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Chapter 4: Problem 23

Which of the following processes will likely result in a precipitation reaction? (a) Mixing a \(\mathrm{NaNO}_{3}\) solution with a \(\mathrm{CuSO}_{4}\) solution. (b) Mixing a \(\mathrm{BaCl}_{2}\) solution with a \(\mathrm{K}_{2} \mathrm{SO}_{4}\) solution. Write a net ionic equation for the precipitation reaction.

Short Answer

Expert verified
Process (b) will result in a precipitation reaction. The net ionic equation is \( \mathrm{Ba^{2+}} + \mathrm{SO_{4}^{2-}} \rightarrow \mathrm{BaSO}_{4(s)} \).

Step by step solution

01

Identify the Potential Precipitation Reactions

A precipitation reaction occurs when two solutions are mixed to form an insoluble product or a precipitate. Using the solubility rules, it can be determined that: \n (a) \(\mathrm{NaNO}_{3}\) and \(\mathrm{CuSO}_{4}\) are both soluble compounds. There won't be any precipitation reaction.\n (b) \(\mathrm{BaCl}_{2}\) and \(\mathrm{K}_{2}\mathrm{SO}_{4}\) react to form \(\mathrm{BaSO}_{4}\) and \(\mathrm{2KCl}\). According to solubility rules, \(\mathrm{BaSO}_{4}\) is insoluble and so a precipitation reaction will occur.
02

Write the total ionic equation

The total ionic equation shows all the particles in the solution as they exist. \n \( \mathrm{Ba^{2+}} +2\mathrm{Cl^{-}} + 2\mathrm{K^{+}} + \mathrm{SO_{4}^{2-}} \rightarrow \mathrm{BaSO}_{4(s)} + 2\mathrm{K^{+}} + 2\mathrm{Cl^{-}} \)
03

Write the net ionic equation

The net ionic equation can be obtained by eliminating the spectator ions, ions which appear on both reactant and product side, from the total ionic equation.\n The net ionic equation will be: \n \( \mathrm{Ba^{2+}} + \mathrm{SO_{4}^{2-}} \rightarrow \mathrm{BaSO}_{4(s)} \)

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Most popular questions from this chapter

Distilled water must be used in the gravimetric analysis of chlorides. Why?

A \(1.00-\mathrm{g}\) sample of a metal \(\mathrm{X}\) (that is known to form \(\mathrm{X}^{2+}\) ions) was added to a \(0.100 \mathrm{~L}\) of \(0.500 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4}\). After all the metal had reacted, the remaining acid required \(0.0334 \mathrm{~L}\) of \(0.500 \mathrm{M} \mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the metal and identify the element.

Give the oxidation number of the underlined atoms in the following molecules and ions: (a) \(\underline{\mathrm{ClF}},\) (b) \(\underline{\mathrm{IF}}_{7}\), (c) \(\underline{\mathrm{CH}}_{4},\) (d) \(\underline{\mathrm{C}}_{2} \mathrm{H}_{2},\) (e) \(\underline{\mathrm{C}}_{2} \mathrm{H}_{4},\) (f) \(\mathrm{K}_{2} \mathrm{Cr} \mathrm{O}_{4},(\mathrm{~g}) \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) (h) \(\mathrm{KMnO}_{4},\) (i) \(\mathrm{NaHCO}_{3},(\mathrm{j}) \underline{\mathrm{L} i}_{2},(\mathrm{k}) \mathrm{NaIO}_{3},(\mathrm{l}) \mathrm{K} \underline{\mathrm{O}}_{2}\) \((\mathrm{m}) \underline{\mathrm{PF}}_{6}^{-},(\mathrm{n}) \mathrm{K} \underline{\mathrm{Au}} \mathrm{Cl}_{4}\)

A sample of \(0.6760 \mathrm{~g}\) of an unknown compound containing barium ions \(\left(\mathrm{Ba}^{2+}\right)\) is dissolved in water and treated with an excess of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). If the mass of the \(\mathrm{BaSO}_{4}\) precipitate formed is \(0.4105 \mathrm{~g}\), what is the percent by mass of Ba in the original unknown compound?

Describe the steps involved in preparing a solution of known molar concentration using a volumetric flask.
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