How many milliequivalents of [tex]K^+[/tex] would be contained in 100 mL of the following solution?

- Potassium Chloride (KCl): [tex]5 \, \text{g}[/tex]
- Potassium Sulfate ([tex]K_2SO_4[/tex]): Not specified
- Purified water q.s. ad 100 mL

Molecular Weights:
- KCl: [tex]74.5 \, \text{g/mol}[/tex]
- [tex]K_2SO_4[/tex]: [tex]174.25 \, \text{g/mol}[/tex]

A. 1450 mEq
B. 1670 mEq
C. 2250 mEq
D. 1243 mEq

The milliequivalents of K+ in the solution is calculated based on the amounts of K+ in the two substances (KCl and K2SO4) present in the solution. The total milliequivalents of K+ in the solution would be 1244mEq.

Explanation:

To calculate the milliequivalents of K+ in the solution, we must first know the millimoles of potassium present in the solution, as 1 milliequivalent of K+ is equal to 1 millimole.

In Potassium Chloride(KCl), the molecular weight of potassium(K) is approximately 39.1g, therefore the millimoles of K+ from the 5g of KCl is (5g/74.5g/mol)*1000 = 67.1mmol.

Similarly, Potassium Sulphate(K2SO4) contains two atoms of K+ per molecule, so the weight of K in it is approximately 78.2g. Therefore, the millimoles of K+ from the 5g of Potassium Sulphate is (5g/174.25g/mol)*2*1000 = 57.3mmol.

Then we add the two values for the total millimoles of K+ in solution, 67.1+57.3 = 124.4mmol, or when speaking in terms of equivalents, 1244mEq.

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