Question

Write a balanced equation for the reaction of barium hydroxide with nitric acid.

Short answer

The balanced equation is \( \text{Ba(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Ba(NO}_3)_2 + 2\text{H}_2\text{O} \).

Step-by-step solution

Identify Reactants

The reaction involves barium hydroxide and nitric acid. Identify the chemical formulas: Barium hydroxide is \( \text{Ba(OH)}_2 \) and nitric acid is \( \text{HNO}_3 \).

Determine Products

In a neutralization reaction between a hydroxide (base) and an acid, the products are typically water (\( \text{H}_2\text{O} \)) and a salt. Here, the salt formed is barium nitrate \( \text{Ba(NO}_3)_2 \).

Write Unbalanced Equation

Combine the identified reactants and products into an equation: \[ \text{Ba(OH)}_2 + \text{HNO}_3 \rightarrow \text{Ba(NO}_3)_2 + \text{H}_2\text{O} \]

Balance the Equation

Make sure all elements have the same number of atoms on each side of the equation. After examining the unbalanced equation, adjust coefficients:- Barium (Ba): 1 on each side.- Hydroxide (OH) and nitrate (NO3): Typically you need 2 mole of HNO3 for each mole of Ba(OH)2 to balance nitrate.- Water: Adjust coefficient to ensure matching H and O atoms.The balanced equation is: \[ \text{Ba(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Ba(NO}_3)_2 + 2\text{H}_2\text{O} \]

Key concepts

Neutralization Reaction

Neutralization reactions are a fascinating type of chemical reaction where an acid and a base react to form water and a salt. This process is essential in many everyday applications, such as antacid tablets and cleaning products. In our given exercise, barium hydroxide, which is a base, reacts with nitric acid, classified as an acid. The result of this neutralization reaction is the formation of water (\( \text{H}_2\text{O} \) and a salt, specifically barium nitrate (\( \text{Ba(NO}_3)_2 \) ). The key takeaway here is that during a neutralization:

• The base provides hydroxide ions (OH⁻).
• The acid provides hydrogen ions (H⁺).
• The ions combine to form water, while the leftover ions form a salt.

It’s important to recognize these patterns as they help predict the products of other neutralization reactions. Whenever you encounter an acid-base reaction, expect the products to typically include water and a salt.

Balancing Chemical Equations

Balancing a chemical equation ensures that the number of each type of atom is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a closed system. In our reaction between barium hydroxide and nitric acid, initially, the equation might not look balanced:\[ \text{Ba(OH)}_2 + \text{HNO}_3 \rightarrow \text{Ba(NO}_3)_2 + \text{H}_2\text{O} \]Balancing this requires careful adjustments:

• Ensure one barium (Ba) atom is present on both sides.
• Recognize the nitrate ions (NO₃⁻). Since two nitrate ions are in the product as a single barium nitrate, you need two nitric acid molecules on the reactant side.
• Add coefficients to water to balance hydrogen and oxygen: 2 water molecules will finalize the equation.

After making these adjustments, the balanced equation is:\[ \text{Ba(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Ba(NO}_3)_2 + 2\text{H}_2\text{O} \]Balancing requires practice, but it becomes easier with experience. It's all about tweaking coefficients to level the atomic playing field.

Chemical Formulas

Chemical formulas are shorthand representations of chemical substances. They provide information about the elements present and their respective quantities. In the exercise at hand, you deal with several formulas:

• Barium hydroxide (\( \text{Ba(OH)}_2 \)) tells you there's one barium atom and two hydroxide groups.
• Nitric acid (\( \text{HNO}_3 \)) indicates one hydrogen atom and one nitrate group.
• The resulting barium nitrate (\( \text{Ba(NO}_3)_2 \)) informs of one barium atom paired with two nitrate groups.

Understanding chemical formulas involves recognizing standard conventions:- Parentheses in formulas, such as in barium hydroxide, indicate groups of atoms that act as a unit.- Subscripts show the number of specific atoms within that group.Gaining comfort with formulas is critical, as it aids in predicting reaction products and balancing equations properly. Mastery of this practice transforms what might seem complicated equations into relatable, logical processes.