Explanation Given Solubility-product constant for lead(II) chromate is 2.8 × 10 − 13 . Solubility-product constant for cobalt(II) hydroxide is 1.3 × 10 − 15 . Solubility-product constant for cobalt(II) sulfide is 5 × 10 − 22 . Solubility-product constant for chromium(II) hydroxide is 1.6 × 10 − 30 . Solubility-product constant for silver sulfide is 6 × 10 − 51 . The balanced chemical equation for dissolution of lead (II) chromate, PbCrO 4 at equilibrium is, PbCrO 4 ( s ) ⇌ Pb 2 + ( a q ) + CrO 4 2 − ( a q ) Make an ICE table for the above reaction. PbCrO 4 ( s ) ⇌ Pb 2 + ( a q ) + CrO 4 2 − ( a q ) Initial ( M ) : 0 0 Change ( M ) : + x 1 + x 1 Equilibrium ( M ) : x 1 x 1 Concentration of each of the species at equilibrium is calculated by the formula, K s p 1 = [ Pb 2 + ] [ CrO 4 2 − ] Where, K s p 1 is the solubility product constant for lead(II) chromate. [ Pb 2 + ] is the equilibrium concentration of Pb 2 + . [ CrO 4 2 − ] is the equilibrium concentration of CrO 4 2 − . Substitute the values of K s p 1 , [ Pb 2 + ] and [ CrO 4 2 − ] in the above formula. 2.8 × 10 − 13 = x 1 × x 1 x 1 2 = 2.8 × 10 − 13 x 1 = 5.29 × 10 − 7 M The concentration of Pb 2 + in water is, [ Pb 2 + ] = x 1 = 5.29 × 10 − 7 M The balanced chemical equation for dissolution of cobalt(II) hydroxide, Co ( OH ) 2 at equilibrium is, Co ( OH ) 2 ( s ) ⇌ Co 2 + ( a q ) + 2 OH − ( a q ) Make an ICE table for the above reaction. Co ( OH ) 2 ( s ) ⇌ Co 2 + ( a q ) + 2 OH − ( a q ) Initial ( M ) : 0 0 Change ( M ) : + x 2 + 2 x 2 Equilibrium ( M ) : x 2 2 x 2 Concentration of each of the species at equilibrium is calculated by the formula, K s p 2 = [ Co 2 + ] [ OH − ] 2 Where, K s p 2 is the solubility product constant for cobalt(II) hydroxide. [ Co 2 + ] is the equilibrium concentration of Co 2 + . [ OH − ] is the equilibrium concentration of OH − . Substitute the values of K s p 2 , [ Co 2 + ] and [ OH − ] in the above formula. 1.3 × 10 − 15 = x 2 × ( 2 x 2 ) 2 4 x 2 3 = 1.3 × 10 − 15 x 2 = 6.88 × 10 − 6 M The concentration of Co 2 + in water is, [ Co 2 + ] = x 2 = 6.88 × 10 − 6 M The balanced chemical equation for dissolution of cobalt(II) sulfide, CoS at equilibrium is, CoS ( s ) ⇌ Co 2 + ( a q ) + S 2 − ( a q ) Make an ICE table for the above reaction. CoS ( s ) ⇌ Co 2 + ( a q ) + S 2 − ( a q ) Initial ( M ) : 0 0 Change ( M ) : + x 3 + x 3 Equilibrium ( M ) : x 3 x 3 Concentration of each of the species at equilibrium is calculated by the formula, K s p 3 = [ Co 2 + ] [ S 2 − ] Where, K s p 3 is the solubility product constant for cobalt(II) sulfide

Laboratory Experiments For Chemistry: The Central Science, Si Edition

14th Edition

ISBN: 9781292221335

Author: Theodore E. Brown

Publisher: PEARSON

See similar textbooks

Videos

Question

Chapter 17.4, Problem 17.12.1PE

Interpretation Introduction

To determine: The salt that has the highest concentration of its cation in the water, out of the given salts.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 17.4, Problem 17.11.2PE

Chapter 17.4, Problem 17.12.2PE

Students have asked these similar questions

None

Is this an intramolecular reaction or an intermolecular reaction?

Chapter 17 Solutions

Laboratory Experiments For Chemistry: The Central Science, Si Edition

Ch. 17.1 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 17.1 - Practice Exercise 2 Calculate the pH of a solution...Ch. 17.1 - Calculate the concentration of the lactate ion in...Ch. 17.1 - Practice Exercise 2 Calculate the format ion...Ch. 17.2 - Practice Exercise 1 If the pH of a buffer solution...Ch. 17.2 - Prob. 17.3.2PE Ch. 17.2 - Prob. 17.4.1PE Ch. 17.2 - Prob. 17.4.2PE Ch. 17.2 - Calculate the number of grams of ammonium chloride...Ch. 17.2 - Prob. 17.5.2PE

Ch. 17.2 - Prob. 17.6.1PE Ch. 17.2 - Determine The pH of the original buffer described...Ch. 17.3 - An acid-base titration is performed: 250.0 mL of...Ch. 17.3 - Prob. 17.7.2PE Ch. 17.3 - Prob. 17.8.1PE Ch. 17.3 - Calculate the pH in the solution formed by adding...Ch. 17.3 - Prob. 17.9.1PE Ch. 17.3 - Prob. 17.9.2PE Ch. 17.4 - Which of these expressions correctly expresses the...Ch. 17.4 - Prob. 17.10.2PE Ch. 17.4 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 17.4 - Prob. 17.11.2PE Ch. 17.4 - Prob. 17.12.1PE Ch. 17.4 - Prob. 17.12.2PE Ch. 17.5 - Consider a saturated solution of the salt MA3, in...Ch. 17.5 - Prob. 17.13.2PE Ch. 17.5 - Prob. 17.14.1PE Ch. 17.5 - Prob. 17.14.2PE Ch. 17.5 - Prob. 17.15.1PE Ch. 17.5 - Prob. 17.15.2PE Ch. 17.6 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 17.6 - Does a precipitate form when 0.050 L of 2.0 × 10-2...Ch. 17.6 - Under what conditions does an ionic compound...Ch. 17.6 - Prob. 17.17.2PE Ch. 17 - Prob. 1DE Ch. 17 - The following boxes represent aqueos solutions...Ch. 17 - Prob. 2E Ch. 17 - Prob. 3E Ch. 17 - Prob. 4E Ch. 17 - Prob. 5E Ch. 17 - Prob. 6E Ch. 17 - Prob. 7E Ch. 17 - Prob. 8E Ch. 17 - 17.9 The following graphs represent the behavior...Ch. 17 - Prob. 10E Ch. 17 - 17.11 The graph below shows the solubility of a...Ch. 17 - 17.12 Three cations, Ni+2, Cu+2, and Ag+, are...Ch. 17 - Prob. 13E Ch. 17 - Prob. 14E Ch. 17 - Prob. 15E Ch. 17 - Use information from Appendix D to calculate the...Ch. 17 - Prob. 17E Ch. 17 - a. calculate the percent ionization of 0.125 M...Ch. 17 - Prob. 19E Ch. 17 - 17.20 Which of the following solutions is a...Ch. 17 - Prob. 21E Ch. 17 - Calculate the pH of a buffer that is 0.105n M in...Ch. 17 - Prob. 23E Ch. 17 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 17 - You are asked to prepare a pH = 3.00 buffer...Ch. 17 - You are asked to prepare an pH = 4.00 buffer...Ch. 17 - Prob. 27E Ch. 17 - Prob. 28E Ch. 17 - Prob. 29E Ch. 17 - Prob. 30E Ch. 17 - Prob. 31E Ch. 17 - Prob. 32E Ch. 17 - The accompanying graph shows the titration curves...Ch. 17 - Prob. 34E Ch. 17 - 17.35 The samples of nitric and acetic acids shows...Ch. 17 - 17.36 Determine whether each of the following...Ch. 17 - Prob. 37E Ch. 17 - Prob. 38E Ch. 17 - Prob. 39E Ch. 17 - Assume that 30.0 mL of a M solution of a week base...Ch. 17 - Prob. 41E Ch. 17 - Prob. 42E Ch. 17 - Prob. 43E Ch. 17 - Prob. 44E Ch. 17 - Prob. 45E Ch. 17 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 17 - Prob. 47E Ch. 17 - Prob. 48E Ch. 17 - 17.49 for each statement, incate whether it is...Ch. 17 - The solubility of two slighty soluble salts of...Ch. 17 - Prob. 51E Ch. 17 - 17.52 a. true or false: solubility and...Ch. 17 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 17 - Prob. 54E Ch. 17 - Prob. 55E Ch. 17 - Prob. 56E Ch. 17 - using calculate the molar solubility of AgBr in a....Ch. 17 - calculate the solubility of LaF3 in grams per...Ch. 17 - Prob. 59E Ch. 17 - Consider a beaker containing a saturated solution...Ch. 17 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 17 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 17 - 17.63 Which of the following salts will be...Ch. 17 - For each of the following slightly soluble salts,...Ch. 17 - Prob. 65E Ch. 17 - Prob. 66E Ch. 17 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 17 - Prob. 68E Ch. 17 - Prob. 69E Ch. 17 - Prob. 70E Ch. 17 - Calculate the minimum pH needed to precipitate Mn...Ch. 17 - Prob. 72E Ch. 17 - Prob. 73E Ch. 17 - Prob. 74E Ch. 17 - Prob. 75E Ch. 17 - Prob. 76E Ch. 17 - A solution containing several metal ions is...Ch. 17 - An unknown solid is entirely soluble in water. On...Ch. 17 - Prob. 79E Ch. 17 - Prob. 80E Ch. 17 - 17.81 Precipitation of the group 4 cautions of...Ch. 17 - Prob. 82E Ch. 17 - Prob. 83AE Ch. 17 - Prob. 84AE Ch. 17 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 17 - Prob. 86AE Ch. 17 - Equal quantities of 0.010 M solution of an acid HA...Ch. 17 - Prob. 88AE Ch. 17 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 17 - A sample of 0.2140 g of an unknown monophonic acid...Ch. 17 - A sample of 0.1687 g of an unknown monoprotic acid...Ch. 17 - Prob. 92AE Ch. 17 - Prob. 93AE Ch. 17 - What is the pH of a solution made by mixing 0.30...Ch. 17 - Suppose you want to do a physiological experiment...Ch. 17 - Prob. 96AE Ch. 17 - Prob. 97AE Ch. 17 - For each pair of compounds, use Kap values to...Ch. 17 - Prob. 99AE Ch. 17 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 17 - Salts containing the phosphate ion are added to...Ch. 17 - Prob. 102AE Ch. 17 - 17.103 The solubility –product constant for barium...Ch. 17 - Prob. 104AE Ch. 17 - Prob. 105AE Ch. 17 - A buffer of what pH is needed to give a Mg2+...Ch. 17 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 17 - Prob. 108AE Ch. 17 - Prob. 109AE Ch. 17 - Prob. 110IE Ch. 17 - Prob. 111IE Ch. 17 - Prob. 112IE Ch. 17 - Prob. 113IE Ch. 17 - Prob. 114IE Ch. 17 - Prob. 115IE Ch. 17 - Prob. 116IE Ch. 17 - A concentration of 10-100 parts per billion (by...Ch. 17 - Prob. 118IE Ch. 17 - Prob. 119IE Ch. 17 - In nonaqueous solvents, it is possible to react HF...

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.