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Chapter 17: Problem 28

Why do we usually not quote the \(K_{\text {sp }}\) values for soluble ionic compounds?

Short Answer

Expert verified
We usually do not quote the \(K_{sp}\) values for soluble ionic compounds because these compounds dissolve almost completely in water. Meaning, given enough volume of water, the salt will dissolve until it is no longer present in solid form. Since the range of possible concentrations is wide and depends on the amount of the compound and solution used, it is not practical or helpful to quote a specific \(K_{sp}\) value.

Step by step solution

01

Understanding \(K_{sp}\) value

The \(K_{sp}\) value, or solubility product constant, is a measure of how much a compound can dissociate in water to form its component ions. Compounds with a higher \(K_{sp}\) value are more soluble and dissociate to a larger extent.
02

Determining Why We Do not typically quote \(K_{sp}\) values for soluble ionic compounds

We usually do not quote a \(K_{sp}\) value for soluble salts. Soluble ionic compounds, such as Sodium Chloride (NaCl) or Potassium Nitrate (KNO3), dissolve almost completely in aqueous solution, given enough volume of water. Because the range of ‪concentrations is wide and the precise concentration depends on the amount of the ionic compound and solute used, it is impractical and unhelpful to quote a \(K_{sp}\) value for these compounds. The \(K_{sp}\) values are more useful for salts that do not dissolve completely in water, as they signify a compound's limit of solubility.

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Most popular questions from this chapter

\(\mathrm{CaSO}_{4}\left(K_{\mathrm{sp}}=2.4 \times 10^{-5}\right)\) has a larger \(K_{\mathrm{sp}}\) value than that of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\left(K_{\mathrm{sp}}=1.4 \times 10^{-5}\right)\). Does it fol- low that \(\mathrm{CaSO}_{4}\) also has greater solubility \((\mathrm{g} / \mathrm{L}) ?\)

A 1.0 -L saturated silver carbonate solution at \(5^{\circ} \mathrm{C}\) is treated with enough hydrochloric acid to decompose the compound. The carbon dioxide generated is collected in a \(19-\mathrm{mL}\) vial and exerts a pressure of \(114 \mathrm{mmHg}\) at \(25^{\circ} \mathrm{C}\). What is the \(K_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) at \(5^{\circ} \mathrm{C} ?\)

A diprotic acid, \(\mathrm{H}_{2} \mathrm{~A}\), has the following ionization constants: \(K_{\mathrm{a}_{1}}=1.1 \times 10^{-3}\) and \(K_{\mathrm{a}_{2}}=2.5 \times 10^{-6} .\) To make up a buffer solution of \(\mathrm{pH} 5.80\), which combination would you choose: \(\mathrm{NaHA} / \mathrm{H}_{2} \mathrm{~A}\) or \(\mathrm{Na}_{2} \mathrm{~A} / \mathrm{NaHA} ?\)

Specify which of these systems can be classified as a buffer system: (a) \(\mathrm{KCl} / \mathrm{HCl}\), (b) \(\mathrm{NH}_{3} / \mathrm{NH}_{4} \mathrm{NO}_{3}\) (c) \(\mathrm{Na}_{2} \mathrm{HPO}_{4} / \mathrm{NaH}_{2} \mathrm{PO}_{4}\)

The molar solubility of \(\mathrm{Pb}\left(\mathrm{IO}_{3}\right)_{2}\) in a \(0.10 \mathrm{M} \mathrm{NaIO}_{3}\) solution is \(2.4 \times 10^{-11} \mathrm{~mol} / \mathrm{L}\). What is \(K_{\mathrm{sp}}\) for \(\mathrm{Pb}\left(\mathrm{IO}_{3}\right)_{2} ?\)
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