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------------------------------------------------ What is the molarity of a solution prepared by dissolving 0.240 g of LiOH in 6.00 mL of solution?

The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters. In this case, the molarity of the LiOH solution is approximately 1.67 M.

Explanation:

To find the molarity (M) of a solution, you need to know the number of moles of solute (LiOH) and the volume of the solution in liters. Let's break down the steps to calculate the molarity of the LiOH solution:

Calculate the number of moles of LiOH:

First, determine the molar mass of LiOH. Lithium (Li) has an atomic mass of approximately 6.94 g/mol, and hydroxide (OH) has a molar mass of approximately 17.01 g/mol.

Molar mass of LiOH = (6.94 g/mol for Li) + (17.01 g/mol for OH) = 23.95 g/mol

Now, calculate the number of moles of LiOH using the given mass:

Moles of LiOH = (0.240 g LiOH) / (23.95 g/mol LiOH) = 0.01002 moles LiOH

Calculate the volume in liters:

The volume of the solution is given as 6.00 ml. To convert this to liters, divide by 1000 (since 1 liter = 1000 ml):

Volume in liters = 6.00 ml / 1000 = 0.00600 L

Calculate the molarity:

Now that you have the moles of LiOH (0.01002 moles) and the volume in liters (0.00600 L), you can calculate the molarity:

Molarity (M) = Moles of solute / Volume of solution in liters

Molarity (M) = 0.01002 moles / 0.00600 L = 1.67 M

The molarity of the LiOH solution is approximately 1.67 moles per liter, or 1.67 M. This means that there are 1.67 moles of LiOH dissolved in one liter of the solution.

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