9.78* A sample of intracellular fluid contains 133 meq / L of K^+ ion. Assume the K^+comes from

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9.78* A sample of intracellular fluid contains 133 meq / L...

9.78* A sample of intracellular fluid contains $133 \mathrm{meq} / \mathrm{L}$ of $\mathrm{K}^{+}$ ion. Assume the $\mathrm{K}^{+}$comes from dissolved $\mathrm{K}_2 \mathrm{SO}_4$, and calculate the number of moles and number of grams of $\mathrm{K}_2 \mathrm{SO}_4$ that would be found in $150 . \mathrm{mL}$ of the intracellular fluid.

Key Concepts

Concentration Unit Conversion

This concept involves understanding and converting concentration units, such as milliequivalents per liter (meq/L), to moles where appropriate. Since the unit meq/L accounts for the charge of the ion present in solution, it is essential to recognize that converting to moles requires dividing or multiplying by the valence of the ion. This conversion is a common step in quantitative chemical analysis and solution chemistry.

Stoichiometric Analysis

Stoichiometry is the process of determining the relationships between reactants and products in chemical reactions. In the context of dissolved ionic compounds, it is important to use the stoichiometric ratio derived from the compound's chemical formula to relate the moles of individual ions to the moles of the overall compound. This analysis is crucial when a solute dissociates into multiple ions, as the measured concentration of one ion must be adjusted according to the number of that ion formed per formula unit.

Molar Mass Calculation

Molar mass is the mass of one mole of a given substance and is calculated by summing the atomic masses of the elements in its molecular formula. This concept is used to convert between the number of moles of a substance and its mass in grams. Understanding molar mass is fundamental in stoichiometry and is widely used in quantitative chemical calculations in both laboratory and industrial settings.

Volume Conversion

Volume conversion involves changing units to ensure consistency in calculations, particularly when using concentration values. For example, converting milliliters to liters is necessary when working with concentration units expressed per liter. This conversion is a standard practice in solution chemistry to provide accurate and consistent results in quantitative assessments.

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