2. Which of the followings will not make a buffer solution (circle all that apply) a 100 mL of 0.1 M NaOH is added to 100 ml. 0.1M HNO₂ solution b. 100 mL of 0.1 M NaOH is added to 200 ml. 0.1M HNO, solution c. 100 mL of 0.1 M NaOH is added to 80 ml. 0.1M HNO, solution d. 100 mL of 0.1 M NaOH is added to 150 ml. 0.1M HNO, solution

2. Which of the followings will not make a buffer solution (circle all that apply) a 100 mL of 0.1 M NaOH is added to 100 ml. 0.1M HNO₂ solution b. 100 mL of 0.1 M NaOH is added to 200 ml. 0.1M HNO, solution c. 100 mL of 0.1 M NaOH is added to 80 ml. 0.1M HNO, solution d. 100 mL of 0.1 M NaOH is added to 150 ml. 0.1M HNO, solution

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.17QAP

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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

2. Which of the followings will not make a buffer solution (circle all that apply)
a. 100 mL of 0.1 M NaOH is added to 100 mL 0.1M HNO₂ solution
b. 100 mL of 0.1 M NaOH is added to 200 ml. 0.1M HNO₂ solution
c. 100 mL of 0.1 M NaOH is added to 80 mL. 0.1M HNO₂ solution
d. 100 mL of 0.1 M NaOH is added to 150 mL 0.1M HNO, solution

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Step 1: Determine the solutions which will not make a buffer solution from the given solutions:

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Step 2: a. The moles of each species remaining after add NaOH and the solution is:

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Step 3: b. The moles of each species remaining after add NaOH and the solution is:

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Step 4: c. The moles of each species remaining after add NaOH and the solution is:

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Step 5: d. The moles of each species remaining after add NaOH and the solution is:

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Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
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Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.
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Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.