Question

use the references to access important values if needed for this question.
does a reaction occur when aqueous solutions of cobalt(ii) chloride and sodium phosphate are combined?
oyes
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if a reaction does occur, write the net ionic equation.
(use the solubility rules provided in the owl preparation page to determine the solubility of compounds. be sure to specify
states such as (aq) or (s). if a box is not needed leave it blank.)

Explanation:

Step1: Write the chemical formulas

Cobalt(II) chloride is \(CoCl_2\), sodium phosphate is \(Na_3PO_4\). In aqueous solution, they dissociate: \(CoCl_2(aq)=Co^{2 +}(aq)+2Cl^{-}(aq)\) and \(Na_3PO_4(aq)=3Na^{+}(aq)+PO_4^{3 -}(aq)\).

Step2: Predict the products

Using the double - displacement reaction rule (\(AB + CD
ightarrow AD+CB\)), the products are \(Co_3(PO_4)_2\) and \(NaCl\). \(NaCl\) is soluble (most chloride salts are soluble, and sodium salts are always soluble). \(Co_3(PO_4)_2\) is insoluble (phosphate salts are generally insoluble except for those with alkali metal cations (\(Na^{+},K^{+},etc.\)) and \(NH_4^{+}\)).
The molecular equation is \(3CoCl_2(aq)+2Na_3PO_4(aq)=Co_3(PO_4)_2(s)+6NaCl(aq)\)

Step3: Write the complete ionic equation

\(3Co^{2 +}(aq)+6Cl^{-}(aq)+6Na^{+}(aq)+2PO_4^{3 -}(aq)=Co_3(PO_4)_2(s)+6Na^{+}(aq)+6Cl^{-}(aq)\)

Step4: Write the net ionic equation

Cancel out the spectator ions (\(Na^{+}\) and \(Cl^{-}\)).
The net ionic equation is \(3Co^{2 +}(aq)+2PO_4^{3 -}(aq)=Co_3(PO_4)_2(s)\)

Answer:

Yes, the net ionic equation is \(3Co^{2 +}(aq)+2PO_4^{3 -}(aq)=Co_3(PO_4)_2(s)\)