If 250 mL of an unknown acids was found to contain 0.45 moles of OH- ions, what concentrations was the unknown acids?
Molarity = M = moles/L. You have 0.45 moles OH^-/0.250 L = (OH^-)
Then (H^+)(OH^-) = 1E-14
Substitute and solve for (H^+)
To find the concentration of the unknown acid, we need to first calculate the concentration (in moles per liter) of OH- ions in the 250 mL solution.
Step 1: Convert the volume to liters:
250 mL = 250/1000 = 0.25 L
Step 2: Calculate the concentration of OH- ions:
0.45 moles / 0.25 L = 1.8 moles/L
Since OH- ions are present in a 1:1 ratio with hydrogen ions (H+), the concentration of the unknown acid would also be 1.8 moles/L.
To determine the concentration of the unknown acid, we need to calculate the molarity (M) of the acid solution.
First, we need to determine the number of moles of the acid. The acid and hydroxide ions react in a 1:1 ratio, meaning that for every mole of OH- ions, there is one mole of acid.
Given that 0.45 moles of OH- ions were present, this also represents the number of moles of the unknown acid.
Next, we need to calculate the molarity of the solution. Molarity is defined as the number of moles of solute per liter of solution, so we need to convert the volume from milliliters (mL) to liters (L).
The conversion factor to convert mL to L is 1 mL = 0.001 L.
Therefore, the volume of the solution is 250 mL * 0.001 L/mL = 0.25 L.
Now, we can calculate the concentration (molarity) of the unknown acid using the formula:
Molarity (M) = moles of solute / volume of solution (in liters)
Molarity = 0.45 moles / 0.25 L = 1.8 M
Hence, the concentration of the unknown acid is 1.8 M.