How many grams of CO2 are needed to neutralize a 5 liters water with a pH of 11 to 7? under the following conditions:
P: 4000 psi, T:230 oF
Note: CO2 is a one of oil reservoir fluid components with mole percent 0f 3.6%.
thanks a million
To calculate the number of grams of CO2 needed to neutralize the water, we need to determine the amount of CO2 required to reduce the pH from 11 to 7.
Step 1: Find the initial concentration of hydroxide ions (OH-) in the water.
Since the pH is 11, we can use the formula:
pOH = 14 - pH
pOH = 14 - 11 = 3
Step 2: Calculate the concentration of hydroxide ions (OH-) using the formula:
[OH-] = 10^(-pOH)
[OH-] = 10^(-3) = 0.001 M
Step 3: Calculate the concentration of hydrogen ions (H+) using the formula:
[H+] = 1 x 10^(-pH)
[H+] = 1 x 10^(-7) = 0.0000001 M
Step 4: Determine the moles of OH- and H+ ions in the water.
Since water has a 1:1 ratio of OH- to H+ ions, the number of moles for both ions will be the same.
Step 5: Calculate the moles of water using the formula:
moles of water = volume (L) / molar volume (L/mol)
Given a volume of 5 liters, we can convert this to moles using the ideal gas law:
PV = nRT
Step 6: Convert the mole percent of CO2 to a decimal.
The mole percent of CO2 is given as 3.6%. To convert this to a decimal, divide by 100:
3.6 / 100 = 0.036
Step 7: Use the mole percent of CO2 to find the moles of CO2 in the oil reservoir fluid.
Multiply the mole percent by the total moles of the oil reservoir fluid.
Step 8: Convert the moles of CO2 to grams using the molar mass.
The molar mass of CO2 is approximately 44 g/mol. Multiply the moles of CO2 by the molar mass to obtain the grams.
By following these steps, you should be able to calculate the number of grams of CO2 needed to neutralize the water under the given conditions.