C06 in lab you want to prepare 4.0 liters of a 1.5 M glucose solution. You will need (1 moles of glucose to prepare this solution.
Select answer choice
6.0
2.7
5.5
The correct answer and explanation is :
Let’s analyze the problem step-by-step:
Problem:
You want to prepare 4.0 liters of a 1.5 M glucose solution. How many moles of glucose do you need?
Step 1: Understanding Molarity (M)
Molarity (M) is defined as: M=moles of soluteliters of solutionM = \frac{\text{moles of solute}}{\text{liters of solution}}
This means: moles of solute=M×liters of solution\text{moles of solute} = M \times \text{liters of solution}
Step 2: Apply the formula
Given:
- Molarity (M) = 1.5 M
- Volume (V) = 4.0 L
Calculate moles: moles=1.5 mol/L×4.0 L=6.0 moles\text{moles} = 1.5 \, \text{mol/L} \times 4.0 \, \text{L} = 6.0 \, \text{moles}
Step 3: Conclusion
You will need 6.0 moles of glucose to prepare 4.0 liters of a 1.5 M glucose solution.
Explanation (300 words):
Molarity is a common way to express the concentration of a solution, defined as the number of moles of solute dissolved in one liter of solution. In this problem, the goal is to prepare 4.0 liters of glucose solution at a molarity of 1.5 M. This means each liter of the solution contains 1.5 moles of glucose.
To find the total moles of glucose required, you multiply the molarity by the total volume of the solution. Since molarity is moles per liter, multiplying it by the volume (in liters) gives the total moles needed.
The calculation is straightforward: moles=molarity×volume=1.5×4.0=6.0 moles\text{moles} = \text{molarity} \times \text{volume} = 1.5 \times 4.0 = 6.0 \text{ moles}
This means that to make a 4.0-liter solution of 1.5 M glucose, you must dissolve 6.0 moles of glucose into enough water to make the total volume 4.0 liters.
This approach assumes the final volume is 4.0 liters (not adding glucose to 4.0 liters but making the total volume 4.0 liters after glucose is dissolved). Molarity depends on final volume, so after adding the glucose, you add water until the solution reaches exactly 4.0 liters.
This calculation is important in lab preparations because accurate concentrations are essential for reproducible and reliable results in experiments involving chemical reactions, biological assays, or clinical tests.
Final Answer:
6.0 moles