1. a) Write the balanced equilibrium expression for dissolving Ca(OH)2 (s), including all physical states. b) Write the solubility equilibrium constant, Ksp, for Ca(OH)2.
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Step 1: Write the balanced equilibrium expression for dissolving Ca(OH)2 (s), including all physical states. Show more…
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1.) Write out the equilibrium expression for Ca(OH)2 (s). At 25 °C 0.7815 g of Ca(OH)2 will dissolve in 1.0 L of H2O. Given this information, calculate the Ksp for Ca(OH)2 at 25 °C. 2.) By adding HCl, will the solubility increase, decrease, or not be changed? Use this fact to discuss what would happen if you begin titrating before you filter excess solid Ca(OH)2 from your solution. 3. Look up and compare the S° values for Ca2+ (aq) and Na+ (aq). Explain why the signs are different between the two values by describing how the ions behave in aqueous solution
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Do number 2 only 2.) By adding HCl, will the solubility increase, decrease, or not be changed? Use this fact to discuss what would happen if you begin titrating before you filter excess solid Ca(OH)2 from your solution.
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The solubility of calcium hydroxide is low enough to be listed as "insoluble" in solubility tables, but it is much more soluble than most of the other ionic compounds that are similarly classified. Its $\mathrm{K}_{\mathrm{sp}}$ is $5.5 \times 10^{-6}$. a) Write the equation for the equilibrium to which the $\mathrm{K}_{\mathrm{sp}}$ is related. b) If you had such an equilibrium, name at least two substances or general classes of substances that might be added to (1) reduce the solubility of $\mathrm{Ca}(\mathrm{OH})_{2}$ and (2) increase its solubility. Justify your choices. c) Without adding a calcium or hydroxide ion, name a substance or class of substances that would, if added, ( 1 ) increase $\left[\mathrm{OH}^{-}\right]$ and (2) reduce $\left[\mathrm{OH}^{-}\right] .$ Justify your choices.
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