Question

Write a balanced chemical equation for the neutralization reaction between each given acid and base. Include the proper phase labels. a) \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{~s}) \rightarrow ?\) b) \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{CsOH}(\mathrm{aq}) \rightarrow ?\)

Short answer

a) \(3\mathrm{HNO}_{3}(\mathrm{aq}) + \mathrm{Fe(OH)}_{3}(\mathrm{s}) \rightarrow \mathrm{Fe(NO}_{3})_{3}(\mathrm{aq}) + 3\mathrm{H}_{2}\mathrm{O}(\mathrm{l})\); b) \(\mathrm{H}_{3}\mathrm{PO}_{4}(\mathrm{aq}) + 3\mathrm{CsOH}(\mathrm{aq}) \rightarrow \mathrm{Cs}_{3}\mathrm{PO}_{4}(\mathrm{aq}) + 3\mathrm{H}_{2}\mathrm{O}(\mathrm{l})\)

Step-by-step solution

Identify the Products

In a neutralization reaction, an acid reacts with a base to produce a salt and water. The general formula for this reaction is:\[\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}\]For part (a):\[\mathrm{HNO}_{3} + \mathrm{Fe(OH)}_{3} \rightarrow \mathrm{Fe(NO}_{3})_{3} + \mathrm{H}_{2}\mathrm{O}\]For part (b):\[\mathrm{H}_{3}\mathrm{PO}_{4} + \mathrm{CsOH} \rightarrow \mathrm{Cs}_{3}\mathrm{PO}_{4} + \mathrm{H}_{2}\mathrm{O}\]

Balance the Chemical Equations

Balancing involves ensuring that the number of atoms of each element is the same on both sides of the equation.For part (a): The formula \(\mathrm{HNO}_{3}\) gives one nitrate ion for each nitric acid molecule, and \(\mathrm{Fe(OH)}_{3}\) has three hydroxide ions, so we need three \(\mathrm{HNO}_{3}\):\[3\mathrm{HNO}_{3} + \mathrm{Fe(OH)}_{3} \rightarrow \mathrm{Fe(NO}_{3})_{3} + 3\mathrm{H}_{2}\mathrm{O}\]For part (b):The formula \(\mathrm{H}_{3}\mathrm{PO}_{4}\) provides three hydrogen ions, so we need three \(\mathrm{CsOH}\):\[\mathrm{H}_{3}\mathrm{PO}_{4} + 3\mathrm{CsOH} \rightarrow \mathrm{Cs}_{3}\mathrm{PO}_{4} + 3\mathrm{H}_{2}\mathrm{O}\]

Assign Proper Phase Labels

Finally, include the phase labels based on the states provided and the nature of the products.For part (a):\[3\mathrm{HNO}_{3}(\mathrm{aq}) + \mathrm{Fe(OH)}_{3}(\mathrm{s}) \rightarrow \mathrm{Fe(NO}_{3})_{3}(\mathrm{aq}) + 3\mathrm{H}_{2}\mathrm{O}(\mathrm{l})\]For part (b):\[\mathrm{H}_{3}\mathrm{PO}_{4}(\mathrm{aq}) + 3\mathrm{CsOH}(\mathrm{aq}) \rightarrow \mathrm{Cs}_{3}\mathrm{PO}_{4}(\mathrm{aq}) + 3\mathrm{H}_{2}\mathrm{O}(\mathrm{l})\]

Key concepts

Neutralization Reaction

Neutralization reactions are a vital part of chemistry, occurring when an acid and a base react to form water and a salt. This is a fundamental concept in acid-base chemistry.
The general formula for a neutralization reaction can be written as :

• Acid + Base → Salt + Water

A neutralization reaction is essential in managing pH levels in solutions, making it highly applicable in everyday life scenarios like digestion and industrial processes. The key to identifying a neutralization reaction comes down to recognizing the reactants as an acid and a base and ensuring the products formed are a salt and water. This simplicity makes it easy to forecast the products of many such reactions.
Each reactant plays a role; the acid typically provides the cation for the salt, and the base contributes the anion. This exchange leads to the formation of a neutral product profile - hence the term "neutralization." Understanding the underlying principles of this type of reaction unlocks a deeper comprehension of how various substances interact chemically.

Balancing Equations

Balancing chemical equations is a necessary skill that ensures the law of conservation of mass is respected in chemical reactions. This law requires that atoms are neither created nor destroyed in a reaction; thus, the number of atoms of each element in the reactants must equal the number in the products.
In practice, balancing involves adjusting coefficients before the chemical formulas in an equation so that the elements' count is equal on both sides. Some tips for effective balancing include:

• Start with elements that appear in the least number of compounds first.
• Balance more complex molecules after simpler ones.
• Adjust coefficients, not subscripts, to balance the equation.

For example, in the equation \[3\mathrm{HNO}_{3} + \mathrm{Fe(OH)}_{3} \rightarrow \mathrm{Fe(NO}_{3})_{3} + 3\mathrm{H}_{2}\mathrm{O}\] the coefficients indicate three nitric acid molecules are needed to react with one iron(III) hydroxide to produce a balanced equation.
Balancing equations is critical in ensuring chemical reactions are accurately represented and allows us to calculate the correct amounts of reactants and products, crucial for practical applications in industries and laboratories.

Phase Labels

Phase labels provide valuable information about the state of each reactant and product in a chemical equation, indicating whether a substance is aqueous, solid, liquid, or gaseous. This information shapes our understanding of how a reaction proceeds.

• (aq) stands for aqueous, meaning the substance is dissolved in water.
• (s) indicates a solid state, usually meaning a precipitate in reactions.
• (l) denotes liquid, often applied to substances naturally found in liquid state.
• (g) is for gaseous substances.

These labels are essential in comprehending the conditions under which reactions occur. For example, in the balanced equation of 3\(\mathrm{HNO}_{3}(\mathrm{aq}) + \mathrm{Fe(OH)}_{3}(\mathrm{s}) \rightarrow \mathrm{Fe(NO}_{3})_{3}(\mathrm{aq}) + 3\mathrm{H}_{2}\mathrm{O}(\mathrm{l})\), the phase labels tell us that particles reactive in solution are combining to form additional aqueous and liquid products.
This knowledge helps predict behaviors such as precipitation, solubility, and evaporation, enhancing our ability to conduct experiments and analyze results effectively.

Acid-Base Reaction

An acid-base reaction represents one of the most common types of chemical reactions, fundamentally revolving around the transfer of protons. Typically, the acid donates protons (H⁺ ions), while the base accepts them. This exchange plays a critical role in determining the outcome of the reaction.
The classic Bronsted-Lowry definition explains acids as proton donors and bases as proton acceptors.

• An acid-base reaction typically results in the formation of water from the interaction of H⁺ ions from the acid and OH⁻ ions from the base.
• In some reactions, no water forms, but other ionic products are created instead.

For instance, in the neutralization reaction between hydrochloric acid and sodium hydroxide \[\mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{NaCl} + \mathrm{H}_{2}\mathrm{O}\]we see an example of a direct proton transfer.
These reactions are not only foundational in understanding chemistry but also in practical applications such as titration in laboratories to determine concentration of solutions, and in biological systems where pH regulation is vital to life processes.