5. A similar experiment, to the one performed in this lab, involved dissolving lead (II) chloride, PbCl₂, in a 0.10 M solution of lead (II) nitrate, Pb(NO₃)₂. The chloride ion was then detected using Fajans's Method. Fajans's Method involves titrating Cl⁻ against silver nitrate to make AgCl. The endpoint of the titration is observed when a dichlorofluorescein indicator changes from yellow to pink. a. Write the reaction for the dissociation of PbCl₂(s). b. Write the Ksp expression for the dissociation of PbCl₂. c. Develop an ICE Chart for the dissociation of PbCl₂ in 0.10 M Pb(NO₃)₂. d. According to Fajans's method the [Cl⁻] = 0.00527 M. What is the Ksp of PbCl₂?

5. A similar experiment, to the one performed in this lab, involved dissolving lead (II) chloride, PbCl₂, in a 0.10 M solution of lead (II) nitrate, Pb(NO₃)₂. The chloride ion was then detected using Fajans's Method. Fajans's Method involves titrating Cl⁻ against silver nitrate to make AgCl. The endpoint of the titration is observed when a dichlorofluorescein indicator changes from yellow to pink. a. Write the reaction for the dissociation of PbCl₂(s). b. Write the Ksp expression for the dissociation of PbCl₂. c. Develop an ICE Chart for the dissociation of PbCl₂ in 0.10 M Pb(NO₃)₂. d. According to Fajans's method the [Cl⁻] = 0.00527 M. What is the Ksp of PbCl₂?

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...

See similar textbooks

Similar questions

4. Consider a solution that is 2.3×10−2 M in Fe2+ and 2.0×10−2 M in Mg2+. (Ksp for FeCO3 is 3.07×10−11 and Ksp for MgCO3 is 6.82×10−6.) a. What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?
Write the equilibrium constant expressions for the following chemical reactions (using the net ionic reactions): a) the formation of FeSCN2+ b) the reaction of KHP with NaOH (see Experiment 1) c) the titration of Na2CO3 with HCl (see Experiment 1)
The Fajans titration uses an adsorption indicator to detect the endpoint of a titration in which a precipitate is formed. For the titration of CI- by Ag*, insoluble AgCl is formed. Indicate what is happening at each step of the titration by completing each statement. During the titration a CI- solution is added to an Ag* solution. an Ag* solution is added to a CI solution.
QUESTION 4. A biochemist wants to use X-ray diffraction to determine the structure of a protein. The biochemist must isolate crystals of the protein from solutions buffered to pH 5.20. Acetic acid/acetate ion would be a good choice for the buffer. What would the ratio of [acid]/[conjugate base] need to be in this buffer?
(b) Shown in the graph below is the titration curve that results when 25.0 mL of 0.200 M HCIO is titrated with 0,200 M NaOH, Carefully draw a second curve on the graph that would result from the titration of 25.0 mL. of 0.200 M HCIO, with 0.200 M NaOH. 14- 13 12 11 10- 9. 8 명 7- 6- 5- 4 3 2. 1 35 Volume of 0:200 M NAOH Added (mL.) 10 15 20 25 30 40 45
Chemistry Titration volume to pH 5.5 using 5.3mM HCl (0.0053 M): Sample Titre (mL) 1a 25.20 1b 25.40 1c 25.35 Calculate the carbonate alkalinity and calculate total alkalinity
How can we answer these questions?
In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.
Iodimetric titration is the direct titration with I2 solution. I2 is a weak oxidizing agent and is used to titrate strong reductants. 1. Before the equivalence point, the addition of small amounts of the titrant, I2, transforms it to the colorless iodide ion, I. After the equivalence point, there is a slight excess of the 12 solution. In the presence of the starch indicator, what color change happens to the mixture? 2. Write the net redox reaction representing the reaction between ascorbic acid, C6H8O6, and I2. Standardization of a Solution A 25.00 mL aliquot portion of 0.02420 M C6H8O6 standard solution was transferred into a conical flask. After adding 50 mL H₂O, the mixture needed 26.12 mL I2 solution to reach the endpoint. 3. Calculate the number of mmoles of C6H8O6-. mmoles C6H8O6 4. How many mmoles of I2 reacted with the C6H8O6? mmoles I2 5. What is the molarity of the 12 solution? MI2 Analysis of Vitamin C Supplement The composition of an OTC Vitamin C Supplement is advertised…
50.0 mL of 0.31 M acrylic acid (C2H3COOH, Ka = 1.71 x 10 ) solution is titrated with 0.31 M NaOH to the equivalence point. The %3D reactants are completely transformed into sodium acrylate C2H3COONA at this point. What is the pH of the titration solution at equivalence point? Please keep your answer to two decimal places.
* 1.26×10-8 M * 0×100 M * 1.50×10-8 M * 7.85×10-9 M * 1.75×10-8 M
BUFFERS, HYDROLYSIS OF SALTS 1. A 0.0250 M Ca(X)2 has a pH of 8.049. Ca(X)2 is composed of a Ca2+ cation and an unknown anion X™, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 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 Kh or Kp of X. D. Given the following Ką values of different weak acids, determine the identity of X. Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH3COOH 1.80 x 10-5 HNO2 4.00 x 10-4