Question

The reaction of borax, calcium fluoride, and concentrated sulfuric acid yields sodium hydrogen sulfate, calcium sulfate, water, and boron trifluoride as products. Write a balanced equation for this reaction.

Short answer

The balanced chemical reaction equation is \(Na_2B_4O_7 + 2CaF_2 + 7H_2SO_4 \rightarrow 2NaHSO_4 + 2CaSO_4 + 5H_2O + 2BF_3\).

Step-by-step solution

Identify the Formulas of the Chemical Compounds

First, identify and write down the formulas of the chemical compounds: Borax is \(Na_2B_4O_7\), Calcium Fluoride is \(CaF_2\), and Sulfuric acid is \(H_2SO_4\). The products are Sodium Hydrogen Sulfate (\(NaHSO_4\)), Calcium Sulfate (\(CaSO_4\)), Water (\(H_2O\)), and Boron Trifluoride (\(BF_3\)).

Write the Unbalanced Chemical Equation

Combine all the reactants and products to write the unbalanced chemical equation: \(Na_2B_4O_7 + CaF_2 + H_2SO_4 \rightarrow NaHSO_4 + CaSO_4 + H_2O + BF_3\)

Balance the Chemical Equation

Balance the chemical equation by ensuring that the number of atoms for each element on the reactant side equals the number on the product side. After adjustments, the balanced equation will be: \(Na_2B_4O_7 + 2CaF_2 + 7H_2SO_4 \rightarrow 2NaHSO_4 + 2CaSO_4 + 5H_2O + 2BF_3\)

Key concepts

Understanding the Borax Reaction

The borax reaction is a fascinating chemical process involving the transformation of compounds to produce new substances. In this context, borax (\(Na_2B_4O_7\)) reacts with calcium fluoride (\(CaF_2\)) and sulfuric acid (\(H_2SO_4\)). This reaction is interesting because it leads to the formation of substances like sodium hydrogen sulfate \((NaHSO_4)\), calcium sulfate \((CaSO_4)\), water \((H_2O)\), and boron trifluoride \((BF_3)\). Knowing these reactions helps chemists understand how different elements interact with each other.

By combining these reactants, we can predict and balance chemical equations, developing deeper insights into chemical processes. This reaction demonstrates how substances can be broken down and reassembled into entirely different compounds.

Decoding Chemical Compounds Formulas

Chemical compounds are representations of substances using chemical symbols and numbers. Each element in a compound is represented by its chemical symbol, and the number of atoms of each element is shown as a subscript. For example, in borax \((Na_2B_4O_7)\), "\(Na\)" represents sodium, and the subscript “2” means there are two sodium atoms. Similarly, \(B_4\) indicates four boron atoms, while \(O_7\) stands for seven oxygen atoms.

• Calcium fluoride \((CaF_2)\) involves calcium \((Ca)\) and two fluorine atoms \((F_2)\).
• Sulfuric acid \((H_2SO_4)\) contains two hydrogen \((H_2)\), one sulfur \((S)\), and four oxygen atoms \((O_4)\).

When writing chemical equations, formulas must be accurate, as they determine how substances will interact in a reaction. This precision is essential for balancing chemical reactions, which leads to our next topic.

Balancing Chemical Reactions Made Easy

Balancing chemical reactions ensures that there are equal numbers of each type of atom on both sides of a chemical equation. This maintains the law of conservation of mass, which states that matter cannot be created or destroyed.

To balance a chemical equation:

• Write the unbalanced equation: \(Na_2B_4O_7 + CaF_2 + H_2SO_4 \rightarrow NaHSO_4 + CaSO_4 + H_2O + BF_3\).
• Count the number of each type of atom on each side. Adjust coefficients to equalize these numbers.
• For this reaction, it involves: \(Na_2B_4O_7 + 2CaF_2 + 7H_2SO_4 \rightarrow 2NaHSO_4 + 2CaSO_4 + 5H_2O + 2BF_3\).

Each side now has the same number of sodium, boron, oxygen, calcium, fluorine, hydrogen, and sulfur atoms, showcasing a beautifully balanced equation.

Exploring Sulfuric Acid Reactions

Sulfuric acid \((H_2SO_4)\) is a powerful acid known for its ability to react with a wide range of substances. It plays a crucial role in the reaction with borax and calcium fluoride to form various products like sodium hydrogen sulfate \((NaHSO_4)\), calcium sulfate \((CaSO_4)\), water \((H_2O)\), and boron trifluoride \((BF_3)\).

In this reaction, sulfuric acid donates hydrogen ions \((H^+)\) to react with compounds, breaking down bonds and forming new substances. The production of sodium hydrogen sulfate and calcium sulfate highlights its ability to react with both salts and other compounds.

Understanding these reactions is crucial for applications in industries, where sulfuric acid is often used as a key reactant due to its strong acidic and dehydrating properties.