what volume of butyric acid would be needed to make 25.0mL of a 1.0M solution?
oh i forgot to mention that butyric acid is a liquid with a density of 1.75gr/mL
can you please explain the steps more?
thanks
If you read the post as an answer to this that had my name, it was not I that wrote that will all the bad language. I've deleted that response. As for your question, I responded below with more explanation.
To the DrBob222 impersonator. If you use my name again for one of your unauthorized diatribes, I will (not shall) ban your computer from this board. I can and will do it.
To the DrBob222 impersonator. If you use my name again for one of your unauthorized diatribes, I will (not shall) ban your computer from this board. I can and I will do it.
Sure! To determine the volume of butyric acid needed to make a 1.0M solution in 25.0mL, here are the steps:
Step 1: Understand the given information.
- The desired volume of the solution is 25.0mL.
- The desired concentration of the solution is 1.0M.
- The density of butyric acid is 1.75g/mL.
Step 2: Convert the volume of the solution to mass.
Since the density of butyric acid is given, we can use it to convert the volume of the solution to mass. The formula to convert is:
Mass = Volume x Density
Mass = 25.0mL x 1.75g/mL
Step 3: Calculate the mass of butyric acid.
Plug in the values:
Mass = 25.0mL x 1.75g/mL
Mass = 43.75g
Step 4: Use the molar mass of butyric acid to convert mass to moles.
The molar mass of butyric acid (C4H8O2) is 88.11 g/mol. Use this value to convert mass to moles using the formula:
Moles = Mass / Molar Mass
Moles = 43.75g / 88.11 g/mol
Step 5: Calculate the volume of butyric acid needed.
Since the molarity of the solution is 1.0M, it means that 1 mole of butyric acid is dissolved in 1 liter (1000 mL) of solution. Therefore, we can use this information to determine the volume of butyric acid needed:
Volume = Moles / Molarity
Volume = 0.496 mol / 1.0 mol/L
Volume = 0.496 L = 496 mL
Therefore, you would need approximately 496 mL of butyric acid to make a 25.0 mL of 1.0 M solution.
Please note that the calculations are based on ideal conditions and assume that the solution is being prepared in a way that does not result in any change in volume or change in concentration due to chemical reactions or other factors.