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Chapter 17: Problem 49

For each statement, indicate whether it is true or false. (a) The solubility of a slightly soluble salt can be expressed in units of moles per liter. (b) The solubility product of a slightly soluble salt is simply the square of the solubility. (c) The solubility of a slightly soluble salt is independent of the presence of a common ion. (d) The solubility product of a slightly soluble salt is independent of the presence of a common ion.

Short Answer

Expert verified
Short Answer: (a) True, the solubility of a slightly soluble salt can be expressed in units of moles per liter (M). (b) False, the solubility product of a slightly soluble salt is the product of the molar concentrations of its ions in a saturated solution, each raised to the power of their stoichiometric coefficients. It is only the square of the solubility if the salt has a 1:1 stoichiometric ratio. (c) False, the solubility of a slightly soluble salt is influenced by the presence of a common ion due to the common ion effect and Le Chatelier's principle. (d) True, the solubility product (Ksp) of a slightly soluble salt is a constant value for a given salt at a particular temperature and is independent of the presence of a common ion.

Step by step solution

01

Statement (a)

This statement is true. The solubility of a slightly soluble salt can be expressed in units of moles per liter (M). Solubility refers to the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature to produce a saturated solution.
02

Statement (b)

This statement is false in general. The solubility product (Ksp) of a slightly soluble salt is the product of the molar concentrations of its ions in a saturated solution, each raised to the power of their stoichiometric coefficients. However, if the salt has a 1:1 stoichiometric ratio (e.g., AB), then the solubility product is the square of the solubility.
03

Statement (c)

This statement is false. According to the common ion effect, the solubility of a slightly soluble salt is influenced by the presence of a common ion. When a common ion is present, the solubility of the salt is decreased due to the shift in the equilibrium according to Le Chatelier's principle.
04

Statement (d)

This statement is true. The solubility product (Ksp) of a slightly soluble salt is a constant value for a given salt at a particular temperature. The presence of a common ion will not affect the solubility product; instead, it will affect the solubility of the salt.

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Most popular questions from this chapter

How many milliliters of 0.105 \(\mathrm{M}\) HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 \(\mathrm{mL}\) of \(0.0950 \mathrm{MNaOH},(\mathbf{b}) 22.5 \mathrm{mL}\) of \(0.118 \mathrm{MNH}_{3},(\mathbf{c}) 125.0\) mL of a solution that contains 1.35 gof NaOH perliter?

A 35.0-mL sample of 0.150\(M\) acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) is titrated with 0.150 \(\mathrm{M} \mathrm{NaOH}\) solution. Calculate the pH after the following volumes of base have been added: (a) 0 \(\mathrm{mL}\) (b) \(17.5 \mathrm{mL},(\mathrm{c}) 34.5 \mathrm{mL},(\mathbf{d}) 35.0 \mathrm{mL},(\mathbf{e}) 35.5 \mathrm{mL},(\mathbf{f}) 50.0 \mathrm{mL}\)

Salts containing the phosphate ion are added to municipal water supplies to prevent the corrosion oflead pipes. (a) Based on the \(\mathrm{pK}_{a}\) values for phosphoric acid \(\left(\mathrm{pK}_{a 1}=7.5 \times 10^{-3} , \right.\) \(\mathrm{p} K_{a 2}=6.2 \times 10^{-8}, \mathrm{p} K_{a 3}=4.2 \times 10^{-13} )\) what is the \(\mathrm{K}_{b}\) value for the \(\mathrm{PO}_{4}^{3-}\) ion? (b) What is the pH of a \(1 \times 10^{-3}\) \(M\) solution of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) (you can ignore the formation of \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) and \(\mathrm{H}_{3} \mathrm{PO}_{4} ) ?\)

Assume that 30.0 \(\mathrm{mL}\) of a 0.10 \(\mathrm{M}\) solution of a weak base \(\mathrm{B}\) that accepts one proton is titrated with a 0.10\(M\) solution of the monoprotic strong acid HA. (a) How many moles of HA have been added at the equivalence point? (b) What is the predominant form of B at the equivalence point? (a) Is the pH \(7,\) less than \(7,\) or more than 7 at the equivalence point?\( (\mathbf{d} )\) Which indicator, phenolphthalein or methyl red, is likely to be the better choice for this titration?

A 1.00 -L solution saturated at \(25^{\circ} \mathrm{C}\) with calcium oxalate \(\left(\mathrm{CaC}_{2} \mathrm{O}_{4}\right)\) contains 0.0061 \(\mathrm{g}\) of \(\mathrm{CaC}_{2} \mathrm{O}_{4} .\) Calculate the solubility-product constant for this salt at \(25^{\circ} \mathrm{C}\) .
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