Using only water and a set volume, you can predict the solubility of a salt and

Question

Using only water and a set volume, you can predict the solubility of a salt and learn whether the reaction between two salts would result in a precipitation reaction. Click on the image to explore this simulation, which demonstrates the solubility of different salts. When you click the simulation link, you may be asked whether to run, open, or save the file. Choose to run or open it. In the simulation, you will find three tabs. The first tab demonstrates the solubility of table salt. The second tab explores other salts that are slightly soluble. The third tab enables you to design your own salt. You can add cations and anions to the beaker that contains water. Mouse over the salt shaker, and move your mouse up and down while clicking the left mouse button to add the salt to the container of water. You can also add and remove water from the container by moving the sliders on the faucets to the left of the container back and forth. Making sure that the default volumes of water of 5.0×10?23 L and 1.0×10?16 L are used in the Table Salt and Slightly Soluble Salts tab, respectively, add each of the possible salts to the water. Make a table indicating how much salt dissolves before the solution becomes saturated.

Rank the salts from most soluble to least soluble. To rank items as equivalent, overlap thenm Copper(I) iodide Mercury(II) bromideThallium(I) sulfideTable salt Silver bromide Most Soluble Least Soluble The correct ranking cannot be determined reset help

Explanation / Answer

For solubility comparisson:

AB <-> A+ + B-; Ksp = [A+][B-] = S*S = S^2 --> S = sqrt(Ksp)

A2B <--> 2A+ + B-2 Ksp = [A+]^2[B-2] = (2S)^2 * S = 4*S^3 --> S = (Ksp/4)^(1/3)

AB2 <--> A+2 + 2B- ; Ksp = [A+2][B-]^2 = S* (2S)^2 = 4*S^3 --> S = (Ksp/4)^(1/3)

A3B <---> 3A+ + B-3 ; Ksp = [A+]^3[B-3] = (3S)^3 * S = 27*S^4 --> S = (Ksp/27)^(1/4)

AB3 <--> A+3 + 3B- ; Ksp = [A+3][B-]^3 = S* (3S)^3 = 27*S^4 --> S = (Ksp/27)^(1/4)

A3B2 <-->3A+2 + 2B-3; Ksp = [A+2]^3[B-3]^2 = (3S)^3 * (2S)^2 = 108*S^5 --> S = (Ksp/108)^(1/5)

A2B3 <-->2A+3 + 3B-2; Ksp = [A+3]^2[B-2]^3 = (2S)^2 * (3S)^3 = 108*S^5 --> S = (Ksp/108)^(1/5)

Now, substitute al Ksp values, and identifty molar solubilities:

CuI 1.27×10–12 AB type = S = sqrt(1.27*10^-12) = 1.126*10^-6 M

HgBr2 6.2×10–20; AB2 type = S = (Ksp/4)^(1/3) = ((6.2*10^-20)/4)^(1/3) = 2.493*10^-7 M

Tl2S 6×10–22 A2B type = S = (Ksp/4)^(1/3) = ((6.2*10^-22)/4)^(1/3) = 5.37*10^-8 M

Table Salt, NaCl --> Ksp >> 1

AgBr 5.35×10–13 AB type =S = sqrt(5.35*10^-13) = 7.31*10^-7 M

Therefore:

NaCl > CuI > AgBr > HgBr2 > Tl2S

Table salt > Copper(I) iodide > Silver bromide > Mercury(II) bromide > Thallium(I) sulfide

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