Write the complete ionic equation and the net ionic equation for the following reaction....
Question:
Write the complete ionic equation and the net ionic equation for the following reaction.
{eq}3Cr(C_2H_3O_2)_2 + 2(NH_4)_3P \to 6NH_4C_2H_3O_2 + Cr_3P_2 {/eq}
Net Ionic Equation:
We can simplify a chemical reaction that occurs in an aqueous solution by omitting the spectator ions. Spectator ions remain dissolved in the solution even after the chemical reaction has occurred. A net ionic equation summarizes the chemical equation in aqueous solution by omitting the spectator ions.
Answer and Explanation: 1
The given balanced molecular equation can be completed by writing the phases of each substance. The reaction is a precipitation reaction as Chromium(III) phosphide is formed. It is the precipitate for the given reaction when mixing the two solutions.
{eq}\rm molecular~equation: 3Cr(C_2H_3O_2)_2(aq) + 2(NH_4)_3P(aq) \to 6NH_4C_2H_3O_2(aq) + Cr_3P_2(s){/eq}
The next step is to separate the chemical equation into their respective ions. In doing so, we get the following complete ionic equation.
{eq}\rm complete~ionic~equation: 3Cr^{3+}(aq) + 2C_2H_3O_2^-(aq) + 6NH_4^+(aq) + 2P^{3-}(aq) \to 6NH_4^+(aq) + 6C_2H_3O_2^-(aq) + Cr_3P_2(s) {/eq}
By removing the acetate and ammonium ions, we obtain the following net ionic equation:
{eq}\rm net~ionic~equation: 3Cr^{3+}(aq) + 2P^{3-}(aq) \to Cr_3P_2(s) {/eq}
Learn more about this topic:
from
Chapter 10 / Lesson 9Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.