How many grams of solute would you use to prepare the following solutions? (b) 1.50 L of 0.250 M glucose (C6H12O6)

Verified step by step guidance

1. Identify the formula for molarity: \( M = \frac{n}{V} \), where \( M \) is molarity, \( n \) is the number of moles of solute, and \( V \) is the volume of the solution in liters.
2. Rearrange the formula to solve for the number of moles of solute: \( n = M \times V \).
3. Substitute the given values into the equation: \( n = 0.250 \, \text{M} \times 1.50 \, \text{L} \).
4. Calculate the number of moles of glucose using the values from the previous step.
5. Use the molar mass of glucose (\( C_6H_{12}O_6 \)) to convert moles to grams. The molar mass of glucose is approximately 180.18 g/mol. Multiply the number of moles by the molar mass to find the mass in grams.

Key Concepts

Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L). Understanding molarity is crucial for calculating how much solute is needed to achieve a desired concentration in a given volume of solution.

Moles of Solute

A mole is a unit that quantifies the amount of substance. One mole of any substance contains Avogadro's number of entities (approximately 6.022 x 10^23). To find the number of moles needed for a solution, you multiply the molarity by the volume of the solution in liters.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between moles and grams. For glucose (C6H12O6), the molar mass is approximately 180.18 g/mol, which is used to calculate the mass of solute required for the solution.