Explanation Given The concentration of Pb ( NO 3 ) 2 solution is 0.10 M . The volume of the sample is 10 mL . The volume of Pb ( NO 3 ) 2 solution added to the sample is 0.2 mL . The molar mass of I − is 126.9045 g / mol . The number of moles of Pb ( NO 3 ) 2 or Pb 2 + is calculated by the formula, Number of moles = Molar concentration × Volume of the solution in liters Substitute the value of molar concentration of Pb ( NO 3 ) 2 and the volume of the solution in the above formula. Number of moles = 0.10 M × 0.2 1000 L = 2 × 10 − 5 mol The total volume of the solution is, 10 mL + 0.2 mL = 10.2 mL Therefore, the final concentration of Pb 2 + after the addition of one drop of Pb ( NO 3 ) 2 to the sample is calculated by the formula, Molar concentration = Number of moles Total volume of the solution in liters Substitute the values of the number of moles of Pb 2 + and the total volume of the solution in the above formula. Molar concentration = 2 × 10 − 5 mol 10.2 1000 L = 1.96 × 10 − 3 M The dissolution equilibrium for PbI 2 is, PbI 2 ( s ) ⇌ Pb 2 + ( a q ) + 2 I − ( a q ) The value of the solubility product ( K sp ) for the dissolution equilibrium is 7

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Chapter 3, Problem 55E

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To determine: The minimum number of grams of I− needed to precipitate PbI2 by the addition of one drop (0.2 mL) of 0.10 M

Pb( NO3)2 to 10 mL of the sample.

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Chapter 3, Problem 54E

Chapter 3, Problem 56E

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Chemistry: The Central Science, Books a la Carte Edition & Solutions to Red Exercises for Chemistry & Mastering Chemistry with Pearson eText -- Access Card Package

Ch. 3.1 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 3.1 - Prob. 3.1.2PE Ch. 3.1 - Consider a saturated solution of the salt MA3, in...Ch. 3.1 - Prob. 3.2.2PE Ch. 3.2 - Prob. 3.3.1PE Ch. 3.2 - Prob. 3.3.2PE Ch. 3.2 - Prob. 3.4.1PE Ch. 3.2 - Prob. 3.4.2PE Ch. 3.3 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 3.3 - Does a precipitate form when 0.050 L of 2.0 × 10-2...

Ch. 3.3 - Under what conditions does an ionic compound...Ch. 3.3 - Prob. 3.6.2PE Ch. 3.4 - Prob. 3.7.1PE Ch. 3.4 - The following boxes represent aqueos solutions...Ch. 3.4 - Prob. 3.8.1PE Ch. 3.4 - Prob. 3.8.2PE Ch. 3.4 - Prob. 3.9.1PE Ch. 3.4 - Prob. 3.9.2PE Ch. 3.4 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 3.4 - Practice Exercise 2 Calculate the pH of a solution...Ch. 3.4 - Calculate the concentration of the lactate ion in...Ch. 3.4 - Practice Exercise 2 Calculate the format ion...Ch. 3.4 - Practice Exercise 1 If the pH of a buffer solution...Ch. 3.4 - Prob. 3.12.2PE Ch. 3.5 - Prob. 3.13.1PE Ch. 3.5 - Prob. 3.13.2PE Ch. 3.5 - Calculate the number of grams of ammonium chloride...Ch. 3.5 - Prob. 3.14.2PE Ch. 3.5 - Prob. 3.15.1PE Ch. 3.5 - Determine The pH of the original buffer described...Ch. 3.6 - An acid-base titration is performed: 250.0 mL of...Ch. 3.6 - Prob. 3.16.2PE Ch. 3.6 - Prob. 3.17.1PE Ch. 3.6 - Calculate the pH in the solution formed by adding...Ch. 3.7 - Prob. 3.18.1PE Ch. 3.7 - Prob. 3.18.2PE Ch. 3.7 - Prob. 3.19.1PE Ch. 3.7 - Prob. 3.19.2PE Ch. 3.7 - Prob. 3.20.1PE Ch. 3.7 - Prob. 3.20.2PE Ch. 3 - The accompanying graph shows the titration curves...Ch. 3 - Prob. 2E Ch. 3 - Prob. 3E Ch. 3 - Prob. 4E Ch. 3 - Prob. 5E Ch. 3 - Prob. 6E Ch. 3 - Prob. 7E Ch. 3 - Prob. 8E Ch. 3 - Prob. 9E Ch. 3 - Use information from Appendix D to calculate the...Ch. 3 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 3 - You are asked to prepare a pH = 3.00 buffer...Ch. 3 - You are asked to prepare an pH = 4.00 buffer...Ch. 3 - Prob. 14E Ch. 3 - Prob. 15E Ch. 3 - Prob. 16E Ch. 3 - Prob. 17E Ch. 3 - Prob. 18E Ch. 3 - Prob. 19E Ch. 3 - Prob. 20E Ch. 3 - 17.35 The samples of nitric and acetic acids shows...Ch. 3 - 17.36 Determine whether each of the following...Ch. 3 - Prob. 23E Ch. 3 - Prob. 24E Ch. 3 - Prob. 25E Ch. 3 - Assume that 30.0 mL of a M solution of a week base...Ch. 3 - Prob. 27E Ch. 3 - Prob. 28E Ch. 3 - Prob. 29E Ch. 3 - Prob. 30E Ch. 3 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 3 - Prob. 32E Ch. 3 - Prob. 33E Ch. 3 - Prob. 34E Ch. 3 - The solubility of two slighty soluble salts of...Ch. 3 - Prob. 36E Ch. 3 - 17.52 a. true or false: solubility and...Ch. 3 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 3 - Prob. 39E Ch. 3 - Prob. 40E Ch. 3 - using calculate the molar solubility of AgBr in a....Ch. 3 - calculate the solubility of LaF3 in grams per...Ch. 3 - Prob. 43E Ch. 3 - Consider a beaker containing a saturated solution...Ch. 3 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 3 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 3 - 17.63 Which of the following salts will be...Ch. 3 - For each of the following slightly soluble salts,...Ch. 3 - Prob. 49E Ch. 3 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 3 - Prob. 51E Ch. 3 - Prob. 52E Ch. 3 - Prob. 53E Ch. 3 - Calculate the minimum pH needed to precipitate Mn...Ch. 3 - Prob. 55E Ch. 3 - Prob. 56E Ch. 3 - Prob. 57E Ch. 3 - Prob. 58E Ch. 3 - Prob. 59E Ch. 3 - An unknown solid is entirely soluble in water. On...Ch. 3 - Prob. 61E Ch. 3 - Prob. 62E Ch. 3 - 17.81 Precipitation of the group 4 cautions of...Ch. 3 - Prob. 64E Ch. 3 - Prob. 65E Ch. 3 - Prob. 66E Ch. 3 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 3 - Prob. 68E Ch. 3 - Equal quantities of 0.010 M solution of an acid HA...Ch. 3 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 3 - (a) Define the terms limiting reactant and excess...Ch. 3 - Prob. 72E Ch. 3 - Prob. 73E Ch. 3 - Prob. 74E Ch. 3 - What is the pH of a solution made by mixing 0.30...Ch. 3 - Suppose you want to do a physiological experiment...Ch. 3 - Prob. 77E Ch. 3 - Prob. 78E Ch. 3 - For each pair of compounds, use Kap values to...Ch. 3 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 3 - Salts containing the phosphate ion are added to...Ch. 3 - Prob. 82E Ch. 3 - 17.103 The solubility –product constant for barium...Ch. 3 - Prob. 84E Ch. 3 - Prob. 85E Ch. 3 - A buffer of what pH is needed to give a Mg2+...Ch. 3 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 3 - Prob. 88AE Ch. 3 - Prob. 89AE Ch. 3 - Prob. 90AE Ch. 3 - Prob. 91AE Ch. 3 - Prob. 92AE Ch. 3 - Prob. 93AE Ch. 3 - Prob. 94AE Ch. 3 - Prob. 95AE Ch. 3 - A concentration of 10-100 parts per billion (by...Ch. 3 - Prob. 97AE Ch. 3 - Prob. 98AE Ch. 3 - In nonaqueous solvents, it is possible to react HF...Ch. 3 - Prob. 100AE Ch. 3 - Prob. 101AE Ch. 3 - Prob. 102AE Ch. 3 - 17.9 The following graphs represent the behavior...Ch. 3 - Prob. 104AE Ch. 3 - 17.11 The graph below shows the solubility of a...Ch. 3 - Prob. 106IE Ch. 3 - Prob. 107IE Ch. 3 - (a) If an automobile travels 225 mi with a gas...Ch. 3 - Prob. 109IE Ch. 3 - Prob. 110IE Ch. 3 - Hydrogen cyanide, HCN, is a poisonous gas. The...Ch. 3 - Prob. 112IE

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The minimum number of grams of I − needed to precipitate PbI 2 by the addition of one drop ( 0.2 mL ) of 0.10 M Pb ( NO 3 ) 2 to 10 mL of the sample.

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To determine: The minimum number of grams of I− needed to precipitate PbI2 by the addition of one drop (0.2 mL) of 0.10 M Pb( NO3)2 to 10 mL of the sample.

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Chapter 3 Solutions

To determine: The minimum number of grams of I− needed to precipitate PbI2 by the addition of one drop (0.2 mL) of 0.10 M

Pb( NO3)2 to 10 mL of the sample.