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
There isn't much explaining.
Definition of molarity is
M = # moles/L solution.
So you want moles. You have L soln in the problem as 25.0 mL = 0.025L. And you have M in the problem as 1.0 M. So all we need to do is find moles needed.
M = moles/L or moles = M x L = 1.0 x 0.025 = 0.025 moles.
Now, how do we find moles?
moles = grams/molar mass
0.025 moles = grams/molar mass.
What's the molar mass. Approximately 88 so 0.025 = g/88 and g = 0.025*88 = 2.20 g approximately.
The problem asks for volume. Use the density to convert grams to mL.
thank you
Certainly! To determine the volume of butyric acid needed to make a 25.0 mL solution with a concentration of 1.0 M, we can follow these steps:
Step 1: Convert the density of butyric acid to grams per milliliter (g/mL).
Given: The density of butyric acid is 1.75 g/mL.
Step 2: Convert the given volume of the solution (25.0 mL) to liters.
Since the unit of concentration is in Molarity (M), the volume needs to be in liters. 1 mL is equivalent to 0.001 L (since there are 1000 mL in a liter), so 25.0 mL is equal to 0.025 L.
Step 3: Use the formula for Molarity (M) to calculate the number of moles (mol) needed.
The formula for Molarity (M) is shown as M = moles/volume (in liters). Rearranging this formula, we have moles = M × volume (in liters). In this case, the concentration (M) is given as 1.0 M, and the volume (in liters) is 0.025 L. Therefore, the number of moles needed is 1.0 M × 0.025 L = 0.025 mol.
Step 4: Calculate the mass of butyric acid needed using the moles and density.
Using the formula mass = moles × molar mass, we need to find the molar mass of butyric acid. The molar mass of butyric acid (C4H8O2) is found by adding up the atomic masses of carbon (C), hydrogen (H), and oxygen (O) in the molecule. Carbon has a molar mass of 12.01 g/mol, hydrogen has a molar mass of 1.01 g/mol, and oxygen has a molar mass of 16.00 g/mol. So, the molar mass of butyric acid is (4 * 12.01 g/mol) + (8 * 1.01 g/mol) + (2 * 16.00 g/mol) = 88.11 g/mol.
Now, we can calculate the mass of butyric acid needed using the moles and density. The mass (in grams) is equal to 0.025 mol × 88.11 g/mol = 2.20 g.
Step 5: Convert the mass of butyric acid to volume using the density.
Since the density of butyric acid is given as 1.75 g/mL, we can use the formula volume = mass/density to find the volume (in milliliters) needed. The volume is equal to 2.20 g / 1.75 g/mL = 1.26 mL.
Therefore, approximately 1.26 mL of butyric acid would be needed to make 25.0 mL of a 1.0 M solution.
Please note that these calculations assume ideal behavior and a dilute solution, and the actual volume required might vary slightly in practice due to experimental uncertainties.