When concentrated \(\mathrm{CaCl}_{2}(\mathrm{aq})\) is added to \(\mathrm{Na}_{2} \mathrm{HPO}_{4}(\mathrm{aq}),\) a white precipitate forms that is \(38.7 \%\) Ca by mass. Write a net ionic equation representing the probable reaction that occurs.

Short Answer

Expert verified
The net ionic equation for the reaction is \(3Ca^{2+} + 2PO_4^{3-} \rightarrow Ca_3(PO_4)_2\)

Step by step solution

01

Identify the Chemical Reaction

First, determine the chemical reaction that would occur. The white precipitate formed implies that \( Ca^{2+} \) ions from \( CaCl_2 \) react with \( \text{PO}_4^{3-} \) ions from \( Na_2\text{HPO}_4 \) to form \( Ca_3(\text{PO}_4)_2 \), a white precipitate.
02

Molar Mass Calculation

Next, we need to calculate the molar masses of Calcium and \( Ca_3(\text{PO}_4)_2 \). The molar mass of Calcium is about \( 40.08 \) g/mol and the molar mass of \( Ca_3(\text{PO}_4)_2 \) is calculated as \( 3 \times 40.08 \) g/mol for Calcium, \( 8 \times 16.00 = 128.00 \) g/mol for Oxygen, and \( 2 \times (1.007 \times 3 + 15.999) = 61.98 \) g/mol for Phosphate. Adding them up gives \( 310.18 \) g/mol.
03

Verify the Mass Percent

Now, confirm that \( Ca_3(\text{PO}_4)_2 \) is \( 38.7 \% \) Ca by mass. This is done by taking the total mass of Calcium, dividing it by the total mass of the compound, and multiplying by 100. \(( 3 \times 40.08 / 310.18) \times 100 = 38.8 \% \), which is very close to our provided value.
04

Write the balanced net ionic equation

Finally, write the balanced net ionic equation. The full equation is \( 3Ca^{2+} + 2PO_4^{3-} \rightarrow Ca_3(PO_4)_2 \). However, since \( Na^{+} \) and \( Cl^{-} \) ions are spectator ions (they do not participate directly in the reaction), the net ionic equation is the same as the full reaction.

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Most popular questions from this chapter

Assign oxidation states to the elements involved in the following reactions. Indicate which are redox reactions and which are not. (a) $\mathrm{MgCO}_{3}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$ $\mathrm{Mg}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})$ (b) $\mathrm{Cl}_{2}(\mathrm{aq})+2 \mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Br}_{2}(\mathrm{aq})$ (c) $\mathrm{Ag}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq}) \longrightarrow$ $\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1)+\mathrm{NO}_{2}(\mathrm{g})$ (d) $2 \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{CrO}_{4}^{2-}(\mathrm{aq}) \longrightarrow \mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})$

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