Questions: Question 14 (5 points) Which of the following is the net ionic equation of the reaction BaCl2(aq) with H2SO4(aq) Ba2+ + 2 Cl+ + 2 H+ + SO42- = Ba2+ + SO42- + 2 H+ + 2 Cl- Ba2+ + 2 Cl + 2 H+ + SO42- = BaSO4(3) + 2 H+ + 2 Cl- Ba2+ + SO42- = BaSO4(s) BaCl2 + H2SO4 = BaSO4(3) + 2 HCl

Question 14 (5 points) Which of the following is the net ionic equation of the reaction BaCl2(aq) with H2SO4(aq) Ba2+ + 2 Cl+ + 2 H+ + SO42- = Ba2+ + SO42- + 2 H+ + 2 Cl- Ba2+ + 2 Cl + 2 H+ + SO42- = BaSO4(3) + 2 H+ + 2 Cl- Ba2+ + SO42- = BaSO4(s) BaCl2 + H2SO4 = BaSO4(3) + 2 HCl

Transcript text: Question 14 (5 points) Which of the following is the net ionic equation of the reaction $\mathrm{BaCl}_{2(\mathrm{aq})}$ with $\mathrm{H}_{2} \mathrm{SO}_{4(\mathrm{aq})}$ $\mathrm{Ba}^{2+}+2 \mathrm{Cl}^{+}+2 \mathrm{H}^{+}+\mathrm{SO}_{4}^{2-}=\mathrm{Ba}^{2+}+\mathrm{SO}_{4}^{2-}+2 \mathrm{H}^{+}+2 \mathrm{Cl}^{-}$ $\mathrm{Ba}^{2+}+2 \mathrm{Cl}+2 \mathrm{H}^{+}+\mathrm{SO}_{4^{2-}}=\mathrm{BaSO}_{4(3)}+2 \mathrm{H}^{+}+2 \mathrm{Cl}^{-}$ $\mathrm{Ba}^{2+}+\mathrm{SO}_{4}{ }^{2-}=\mathrm{BaSO}_{4(\mathrm{~s})}$ $\mathrm{BaCl}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4}=\mathrm{BaSO}_{4(3)}+2 \mathrm{HCl}$

Solution

Solution Steps

Step 1: Identify the Reactants and Products

The reaction involves barium chloride ($\mathrm{BaCl}_2$) and sulfuric acid ($\mathrm{H}_2\mathrm{SO}_4$). When these react, barium sulfate ($\mathrm{BaSO}_4$) and hydrochloric acid ($\mathrm{HCl}$) are formed. The balanced molecular equation is: \[ \mathrm{BaCl}_2 + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{BaSO}_4 + 2\mathrm{HCl} \]

Step 2: Write the Complete Ionic Equation

In aqueous solution, strong electrolytes like $\mathrm{BaCl}_2$ and $\mathrm{H}_2\mathrm{SO}_4$ dissociate into ions: \[ \mathrm{Ba}^{2+} + 2\mathrm{Cl}^- + 2\mathrm{H}^+ + \mathrm{SO}_4^{2-} \rightarrow \mathrm{BaSO}_4 + 2\mathrm{H}^+ + 2\mathrm{Cl}^- \]

Step 3: Identify and Remove Spectator Ions

Spectator ions are ions that appear on both sides of the equation and do not participate in the reaction. In this case, $\mathrm{Cl}^-$ and $\mathrm{H}^+$ are spectator ions.

Step 4: Write the Net Ionic Equation

After removing the spectator ions, the net ionic equation is: \[ \mathrm{Ba}^{2+} + \mathrm{SO}_4^{2-} \rightarrow \mathrm{BaSO}_4(\mathrm{s}) \]

Final Answer

The net ionic equation for the reaction of $\mathrm{BaCl}_2$ with $\mathrm{H}_2\mathrm{SO}_4$ is: \[ \boxed{\mathrm{Ba}^{2+} + \mathrm{SO}_4^{2-} = \mathrm{BaSO}_4(\mathrm{s})} \]

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