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It is found that up to 0.0110 g of SrF2 dissolves in 100 mL of aqueous solution at a certain temperature. Determine the value of Ksp for SrF2. 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products.

It is found that up to 0.0110 g of SrF2 dissolves in 100 mL of aqueous solution at a certain temperature. Determine the value of Ksp for SrF2. 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 70QAP: . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method...
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It is found that up to 0.0110 g of SrF2 dissolves in 100 mL of aqueous solution at a certain temperature. Determine the value of Ksp for SrF2. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. SRF2(s) Sr** (aq) 2 F (aq) + Initial (M) 8.76 x 10-4 Change (M) -8.76 x 10-4 +x +2x Equilibrium | (M) +x +2x Your Initial concentration for SrF2 is incorrect. Remember, there will be no ions present initially because the solid has not dissociated yet. Your Change in concentration for Sr2* is incorrect. In this problem, you should use the given molar solubility to determine the concentration of each ion at Equilibrium and hence the Change. Remember that the concentration of each ion will be directly proportional to the number of moles of the ion produced from 1 mole of the solid! Your Change in concentration for F is incorrect. In this problem, you should use the given molar solubility to determine the concentration of each ion at Equilibrium and hence the Change. Remember that the concentration of each ion will be directly proportional to the number of moles of the ion produced from 1 mole of the solid!
Transcribed Image Text:It is found that up to 0.0110 g of SrF2 dissolves in 100 mL of aqueous solution at a certain temperature. Determine the value of Ksp for SrF2. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. SRF2(s) Sr** (aq) 2 F (aq) + Initial (M) 8.76 x 10-4 Change (M) -8.76 x 10-4 +x +2x Equilibrium | (M) +x +2x Your Initial concentration for SrF2 is incorrect. Remember, there will be no ions present initially because the solid has not dissociated yet. Your Change in concentration for Sr2* is incorrect. In this problem, you should use the given molar solubility to determine the concentration of each ion at Equilibrium and hence the Change. Remember that the concentration of each ion will be directly proportional to the number of moles of the ion produced from 1 mole of the solid! Your Change in concentration for F is incorrect. In this problem, you should use the given molar solubility to determine the concentration of each ion at Equilibrium and hence the Change. Remember that the concentration of each ion will be directly proportional to the number of moles of the ion produced from 1 mole of the solid!
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