Interpretation Introduction To determine: If a precipitate forms when 0.050 L of 2.0 × 10 − 2 M NaF is mixed with 0.010 L of 1.0 × 10 − 2 M Ca ( NO 3 ) 2 . Explanation Refer Appendix D The solubility-product-constant, K s p for CaF 2 is 3.9 × 10 − 11 . The chemical equation for the reaction between solutions of NaF and Ca ( NO 3 ) 2 is, NaF ( a q ) + Ca ( NO 3 ) 2 ( a q ) → NaNO 3 ( a q ) + CaF 2 The salts formed after the reaction are NaNO 3 and CaF 2 . Like all sodium salts, NaNO 3 is soluble, but whether CaF 2 will precipitate or not it depends on its reaction quotient. Dissolution of CaF 2 is given as, CaF 2 ( s ) ⇌ Ca 2+ ( a q ) + 2F − ( a q ) The moles of Ca 2 + in the solution is calculated by the formula, n 1 = M 1 × V 1 Where, n 1 is the moles of Ca 2 + . M 1 is the molarity of Ca 2 + . V 1 is the volume of Ca ( NO 3 ) 2 solution. Substitute the values of M 1 and V 1 in the above formula. n 1 = 1.0 × 10 − 2 M × 0.010 L = 1.0 × 10 − 4 mol The moles of F − in the solution is calculated by the formula, n 2 = M 2 × V 2 Where, n 2 is the moles of F − . M 2 is the molarity of F − . V 2 is the volume of NaF solution. Substitute the values of M 1 and V 1 in the above formula. n 2 = 2.0 × 10 − 2 M × 0.050 L = 1.0 × 10 − 3 mol Total volume of the solution is calculated by the formula, V = V 1 + V 2 Where, V is the total volume of the solution

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Chapter 17.6, Problem 17.16.2PE

Interpretation Introduction

To determine: If a precipitate forms when 0.050 L of 2.0×10−2 M

NaF is mixed with 0.010 L of 1.0×10−2 M

Ca( NO3)2 .

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Chapter 17.6, Problem 17.16.1PE

Chapter 17.6, Problem 17.17.1PE

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Chapter 17 Solutions

MAST F/ CHEM: THE CENTRAL SCI CODE ALON

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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. 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If a precipitate forms when 0.050 L of 2.0 × 10 − 2 M NaF is mixed with 0.010 L of 1.0 × 10 − 2 M Ca ( NO 3 ) 2 .

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To determine: If a precipitate forms when 0.050 L of 2.0×10−2 M NaF is mixed with 0.010 L of 1.0×10−2 M Ca( NO3)2 .

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Chapter 17 Solutions

To determine: If a precipitate forms when 0.050 L of 2.0×10−2 M

NaF is mixed with 0.010 L of 1.0×10−2 M

Ca( NO3)2 .