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Chapter 15: Q61E (page 875)
Question: Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?
A saturated solution is not produced because of the small amount of solid.
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Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected.
\(\begin{array}{l}(a)AgCl(\;s\;)in 0.025MNaCl \\(b)Ca{F_2}(\;\;s\;)in 0.00133MKF \\(c)A{g_2}S{O_4}(\;\;s\;)in 0.500\;L of a solution containing 19.50\;g of {K_2}S{O_4}\\(d)Zn{(OH)_2}(\;s\;)in a solution buffere data pHof 11.45\end{array}\)
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
\(\begin{array}{l}(a)BaSe{O_4},0.0118\;g/100\;mL\\(b)Ba{\left( {Br{O_3}} \right)_2} \times {H_2}O,0.30\;g/100\;mL\\(c)N{H_4}MgAs{O_4} \times 6{H_2}O,0.038\;g/100\;mL\\(d)L{a_2}{\left( {Mo{O_4}} \right)_3},0.00179\;g/100\;mL\end{array}\)
Calculate the concentration of Ag+ required to begin precipitation of Ag2CO3 in a solution that is 2.50 脳 10-6M in CO3 2-
Calculate the volume of 1.50MCH3CO2H required to dissolve a precipitate composed of 350mg each of and CaCO3,SrCO3,BaCO3
Question: Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each:
\(\;(a)\;C{O_2} + O{H^ - } \to HCO_3^ - \)
\({\rm{\;}}(b)\;B{(OH)_3} + O{H^ - } \to B(OH)_4^ - \)
\({\rm{\;}}(c)\;{I^ - } + {I_2} \to I_3^ - \)
\({\rm{\;}}(d)\;AlC{l_3} + C{l^ - } \to AlCl_4^ - (use\;Al - Cl\;single bonds){\rm{\;}}\)
\({\rm{\;}}(e)\;{O^{2 - }} + S{O_3} \to SO_4^{2 - }\)
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