We will calculate the amount of acid to use in each titration. Assume that you are using 0.0512 M NaOH(aq). A good volume of NaOH(aq) to use per titration is 15 mL. From this molarity and volume, the moles of NaOH can be calculated. Since the unknown acid is monoprotic, this also equals the number of moles of acid to use. A typical molar mass for an unknown acid in this experiment is 380 g/mol. Using this molar mass, calculate the mass (in grams) of unknown acid you should use per titration. Since we have been estimating values, round your answer to two significant figures. (need detailed help, not good with this at all)
To calculate the mass of the unknown acid to use per titration, we can follow these steps:
Step 1: Calculate the moles of NaOH used per titration.
Given that the concentration of NaOH solution is 0.0512 M, and the volume used is 15 mL (or 0.015 L), we can use the equation:
moles of NaOH = concentration (M) × volume (L)
moles of NaOH = 0.0512 M × 0.015 L = 0.000768 moles of NaOH
Step 2: Determine the moles of acid to use.
Since the unknown acid is monoprotic, moles of NaOH will also be equal to moles of acid.
moles of acid = moles of NaOH = 0.000768 moles
Step 3: Calculate the mass of the unknown acid.
Given that the molar mass of the unknown acid is 380 g/mol, we can use the equation:
mass (g) = moles × molar mass
mass (g) = 0.000768 moles × 380 g/mol = 0.29216 g
Step 4: Round the answer to two significant figures.
Rounding the calculated mass to two significant figures, we get:
mass (g) = 0.29 g
Therefore, you should use 0.29 grams of the unknown acid per titration.