What kind of solution would you have if it contained 50 grams of sodium chloride in 100 mL of water at 30˚C?
The Correct Answer and Explanation is:
To determine the type of solution containing 50 grams of sodium chloride (NaCl) in 100 mL of water at 30°C, we first need to calculate the concentration of the sodium chloride solution. The concentration can be calculated using the formula for molarity:
[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
]
Step 1: Calculate the Moles of Sodium Chloride
First, we need to find the molar mass of sodium chloride (NaCl). The molar mass is calculated as follows:
- Sodium (Na) = 22.99 g/mol
- Chlorine (Cl) = 35.45 g/mol
[
\text{Molar mass of NaCl} = 22.99 + 35.45 = 58.44 \, \text{g/mol}
]
Next, we convert the mass of NaCl into moles:
[
\text{Moles of NaCl} = \frac{50 \, \text{g}}{58.44 \, \text{g/mol}} \approx 0.856 \, \text{mol}
]
Step 2: Calculate the Volume in Liters
Since we have 100 mL of water, we convert this to liters:
[
100 \, \text{mL} = 0.1 \, \text{L}
]
Step 3: Calculate the Molarity
Now, we can calculate the molarity of the solution:
[
\text{Molarity} = \frac{0.856 \, \text{mol}}{0.1 \, \text{L}} = 8.56 \, \text{M}
]
Step 4: Classify the Solution
An 8.56 M sodium chloride solution is highly concentrated, indicating that it is a hypertonic solution. In biological terms, a hypertonic solution has a higher concentration of solutes compared to the inside of a cell. This can lead to osmosis, where water moves out of cells, potentially causing them to shrink. Such solutions are often used in various applications, including laboratory experiments and medical treatments, but they can also be hazardous if cells are exposed to them for extended periods.
In conclusion, the solution containing 50 grams of sodium chloride in 100 mL of water at 30°C is a highly concentrated hypertonic solution, which can have significant implications in biological and chemical contexts.