Calculate the mass needed for each of the following ion...

Calculate the mass needed for each of the following ion equivalents:
(a) $0.25 \mathrm{Eq} \mathrm{Ca}^{2+}$
(b) $75 \mathrm{mEq} \mathrm{K}^{+}$
(c) $199 \mathrm{mEg} \mathrm{SO}_{4}^{2-}$
(d) $0.65 \mathrm{Eq} \mathrm{PO}_{4}^{3-}$

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Key Concepts

Equivalent and Milliequivalent Concept

This concept refers to a measure of chemical reactivity, particularly in acid-base and redox reactions, where one equivalent is the amount of substance that will combine with or displace one mole of hydrogen ions (H+) or electrons. Milliequivalents (mEq) are simply one thousandth of an equivalent. Understanding this concept is vital for converting between the weight of an ion and its reactivity based on its charge.

Molar Mass and Molecular Weight

Molar mass is the mass of one mole of a substance and is expressed in grams per mole. It plays a crucial role in converting between moles (or equivalents) and grams. When calculating the mass needed per equivalent of an ion, the molar mass, adjusted by the ion's valence, is used to determine the proportion of the substance that corresponds to one equivalent.

Valence and Charge Factor

The valence, or charge, of an ion indicates how many electrons it can lose, gain, or share when it reacts. This charge is essential for converting between moles and equivalents because an ion with a higher charge will have a different relationship between its molar mass and the number of equivalents. For instance, an ion with a +2 charge will have one equivalent equal to half a mole of that ion, making the adjustment for its reactivity based on its charge factor.

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