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Chapter 8: Problem 91

Write the formula of the precipitate formed when these solutions are mixed: (a) Aluminum nitrate and sodium hydroxide (b) Potassium phosphate and calcium chloride (c) Magnesium sulfate and sodium carbonate

Short Answer

Expert verified
(a) Al(OH)3 (b) Ca3(PO4)2 (c) MgCO3

Step by step solution

01

(a) Identify the reactants and possible products in the reaction

In this case, the given reactants are aluminum nitrate (Al(NO3)3) and sodium hydroxide (NaOH). We can carry out a double displacement reaction between these two reactants by exchanging the positive ions (cations: Al3+ and Na+) and negative ions (anions: NO3- and OH-). This gives us the possible products, sodium nitrate (NaNO3) and aluminum hydroxide (Al(OH)3).
02

(a) Determine the precipitate formed in the reaction

We can determine which of these products is likely to form a precipitate by referring to the solubility rules. Nitrates are generally soluble, so sodium nitrate (NaNO3) will remain in solution. Hydroxides are generally insoluble (except for Group 1 and 2 elements), so aluminum hydroxide (Al(OH)3) will form a precipitate. Thus, the formula of the precipitate formed in this reaction is Al(OH)3.
03

(b) Identify the reactants and possible products in the reaction

In this case, the given reactants are potassium phosphate (K3PO4) and calcium chloride (CaCl2). We can carry out a double displacement reaction between these two reactants by exchanging the cations (K+ and Ca2+) and anions (PO4^3- and Cl-). This gives us the possible products, potassium chloride (KCl) and calcium phosphate (Ca3(PO4)2).
04

(b) Determine the precipitate formed in the reaction

We can determine which of these products is likely to form a precipitate by referring to the solubility rules. Chlorides are generally soluble (except for silver and lead), so potassium chloride (KCl) will remain in solution. Phosphates are generally insoluble (except for Group 1 elements), so calcium phosphate (Ca3(PO4)2) will form a precipitate. Thus, the formula of the precipitate formed in this reaction is Ca3(PO4)2.
05

(c) Identify the reactants and possible products in the reaction

In this case, the given reactants are magnesium sulfate (MgSO4) and sodium carbonate (Na2CO3). We can carry out a double displacement reaction between these two reactants by exchanging the cations (Mg 2+ and Na+) and anions (SO4^2- and CO3^2-). This gives us the possible products, sodium sulfate (Na2SO4) and magnesium carbonate (MgCO3).
06

(c) Determine the precipitate formed in the reaction

We can determine which of these products is likely to form a precipitate by referring to the solubility rules. Sulfates are generally soluble (except for barium, calcium, and lead), so sodium sulfate (Na2SO4) will remain in solution. Carbonates are generally insoluble (except for Group 1 elements), so magnesium carbonate (MgCO3) will form a precipitate. Thus, the formula of the precipitate formed in this reaction is MgCO3.

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Most popular questions from this chapter

You need nickel(II) hydroxide, but there is none in the lab. However, there are lots of other ionic compounds on the shelves. Propose a synthesis for nickel(II) hydroxide.

When an aqueous solution of ammonium sulfate is added to an aqueous solution of calcium nitrate, a precipitate forms. (a) Write a net ionic equation for the precipitation. (b) Write the precipitation reaction in a way that emphasizes that a double- replacement reaction has taken place.

Balance this chemical equation, and classify it as combination, decomposition, single-replacement, or double-replacement: \(\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}+\mathrm{H}_{2} \mathrm{O}\)

Consider the ionic bonds between \(\mathrm{Na}^{+}\) ions and \(\underline{\mathrm{Cl}}^{-}\) ions in \(\mathrm{NaCl}(\mathrm{s}) .\) Why must energy be added to break these bonds (in other words, what is the added energy used for)?

Indicate whether each compound is soluble or insoluble in water: (a) \(\mathrm{BaCO}_{3}\) (b) \(\mathrm{K}_{2} \mathrm{~S}\) (c) \(\mathrm{CaSO}_{4}\) (d) \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) (e) \(\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}\)
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