What is the net ionic equation of H2SO4 and BaOH2

Net Ionic Equation of H2SO4 and BaOH2

When sulfuric acid (H₂SO₄) reacts with barium hydroxide (Ba(OH)₂), a double displacement reaction occurs, resulting in the formation of barium sulfate (BaSO₄) and water (H₂O).

Overall Balanced Equation

The overall balanced equation for the reaction is:

Ionic Equation

The ionic equation represents all strong electrolytes as ions. For this reaction, it looks like this:

Net Ionic Equation

To derive the net ionic equation, we remove the spectator ions. These are ions that appear on both sides of the equation in the same form. Here, the barium ion ($\text{Ba}^{2+}$) and the sulfate ion ($\text{SO}_4^{2-}$) directly react to form the precipitate.

The net ionic equation is:

Key Points:

• Strong electrolytes such as H₂SO₄ and Ba(OH)₂ are split into their respective ions.
• Spectator ions are excluded in the net ionic equation.
• The formation of a precipitate (BaSO₄) is the driving force of the reaction.

Explanation of Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is crucial because mass and charge must be conserved in every chemical reaction.

Basic Steps

1. Write the Unbalanced Equation: Start with the skeleton equation, which shows the reactants and products with their chemical formulas.
2. List the Number of Atoms: Tally the number of each type of atom on both sides of the equation.
3. Balance the Atoms: Use coefficients to balance each type of atom. Coefficients are placed in front of the chemical formulas.

Example

Consider the reaction of hydrogen gas with oxygen gas to form water:

$\text{Unbalanced:} \quad H_2 + O_2 \rightarrow H_2O$

Step-by-Step Balancing

1. List the Atoms:

   • Reactants: $H_2$ (2 H atoms), $O_2$ (2 O atoms)
   • Products: $H_2O$ (2 H atoms, 1 O atom)

2. Balance Oxygen Atoms: Notice there are 2 oxygen atoms on the reactant side and 1 oxygen atom on the product side. So, place a coefficient of 2 in front of $H_2O$:

3. Balance Hydrogen Atoms: Now there are 4 hydrogen atoms on the product side (because of the coefficient 2) but only 2 hydrogen atoms on the reactant side. Place a coefficient of 2 in front of $H_2$:

Verification

Confirm that each type of atom is balanced:

• Hydrogen: $2 \times 2 = 4$ (Reactants) and $2 \times 2 = 4$ (Products)
• Oxygen: $1 \times 2 = 2$ (Reactants) and $2 \times 1 = 2$ (Products)

Both sides have 4 hydrogen atoms and 2 oxygen atoms, so the equation is balanced.

Important Points

• Coefficients should be the smallest possible integers.
• Subscripts in chemical formulas should never be changed to balance an equation.

Understanding this process is essential for studying chemical reactions and stoichiometry. The balanced equation provides the mole ratio needed for quantitative analysis.

Explanation

When dealing with chemical reactions, particularly in aqueous solutions, not all ions participate in the reaction process. Those that do not undergo any change and remain in the same state on both the reactant and product sides are known as spectator ions. To identify these, follow these steps:

Step-by-step Process

1. Write the balanced molecular equation:

   • Ensure the given chemical reaction is balanced with the same number of atoms for each element on both sides of the equation.

2. Convert to the complete ionic equation:

   • Break down all aqueous compounds into their respective ions. For instance, if you have a compound like $\text{NaCl}$, it dissociates into $\text{Na}^+$ and $\text{Cl}^-$.

3. Identify ions that appear unchanged:

   • Compare ions on both sides of the complete ionic equation. Those ions that are present in the same form and state are the spectator ions.

Example

Consider the reaction between sodium chloride and silver nitrate:

1. Molecular Equation:

   $$\text{NaCl(aq)} + \text{AgNO}_3\text{(aq)} \rightarrow \text{NaNO}_3\text{(aq)} + \text{AgCl(s)}$$

2. Complete Ionic Equation:

   $$\text{Na}^+ \text{(aq)} + \text{Cl}^- \text{(aq)} + \text{Ag}^+ \text{(aq)} + \text{NO}_3^- \text{(aq)} \rightarrow$$

3. Spectator Ions:
   • Notice that $\text{Na}^+$ and $\text{NO}_3^-$ ions appear on both sides of the equation, unchanged.
   • Therefore, $\text{Na}^+$ and $\text{NO}_3^-$ are the spectator ions.

Net Ionic Equation

After removing the spectator ions from the complete ionic equation, we get the net ionic equation, which shows only the ions and molecules directly involved in the reaction:

Understanding the identification of spectator ions helps simplify chemical equations and focus on the actual chemistry occurring in the reaction.