125 M HCl (aq). Calculate the pH at the following points of the titration curve. a. 16 mL HCl added b. 30 mL HCl added c. 32 mL HCl added d. 34 mL HCl added
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