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Write a long answer to the following questions in few words or sentence.
A solution of \(Na_2O_3\) is mixed with a solution of \(CaCl_2\). Predict what happens.
The four ions involved are \(Na^+\), \(CO_3^2{^–}\), \(Ca^2{^+}\) and \(Cl^–\). The combinations of the \(Na^+\) and \(Cl^–\) and the \(Ca^2{^+}\) and \(CO_3^2{^–}\) produce the compounds \(NaCl\) and \(CaCO_3\). If both of these compounds are , no reaction takes place. In this case, however, \(CaCO_3\) is . Thus a reaction occurs that we can illustrate with a balanced reaction written in molecular form.
\(Na_2CO_3\)(aq) + \(CaCl_2\)(aq) → +
The equation written in total ionic form is
\(2Na^+\)(aq) + \(CO_3^2{^–}\)(aq) + \(Ca^2{^+}\)(aq) + \(2Cl^–\)(aq) → \(CaCO_3\)(s) + \(2Na^+\) + \(2Cl^–\).
The net ionic equation will be \(Ca^2{^+}\)(aq) + \(CO_3^2{^–}\)(aq) → .
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