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If the density of ocean water at a depth of 1.00 x 104 m is 1.071 g/mL and if 26.0 g of water at that depth contains 182mg of potassium chloride, what is the molarity of potassium chloride in the sample?

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Answer:

Molarity of potassium chloride is 0.100M

Explanation:

Molarity is defined as moles of solute per liter of solvent.

Moles of solute (Potassium chloride; MW: 74.55g/mol):

0.182g × (1mol / 74.55g) = 2.44x10⁻³mol KCl

Liters of water using density are:

26.0g Water × ( 1mL / 1.071g) × (1L / 1000mL) = 0.0243L

Thus, molarity of KCl in the sample is:

2.44x10⁻³mol KCl / 0.0243L = 0.100M

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