Hello everyone
I need your help at once.
How many grams of CO2 are needed to neutralize a 5 L tank of water with a pH of 11.5?
my answer is around 220 grams of CO2.
is that true or not?
I don't get anywhere near that figures but I may have made some wrong assumptions. If you wish to show your work I'll be happy to check it.
Thank you very much indeed for your effort and quick response Sir.
Please, kindly write your valuable solution down.
I guess that my solution is likely to be wrong.
it is necessary to mention that co2 is a one of oil reservoir components at the following conditions: mole percent= 3.6%, reservoir Press. = 3000 - 5000 psi and reservoir Temp. = 200-240 oF.
meanwhile, the figure above has been mistaken and must be corrected to 0.220 gr co2.
honestly speaking, my field is chemical engg. and don't have a good knowledge in this regard.
I solved my question through the solution method of the following sample that had answered in this website and used co2 instead of HCL and set a pH of 7!!!! therefore, the figure of .220 gram of co2 must be wrong.
How many grams of HCl are needed to change 1000 L of water with a pH of 11 to a pH of 5.5?
To determine the number of grams of CO2 needed to neutralize a 5 L tank of water with a pH of 11.5, we need to follow a series of steps.
Step 1: Calculate the concentration of hydroxide ions (OH-) in the water.
Since pH is a measure of the concentration of hydrogen ions (H+), we can use the pH to find the concentration of hydroxide ions. The pH scale is logarithmic, so to convert a pH value to concentration, we'll use the formula: [OH-] = 10^(-pOH), where pOH is equal to 14 (the pOH value at neutrality) minus the given pH value.
In this case, pOH = 14 - 11.5 = 2.5.
Step 2: Calculate the amount of OH- ions in moles.
We multiply the concentration of hydroxide ions obtained from Step 1 by the volume of water in liters:
Amount of OH- ions (in moles) = Concentration of OH- ions × Volume of water in liters.
Step 3: Calculate the number of moles of CO2 required to neutralize the OH- ions.
The balanced chemical equation for the reaction between CO2 and OH- ions is: CO2 + 2OH- → H2CO3.
From the equation, we can see that 1 mole of CO2 reacts with 2 moles of OH- ions. Therefore, the number of moles of CO2 needed to neutralize the OH- ions is half the amount of OH- ions in moles obtained from Step 2.
Step 4: Calculate the number of grams of CO2 required.
To convert from moles to grams, we need to know the molar mass of CO2, which is approximately 44 grams/mol:
Mass of CO2 (in grams) = Number of moles of CO2 × Molar mass of CO2.
Now, let's calculate the answer using these steps.
Step 1: [OH-] = 10^(-2.5) = 0.003162 M
Step 2: Amount of OH- ions (in moles) = 0.003162 M × 5 L = 0.01581 moles
Step 3: Number of moles of CO2 needed = 0.01581 moles / 2 = 0.007905 moles
Step 4: Mass of CO2 (in grams) = 0.007905 moles × 44 grams/mol ≈ 0.347 grams
Therefore, the correct answer is approximately 0.347 grams of CO2, not 220 grams as you mentioned.