Question

How many equivalents of hydroxide ion are needed to react with 1.53 equivalents of hydrogen ion? How did you know this when no balanced chemical equation was provided for the reaction?

Short answer

1.53 equivalents of hydroxide ions are needed to react with 1.53 equivalents of hydrogen ions in a neutralization reaction. We can determine this without a balanced chemical equation because neutralization reactions occur when the equivalents of hydrogen ions (H⁺) and hydroxide ions (OH⁻) are equal, as shown in the equation: \(H⁺ + OH⁻ → H₂O\).

Step-by-step solution

Understand the concept of neutralization

In a neutralization reaction, an acid reacts with a base to form water. In this process, hydrogen ions (H⁺) from the acid combine with hydroxide ions (OH⁻) from the base, forming water (H₂O). The overall equation for neutralization is: \(H⁺ + OH⁻ → H₂O\) The neutralization is complete when the number of equivalents of hydrogen ions equals the number of equivalents of hydroxide ions.

Use the given information to determine the required equivalents of hydroxide ion

We are given 1.53 equivalents of hydrogen ions. To completely neutralize this amount of hydrogen ions, we have to supply an equal number of hydroxide ions. So, the required equivalents of hydroxide ion would be 1.53.

Provide the final answer

1.53 equivalents of hydroxide ions are needed to react with 1.53 equivalents of hydrogen ions in a neutralization reaction. We can determine this without a balanced chemical equation because neutralization reactions occur when the equivalents of hydrogen ions and hydroxide ions are equal.

Key concepts

Equivalents of Hydrogen Ion

Understanding the concept of \( H^+ \) equivalents is crucial for delving into acid-base chemistry. An equivalent of a hydrogen ion is a measure of its capacity to combine with or displace other substances in a chemical reaction, particularly during neutralization. This is strongly associated with the concept of normality, which is the number of equivalents per liter of solution.

In neutralization reactions, we measure the acidity or basicity based on the number of hydrogen ions or hydroxide ions present. Since one hydrogen ion can potentially neutralize one hydroxide ion, the equivalents of \( H^+ \) will directly tell you how much of \( OH^- \) is needed for the reaction to reach completion. This 1:1 ratio is the backbone of simple neutralization equations.

To simplify, imagine the hydrogen ion as a single puzzle piece, and the hydroxide ion as the matching piece. Just one of each is needed to complete the puzzle. This analogy can help students visualize why the equivalents must match for the reaction to proceed effectively.

Hydroxide Ion

Let's focus on the hydroxide ion, commonly represented as \( OH^- \). This polyatomic ion is composed of one oxygen atom bonded to a hydrogen atom, with an extra electron giving it a negative charge. It plays a fundamental role in the chemistry of bases. When dissolved in water, a substance that releases hydroxide ions is termed a base and is said to be alkaline.

Similar to the hydrogen ion, the hydroxide ion has equivalents which signify its capability to neutralize an equivalent amount of acid, typically represented by the \( H^+ \) ions. When the equivalents of hydrogen ions and hydroxide ions are equal, such as in our exercise where 1.53 equivalents of \( H^+ \) require 1.53 equivalents of \( OH^- \), it signifies complete neutralization. This relationship makes understanding reactions intuitive: for every acid particle there needs to be a base particle for neutralization to occur.

Chemical Equation

A chemical equation is a symbolic representation of a chemical reaction where reactants are transformed into products. It shows the substances involved and their respective quantities. In the context of neutralization, the reaction typically involves an acid and a base, and the equation will reflect their interaction to form water and possibly a salt.

While a chemical equation provides a detailed look at the substances and their stoichiometry, neutralization reactions offer simplicity due to the 1:1 molar relationship between hydrogen and hydroxide ions for the formation of water. This means that, even without a full chemical equation provided, knowledge of one reactant's equivalents allows the determination of the other's required quantity.

In educational terms, this can be an excellent introduction to stoichiometry for students, as it simplifies the concept of mole-to-mole relationships to a basic principle that is easily visualized and understood.