1. A 0.0450 M Ca(X), has a pH of 11.079. CaX₂ is composed of a Cacation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X), into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the Kor Ks of X D. Given the following K, values of different weak acids, determine the identity of X Weak acids KI HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH₂COOH 1.80 x 10-5 HNO₂ 4.00 x 10-4

1. A 0.0450 M Ca(X), has a pH of 11.079. CaX₂ is composed of a Cacation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X), into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the Kor Ks of X D. Given the following K, values of different weak acids, determine the identity of X Weak acids KI HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH₂COOH 1.80 x 10-5 HNO₂ 4.00 x 10-4

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

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A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
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Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M propanoic acid (HC3H5O2,Ka = 1.3 105) with 0.100 M NaOH.
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1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…