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Chapter 8: Q9P (page 183)

The equilibrium constant for dissolution of a non ionic compound, such as diethyl ether(CH3CH2OCH2CH3) , in water can be written

ether(I)謴ether(aq)K=[etheraq]纬ether

At low ionic strength, role="math" localid="1654837696819" 纬鈮�1 for neutral compounds. At high ionic strength, most neutral molecules can be salted out of aqueous solution. That is, when a high concentration typically (>1M)of a salt such as NaCIis added to aqueous solution, neutral molecules usually becomes less soluble. Does the activity coefficient, 纬ether increases or decreases at high ionic strength?

Short Answer

Expert verified

Thus, the neutral compound in ether would preferentially be extracted in the ether layer and can be easily separated by salting out the layer.

Step by step solution

01

Step 1:Activity Coefficient of Ether at high NaCI concentration

At high concentrations, the activity coefficient value of ether would be very low, and the value would decrease at high ionic strength. Which makes the value of as,

K=etheraq脳activitycoefficient

The value is too small to extract from the aqueous layer.

02

Neutral molecules of Ether at high NaCI concentration

As a result, the neutral compound in ether will preferentially extract in the ether layer and can be easily separated by salting out the layer.

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Most popular questions from this chapter

24. Consider the dissolution of the compound,which gives X2Y22+,X2Y4+,X2Y3(aq)andY2-. Use the mass balance to find an

expression forY2-in terms of the other concentrations. Simplify

your answer as much as possible.

(a) Ion Pairing . As in problem 8-30, find the concentration, ionic strength, and ion pair fraction in 0.025FMgSO4

(b) Two possibly important reactions that we did not consider are acid hydrolysis of Mg+Mg2++H2O謴MgOH++H+and base hydrolysis of SO2-4. Write these two reactions and find their equilibrium constants in Appendices I and G. With the assumed pH near 7.20 and neglecting activity coefficient, show that both reactions are negligible.

Ammonia Equilibrium treated by solver. We now use the solve spreadsheet introduced in Figure 8 - 9 for TIN3 solubility to find the concentration of species in 0.01 M ammonia solution, neglecting activity coefficient. In the systematic treatment of equilibrium of NH3hydrolysis, we have four unknowns (NH3,[NH4+],H+,OH-) and two equilibrium (8-13) , (8-14). Therefore we will estimate the concentration of 4unknowns - 2equilibirum = 2species, for which I choose localid="1663566766281" NH+andOH-. Setup the spreadsheet shown below, in which the estimate localid="1663566820791" pNH4+=3.pOH-= 3 appears in B6andB7 . (Estimates comes from the Kbequilibrium 8-17 with [NH4+]=[OH-]=Kb[NH3]鈮�10-4.755[0.01]鈬�pNH4+=pOH-鈮�3. Estimate donot have to be very good for Solver to work. The formula in cell C8 is [NH3]=[NH4+].

[OH-]/Kb and the formula in the cell C9 is [H+]=Kw/[OH-]. The mass balance b1appears in cell F6 and the charge balance b2 appears in cell F7 . Cell F8 has the sum b12+b22. As described for TIN3on page 176, open the solver window and set the Solver Option. Then use the Solver to set the target cell F8 Equal to Min by changing cells B6 : B7 . What are the concentrations of the species? What fraction of ammonia (=NH4+/NH4++NH3) is hydrolyzed. Your answer should agree with those from Goal Seek in Figure 8-8

Find [Hg22+] in equilibrium with 0.010MKCl saturated withHg2Cl2.

(a) Write the mass balance for CaCl2in water if the species areCa2+ andCI- .

(b) Write the mass balance if the species areCa2+,CI-,CaCI+ , andCaOH+

(c) Write the charge balance for part (b).
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