A handbook gives the aqueous solubility of carbon monoxide at 0 °C and 1 atm CO pressure to be 0.0354 mg CO per mL of solution to obtain 0.100 M CO?
To determine the amount of carbon monoxide (CO) in milligrams required to produce a 0.100 M CO solution at 0 °C and 1 atm CO pressure, we can use a few calculations.
First, let's define the given data:
- Aqueous solubility of CO at 0 °C and 1 atm CO pressure: 0.0354 mg CO/mL
We need to find the amount of CO needed to obtain a 0.100 M CO solution.
To achieve this, follow these steps:
Step 1: Convert the molarity (M) to moles per liter (mol/L):
We know that 0.100 M CO means 0.100 moles of CO dissolved in 1 liter of solution.
Step 2: Calculate the volume of the solution required to achieve 0.100 M CO:
We can use the equation:
moles = Molarity × volume (L)
Rearranging the equation:
volume (L) = moles / Molarity
For 0.100 moles of CO in 1 liter of solution (0.100 M), the volume required will be 1 liter.
Step 3: Convert the volume from liters to milliliters:
Since we were given the solubility in mg/mL, we need to convert the volume from liters to milliliters.
1 liter = 1000 milliliters
Therefore, 1 liter is equal to 1000 mL.
Step 4: Calculate the amount of CO in milligrams:
To determine the amount of CO required to obtain a 0.100 M CO solution, we multiply the volume (in mL) by the solubility (in mg/mL).
Amount of CO (mg) = volume (mL) × solubility (mg/mL)
In this case, the volume is 1000 mL (as calculated in Step 3), and the solubility is given as 0.0354 mg CO/mL.
Substituting the values:
Amount of CO (mg) = 1000 mL × 0.0354 mg CO/mL
Calculating this:
Amount of CO (mg) = 35.4 mg
Therefore, to obtain a 0.100 M CO solution at 0 °C and 1 atm CO pressure, you would need 35.4 milligrams of CO.