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If 500 ml of 1 M solution of glucose is ...

If 500 ml of 1 M solution of glucose is mixed with 500ml of 1M solution of glucose final moalrity of solution will be:

A

1M

B

0.5M

C

2M

D

1.5M

Text Solution

AI Generated Solution

The correct Answer is:
To find the final molarity of the solution when 500 mL of 1 M glucose solution is mixed with another 500 mL of 1 M glucose solution, we can follow these steps: ### Step 1: Calculate the number of moles of glucose in each solution - **Molarity (M)** is defined as moles of solute per liter of solution. - For the first solution: \[ \text{Moles of glucose} = \text{Molarity} \times \text{Volume (in L)} = 1 \, \text{M} \times 0.5 \, \text{L} = 0.5 \, \text{moles} \] - For the second solution (which is identical): \[ \text{Moles of glucose} = 1 \, \text{M} \times 0.5 \, \text{L} = 0.5 \, \text{moles} \] ### Step 2: Calculate the total number of moles of glucose - Total moles of glucose after mixing both solutions: \[ \text{Total moles} = 0.5 \, \text{moles} + 0.5 \, \text{moles} = 1 \, \text{mole} \] ### Step 3: Calculate the total volume of the mixed solution - Total volume after mixing: \[ \text{Total volume} = 500 \, \text{mL} + 500 \, \text{mL} = 1000 \, \text{mL} = 1 \, \text{L} \] ### Step 4: Calculate the final molarity of the mixed solution - Final molarity (M) is calculated using the formula: \[ \text{Molarity} = \frac{\text{Total moles}}{\text{Total volume (in L)}} \] - Substituting the values: \[ \text{Final molarity} = \frac{1 \, \text{mole}}{1 \, \text{L}} = 1 \, \text{M} \] ### Final Answer: The final molarity of the solution after mixing is **1 M**. ---
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