Question

Rochelle salt is the tetrahydrate of \(\mathrm{KNaC}_{4} \mathrm{H}_{4} \mathrm{O}_{6},\) which means there are four molecules of water per \(\mathrm{KNaC}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) Write the formula for Rochelle salt.

Short answer

The chemical formula for Rochelle salt is \(KNaC_4H_4O_6 \cdot 4H_2O\).

Step-by-step solution

Identifying the Components

Rochelle salt consists of a compound with the formula \(KNaC_4H_4O_6)\), which is potassium sodium tartrate, and it is a tetrahydrate meaning it has four water molecules (\(H_2O\)) associated with it.

Writing the Formula for the Tetrahydrate

To write the formula for the tetrahydrate of potassium sodium tartrate, write the formula of the compound and then add \(\cdot 4H_2O\) to indicate the four water molecules per formula unit.

Combining the Compound and Water Molecules

Combine the potasssium sodium tartrate unit with the four water molecules to get the final formula: \(KNaC_4H_4O_6 \cdot 4H_2O\).

Key concepts

Potassium Sodium Tartrate

Potassium sodium tartrate, known historically as Rochelle salt, is an important chemical compound used in various applications including baking, as a pH buffer, and in electroplating. It consists of equal parts sodium and potassium cations and the tartrate anion, a derivative of tartaric acid. Its key characteristic is its ability to form stable complexes with other ions, which is beneficial in analytical chemistry for identifying the presence of certain metal ions.

The compositional balance between potassium and sodium is crucial for its effectiveness. Formally, this compound embodies both monovalent cations, which are essential to maintain the charge neutrality with the doubly negatively charged tartrate anion. This sophisticated synergy is an excellent example of how ionic compounds are structured to ensure stability and functionality.

Understanding the composition and structure of potassium sodium tartrate provides insights into its solubility behavior in water and its capability to crystallize into various hydrate forms, including its tetrahydrate variant—Rochelle salt. This knowledge is instrumental for students and professionals in fields such as food science, pharmacology, and chemistry.

Chemical Hydrates

Chemical hydrates are compounds that contain water molecules bound within their crystalline structure. These water molecules are essential for the formation of the crystal and its physical properties. In the case of Rochelle salt, the water is not loosely attached; rather, it's integrated into the structure, forming a tetrahydrate. This means each formula unit of the salt will have four water molecules associated with it.

Understanding hydrates is critical because their formation can alter the mass, solubility, and various other properties of the original compound. Dehydration, which is the loss of these water molecules, can occur when the hydrate is exposed to heat or reduced pressure. This can be a crucial factor in industries like pharmaceuticals, where the hydration state of a compound can significantly affect its usability and effectiveness. Hydrates also highlight the dynamic interactions between ionic compounds and water, underscoring the adaptability of substances through physical changes.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships of the reactants and products in a chemical reaction. It is essentially the math behind chemistry, enabling chemists to predict the amounts of substances consumed and produced in a given reaction. In the context of Rochelle salt's formation, stoichiometry provides the ratio of potassium sodium tartrate to water molecules, which is 1:4 in this case.

When we say Rochelle salt is a tetrahydrate, stoichiometry clarifies that there are precisely four water molecules for every one unit of potassium sodium tartrate. Through stoichiometric calculations, one can determine the amount of starting materials required to create a given amount of Rochelle salt. These calculations are pivotal in ensuring that chemical reactions are carried out efficiently in laboratories and industry without wasting reactants.

Students often use stoichiometric principles to balance chemical equations and to understand the principles of conservation of mass and mole ratio. Grasping these concepts is invaluable not only in academics but also in a variety of scientific careers, where precise formulations and reactions are the cornerstones of product development and quality control.