The concentration of an aqueous solution of `0.01 M CH_(3)OH` solution is very nearly equal to which of the following

Options

A. `0.01% CH_(3)OH`
B. `0.01m CH_(3)OH`
C. `x_(CH_(3)OH)=0.01`
D. `0.01N CH_(3)OH`

Explanation

To solve the problem of determining the concentration of a 0.01 M CH₃OH (methyl alcohol) solution, we can follow these steps:

### Step 1: Understand Molarity
Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, we have a 0.01 M solution of CH₃OH, which means there are 0.01 moles of CH₃OH in 1 liter of solution.

### Step 2: Consider the Density of Water
The problem states that the solution is aqueous, meaning water is the solvent. The density of water is approximately 1 g/mL, which means 1 liter of water has a mass of about 1000 grams.

### Step 3: Relate Molarity to Molality
In solutions where the density of the solvent (water) is 1 g/mL, molarity and molality can be considered nearly equal. This is because molality (m) is defined as the number of moles of solute per kilogram of solvent. Since 1 liter of water weighs about 1 kg, the molarity and molality will be very similar.

### Step 4: Calculate the Concentration
Given that the molarity is 0.01 M, we can conclude that the molality will also be approximately 0.01 m. Therefore, the concentration of the 0.01 M CH₃OH solution is very nearly equal to 0.01 m.

### Conclusion
Thus, the concentration of the aqueous solution of 0.01 M CH₃OH is very nearly equal to 0.01 m (molality).

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