How many milliliters of 1.40 M KOH solution are needed to provide 0.120 mol of KOH?

please explain how to solve

M = moles/L

Solve for L and convert to mL.

To solve this problem, you can use the equation which relates the amount of substance (in moles), concentration (in moles per liter), and volume (in liters):

moles = concentration × volume

First, rearrange the equation to solve for volume:

volume = moles / concentration

Now, plug in the given values:

moles = 0.120 mol
concentration = 1.40 M

volume = 0.120 mol / 1.40 M

Calculate:

volume = 0.0857 L

Finally, convert liters to milliliters by multiplying by 1000:

volume = 0.0857 L × 1000 mL/L

volume ≈ 85.7 mL

Therefore, you would need approximately 85.7 milliliters of the 1.40 M KOH solution to provide 0.120 mol of KOH.

To determine the volume of a solution needed to provide a specific amount of a solute, you can use the formula:

Volume (in liters) = Amount of solute (in moles) / Concentration of the solution (in moles per liter)

In this case, we need to calculate the volume of a 1.40 M KOH solution needed to provide 0.120 mol of KOH.

Step 1: Convert the amount of KOH from moles to millimoles (mmol). Since 1 mol = 1000 mmol, multiply 0.120 mol by 1000 to get 120 mmol.

Step 2: Use the formula to calculate the volume of the solution:
Volume (in liters) = 120 mmol / 1.40 mol/L

Step 3: Convert the volume from liters to milliliters (mL). Since 1 L = 1000 mL, multiply the volume in liters by 1000 to get the solution volume in milliliters.

Therefore, the solution will require 120 mmol of KOH, which is equivalent to 85.7 mL of 1.40 M KOH solution.