Explanation Refer Table 17.1 The equilibrium constant for formation of Cr ( OH ) 4 − , K f is 8 × 10 29 . The pOH value for the solution is calculated by the formula, pOH = 14.00 − pH Substitute the value of pH in the above formula. pOH = 14.00 − 10.00 = 4.00 The concentration of OH − at equilibrium is calculated by the formula, [ OH − ] = 10 ( − pOH ) Where, [ OH − ] is the equilibrium concentration of OH − in the solution. Substitute the value of pOH in the above formula. [ OH − ] = 10 ( − 4.00 ) = 0.0001 M As one mole of Cr ( NO 3 ) 3 dissociates to give one mole of Cr 3 + , 0.010 mol of Cr ( NO 3 ) 3 gives 0.010 mol of Cr 3 + .Moreover, as the volume of the solution is 1 L , the initial concentration of Cr 3 + is equal to its number of moles. The chemical equation for the equilibrium between Cr 3 + and Cr ( OH ) 4 − is, Cr ( OH ) 4 − ( a q ) ⇌ Cr 3 + ( a q ) + 4 OH − ( a q ) The K f for formation of Cr ( OH ) 4 − is very high that means all of Cr 3 + get converted to Cr ( OH ) 4 − and hence its initial concentration is same as that of Cr 3 + . The equilibrium constant for the above reaction is reverse of K f . Make an ICE table for the above reaction. Cr ( OH ) 4 − ( a q ) ⇌ Cr 3 + ( a q ) + 4 OH − ( a q ) Initial ( M ) : 0

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Coordination Chemistry

It is a part of chemistry, in which the study of compounds that have central atoms surrounded by molecules or ions, known as ligand, is known as coordination chemistry.

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Chapter 17.5, Problem 17.15.2PE

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To determine: The concentration of Cr3+ in equilibrium with Cr(OH)4−(aq) when 0.010 mol of Cr( NO3)3 is dissolved in 1 L of solution buffered at pH 10.0 .

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Chapter 17.5, Problem 17.15.1PE

Chapter 17.6, Problem 17.16.1PE

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Chapter 17 Solutions

CHEMISTRY: THE CENTRAL SCIENCE

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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. 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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...

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The concentration of Cr 3 + in equilibrium with Cr ( OH ) 4 − ( a q ) when 0.010 mol of Cr ( NO 3 ) 3 is dissolved in 1 L of solution buffered at pH 10 .0 .

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To determine: The concentration of Cr3+ in equilibrium with Cr(OH)4−(aq) when 0.010 mol of Cr( NO3)3 is dissolved in 1 L of solution buffered at pH 10.0 .

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Chapter 17 Solutions