Chemistry: An Atoms-Focused Approach (Second Edition)
2nd Edition
ISBN: 9780393614053
Author: Thomas R. Gilbert, Rein V. Kirss, Stacey Lowery Bretz, Natalie Foster
Publisher: W. W. Norton & Company
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Students have asked these similar questions
Do all titrations of a strong base with a strong add have the same PH at the equivalence point?
Consider the titration of a weak acid with a strong base at the equivalence point. Choose all true statements that apply.
The moles of weak acid and its conjugate base are equal in the solution.
The moles of weak acid originally in the solution is equal to the moles of strong base added.
The pH is equal to the pKa of the acid.
All of the weak acid originally present in the solution has been converted into its conjugate base.
In the titration of a strong acid (the analyte) with a strong base (the titrant), what type of pH problem must be solved if the titration is stopped at any point after the equivalence point?
Chapter 16 Solutions
Chemistry: An Atoms-Focused Approach (Second Edition)
Ch. 16 - Prob. 16.1VPCh. 16 - Prob. 16.2VPCh. 16 - Prob. 16.3VPCh. 16 - Prob. 16.4VPCh. 16 - Prob. 16.5VPCh. 16 - Prob. 16.6VPCh. 16 - Prob. 16.7VPCh. 16 - Prob. 16.8VPCh. 16 - Prob. 16.9VPCh. 16 - Prob. 16.10VP
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- Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.arrow_forwardEach of the solutions in the table has the same volume and the same concentration, 0.1 M. Which solution requires the greatest volume of 0.1-M NaOH to titrate to the equivalence point? Explain your answer.arrow_forwardA buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?arrow_forward
- Describe at least two ways that the solubility of a sparingly soluble metal hydroxide can be changed.arrow_forwardDraw the titration curves for the titrations of (a) a strong acid with a strong base, (b) a strong acid with a weak base, (c) a weak acid with a strong base and (d) a weak acid with a weak base. Make sure you label each of them properly (volume on x-axis and pH on the y-axis). Describe how you would determine the Ka for a weak acid from the titration curves.arrow_forwardWhy is the titration curve steepest at the equivalence point?arrow_forward
- What must the ratio of acetic acid to acetate ion be to have a buffer with a pH value of 5.00?arrow_forwardA mixture of 5.0 mL 1.0 M HCl and 15.0 mL acetic acid is titrated with 1.0 M NaOH solution. At equivalence point, 43.2 mL of NaOH consumed. What is the concentration of the original acetic acid? How many moles of acetic acid are in the acid mixture?arrow_forwardTerm Definition A point during a titration when a sudden change occurs in some observable property of the solution such as colour, pH, or conductivity The point during a titration at which the exact theoretical amount of titrant has been added to react completely with the sample A solution that has a known concentration The solution that is added from a burette during a titration analysis A technique used to determine the concentration of a substance in a solution by adding measured quantities of another substance that it is known to react with until an endpoint is reached titration endpoint equivalence point standard solution titrantarrow_forward
- A chemistry graduate student is given 100. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K =4.9 × 10 mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH 8.71? What a You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forwardA chemistry graduate student is given 100. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K = 4.9 × 10-10, what mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.78? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 0x10 X Śarrow_forwardTwo buffers are prepared from the same weak acid and its conjugate base. Using the Henderson-Hasselbalch formula, explain how it is possible for both to have the same pH if the concentration of the acid differs. Which of the two buffers would have the larger buffer capacity?arrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY