Results and Discussion for Experiment 10: Solubility - Common Ion Effect. State the results of the...
Results and Discussion for Experiment 10: Solubility - Common Ion Effect. State the results of the experiment. Explain the differences in the solubility of calcium iodate in water versus calcium chloride in terms of equilibrium and the common ion effect. Which aspects of the experiment made it difficult for you to accurately determine the concentration of iodate?
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Results and Discussion for Experiment 10: Solubility - Common
Ion Effect. State the results of the...
Pre-Lab: Solubility and the Common-Ion Effect Name: (You must show work for credit) 1. The solubility...
Pre-Lab: Solubility and the Common-Ion Effect Name: (You must show work for credit) 1. The solubility of silver carbonate (mm is its Ksp? 275.745), is 33.5 mg/L. What is its molar solubility, and what A student preforming the lab for the solubility of calcium iodate, titrated a 10.00 mL sample of saturated calcium iodate solution with a 0.011 M sodium thiosulfate solution, The titration required 21.62 mL to turn the solution clear. What was the concentration of the iodate in...
D. Questions: Common Ion Effect on a Chemical System Common Ion Effect on a Chemical System...
D. Questions: Common Ion Effect on a Chemical System Common Ion Effect on a Chemical System - Fe3+(aq) + SCN (aq) [Fe(SCN)]2+ (aq) 1. a. What evidence do you have that the equilibrium shifted when additional iron(III) chloride was added to the test solution made from iron(III)chloride and potassium thiocyanate? n o too . b. In which direction did the equilibrium shift? Explain. c. Which ion created the stress on the system that caused the equilibrium to shift?
Solubility product constant of calcium iodate/common ion effect. I am unsure how to do this however...
Solubility product constant of calcium iodate/common ion
effect.
I am unsure how to do this however I am only asking for help on
trial one as there are 4 total trials and I would like to be able
to do those on my own after I have learned how to do the work.
Thanks.
Also, could you provide the balanced equation for the titration
as well as the solubility equation for iodate?
Part A: Saturated Calcium lodate-No Added Calcium lon...
G. Common ion effect 1. What is the molar solubility of calcium hydroxide (Ksp 5.5 x...
G. Common ion effect 1. What is the molar solubility of calcium hydroxide (Ksp 5.5 x 10) under the following conditions? . In pure water. ii. In water with a pH of 7.25 iii. In water with a pH of 12.50 2. What is the molar solubility of lead (II) fluoride (Ksp 2.7 x 10) under the following conditions? i. In pure water. ii. In a 2.5 x 105 M NaF solution
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...
Experiment 8 Solubility of lonic Precipitates Lead chloride is a slightly soluble salt. When lead chloride...
Experiment 8 Solubility of lonic Precipitates Lead chloride is a slightly soluble salt. When lead chloride dissolves in pure water or an aqueous solution, the small quantity that dissolves completely ionizes and reaches equilibrium in a saturated solution, PbCl(s) ® Pb (aq) + 2Cl(aq) Kp = [Pb (C) (1) Lets be the molar solubility of lead chloride. In pure water, s = [Pb ) = (CH) / 2. In a solution containing Cl, a common ion to lead chloride, s...
Review I Constants Periodic Table The common-ion effect is an application of Le Châtelier's principle, which...
Review I Constants Periodic Table The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system that is stressed will work to alleviate that stress and reestablish equilibrium. Part B-Calculate the molar solubility in NaOH Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.190 M NaOH? Express your answer with the appropriate units. View Available Hint(s) molar solubilityValue Units Submit X Incorrect; Try Again Part C Complete...
Explain the effect of the presence of potassium nitrate and sodium nitrate on the solubility of...
Explain the effect of the presence of potassium nitrate and sodium nitrate on the solubility of KHT using Le Chatelier's principle. (Begin by writing the chemical equation for the equilibrium. Consider only the magnitude of the solublility.) A laboratory experiment designed to determine the solubility product constant for magnesium hydroxide involved a similar procedure to establish a saturated solution. The hydroxide ion concentration was then determined using a pH meter. The pH was recorded as 10.52. Determine Ksp.
1. In your own words explain the common ion effect. 2. What would happen to the...
1. In your own words explain the common ion effect. 2. What would happen to the volume of titrant needed to reach the equivalence point, if some of the solid particles were part of the analyte transferred into the Erlenmeyer flask? 3. In this experiment should the Kremain constant in this experiment? Why or why not? 4. Determine the mole ratio of sodium thiosulfate to the thiosulfate ion in the dissociation reaction: Na,3.0, -> 2Nat + 5.0, 5. Determine the...
Calculating the Effect of a Common Ion on Solubility Consider a saturated solution of the salt...
Calculating the Effect of a Common Ion on Solubility Consider a saturated solution of the salt MX3, which M is a metal cation with a 3+ charge and X is an anion with a 1− charge, in water at 298 K. Which of the following will affect the Ksp of MX3 in water? Consider a saturated solution of the salt , which is a metal cation with a charge and is an anion with a charge, in water at 298 . Which of the...
Pre-Lab: Solubility and the Common-Ion Effect Name: (You must show work for credit) 1. The solubility of silver carbonate (mm is its Ksp? 275.745), is 33.5 mg/L. What is its molar solubility, and what A student preforming the lab for the solubility of calcium iodate, titrated a 10.00 mL sample of saturated calcium iodate solution with a 0.011 M sodium thiosulfate solution, The titration required 21.62 mL to turn the solution clear. What was the concentration of the iodate in...
D. Questions: Common Ion Effect on a Chemical System Common Ion Effect on a Chemical System - Fe3+(aq) + SCN (aq) [Fe(SCN)]2+ (aq) 1. a. What evidence do you have that the equilibrium shifted when additional iron(III) chloride was added to the test solution made from iron(III)chloride and potassium thiocyanate? n o too . b. In which direction did the equilibrium shift? Explain. c. Which ion created the stress on the system that caused the equilibrium to shift?
Solubility product constant of calcium iodate/common ion
effect.
I am unsure how to do this however I am only asking for help on
trial one as there are 4 total trials and I would like to be able
to do those on my own after I have learned how to do the work.
Thanks.
Also, could you provide the balanced equation for the titration
as well as the solubility equation for iodate?
Part A: Saturated Calcium lodate-No Added Calcium lon...
G. Common ion effect 1. What is the molar solubility of calcium hydroxide (Ksp 5.5 x 10) under the following conditions? . In pure water. ii. In water with a pH of 7.25 iii. In water with a pH of 12.50 2. What is the molar solubility of lead (II) fluoride (Ksp 2.7 x 10) under the following conditions? i. In pure water. ii. In a 2.5 x 105 M NaF solution
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...
Experiment 8 Solubility of lonic Precipitates Lead chloride is a slightly soluble salt. When lead chloride dissolves in pure water or an aqueous solution, the small quantity that dissolves completely ionizes and reaches equilibrium in a saturated solution, PbCl(s) ® Pb (aq) + 2Cl(aq) Kp = [Pb (C) (1) Lets be the molar solubility of lead chloride. In pure water, s = [Pb ) = (CH) / 2. In a solution containing Cl, a common ion to lead chloride, s...
Review I Constants Periodic Table The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system that is stressed will work to alleviate that stress and reestablish equilibrium. Part B-Calculate the molar solubility in NaOH Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.190 M NaOH? Express your answer with the appropriate units. View Available Hint(s) molar solubilityValue Units Submit X Incorrect; Try Again Part C Complete...
Explain the effect of the presence of potassium nitrate and sodium nitrate on the solubility of KHT using Le Chatelier's principle. (Begin by writing the chemical equation for the equilibrium. Consider only the magnitude of the solublility.) A laboratory experiment designed to determine the solubility product constant for magnesium hydroxide involved a similar procedure to establish a saturated solution. The hydroxide ion concentration was then determined using a pH meter. The pH was recorded as 10.52. Determine Ksp.
1. In your own words explain the common ion effect. 2. What would happen to the volume of titrant needed to reach the equivalence point, if some of the solid particles were part of the analyte transferred into the Erlenmeyer flask? 3. In this experiment should the Kremain constant in this experiment? Why or why not? 4. Determine the mole ratio of sodium thiosulfate to the thiosulfate ion in the dissociation reaction: Na,3.0, -> 2Nat + 5.0, 5. Determine the...
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