A CHM 122 student determines that the molar solubility of ABCI(s) in pure water is 1.3x 10 mol/L.What would be the molar solubility of AgCl(s) in 0.31 M SrCl,(aq)?The Ksp value for AgCI(s) iss K = 1.8 x 10 10Type your answer in the space below using scientificnotation.(example: 0.012 = 1.2*10^-2)

The Ksp for a salt is be expressed as: AxBy → x Ay+ + y Bx- Ksp = [Ay+]x [Bx-]y

À CHM 122 student determines that the molar solubility of AGCI(s) in pure water is 1.3 x 10 mol/L. What would be the molar solubility of AgCI(s) in 0.31 M SrCl2(aq)? The Ksp Value for AGCI(s) is Ksp = 1.8 x 10 10. Type your answer in the space below using scientific notation. (example: 0.012 = 1.2*10^-2)

À CHM 122 student determines that the molar solubility of AGCI(s) in pure water is 1.3 x 10 mol/L. What would be the molar solubility of AgCI(s) in 0.31 M SrCl2(aq)? The Ksp Value for AGCI(s) is Ksp = 1.8 x 10 10. Type your answer in the space below using scientific notation. (example: 0.012 = 1.2*10^-2)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.60PAE

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To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?
Consider the insoluble salts JQ, K2R, L2S3, MT2, and NU3. They are formed from the metal ions J+, K+, L3+, M2+, and N3+ and the nonmetal ions Q-, R2-, S2-, T-, and U-. All the salts have the same Ksp, 11010 at 25C. (a) Which salt has the highest molar solubility? (b) Does the salt with the highest molar solubility have the highest solubility in g salt/100 g water? (c) Can the solubility of each salt in g/ 100 g water be determined from the information given? If yes, calculate the solubility of each salt in g/100 g water. If no, why not?
How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?
ΔG° for the reaction AgCl(s) ⇌ Ag+(aq) + Cl-(aq) is 55.6kJ/mol at 25 °C. What is the molar solubility of AgCls) , in mol/L at this temperature? Express your answer in scientific notation rounded to three significant figures. 1.23 x 10-4 should be written as 1.23*10^-4
In a saturated solution of silver sulfate Ag2SO4(S), the molar solubilty is 3.6 × 10-4 mol/L. The Ksp of silver sulfate would be?
The solubility product constant for CaCO3 (s) in water is Ksp = [Ca+2] [CO3 -2] = 4.8 x 10^-9 Consider a 1.00 M solution of calcium chloride, in which you drop a piece of Dry Ice. Show that the minimum concentration (threshold amount) of carbonate ions necessary for a precipitate to appear is 4.8 x 10-9 M. Another way to think about this situation is to calculate the Q for the calcium chloride/Dry Ice solution and ask “will precipitation occur?”..
The solubility product constant of silver sulfate, Ag2SO4, is 1.2 x 10-5. Determine the mass of Ag2SO4 that can be dissolved in 2.00L of a 0.572 M solution of sodium sulfate, Na2SO4.
The KspKsp of cobalt(II) hydroxide, Co(OH)2, is 5.92×10−15. Calculate the molar solubility, s, of this compound.
Calculate the molar solubility and solubility in g/L of gold(III) chloride (AuCl3, 303.33 g/mol) inpure water. Ksp = 3.2 x 10-25

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