Determine the volume of 0.150 M NaOH that neutralizes 0.188 g of a diprotic acid having a molar mass of 152.2 g/mol?
Let's let the diportic acid be H2A.
The equation is
H2A + 2NaOH ==> Na2A + 2H2O
moles H2A = 0.188/152.2
Convert moles H2A to moles NaOH using the coefficients in the balanced equation.
Now convert moles NaOH to L using M = moles/L.
To determine the volume of the NaOH solution that neutralizes the given quantity of a diprotic acid, we need to apply the concept of stoichiometry.
First, calculate the number of moles of the diprotic acid. This can be done using the formula:
moles = mass (g) / molar mass (g/mol)
moles of diprotic acid = 0.188 g / 152.2 g/mol
Now, since NaOH is a strong base, it reacts with the diprotic acid in a 1:2 ratio. This means that 1 mole of diprotic acid reacts with 2 moles of NaOH.
Using this stoichiometric ratio, we can determine the number of moles of NaOH needed to neutralize the given moles of acid:
moles of NaOH = 2 * moles of diprotic acid
Next, we need to convert the moles of NaOH into volume using the molarity (M) of NaOH solution. Molarity is defined as the number of moles of solute (NaOH) divided by the volume of the solution in liters:
Molarity (M) = moles of solute / volume of solution (in liters)
Rearranging the equation, we can solve for the volume of the solution:
Volume of solution (in liters) = moles of solute / molarity (M)
In this case, the molarity of NaOH solution is given as 0.150 M. Substitute the known values into the equation to calculate the volume of the NaOH solution:
Volume of NaOH solution (in liters) = moles of NaOH / molarity (M)
Finally, convert the volume from liters to milliliters (mL) if desired:
Volume (in mL) = Volume (in liters) * 1000
Therefore, following these steps will allow us to determine the volume of the 0.150 M NaOH solution that neutralizes 0.188 g of a diprotic acid with a molar mass of 152.2 g/mol.