Calculate amount (in grams) of unknown acid used for titration. You want 30 mL of titrant to get the equivalence point. Assume that the base is 0.05 M and the unknown acid molar mass is around 400 g/mol.

Well, well, well, looks like we have ourselves a titration conundrum! Let's get cracking, shall we?

To find the amount of unknown acid used for titration, we need to use the equation M1V1 = M2V2, where M1 is the molarity of the base, V1 is the volume of the base used, M2 is the molarity of the acid, and V2 is the volume of the acid used.

We're given that the base has a concentration of 0.05 M and we want to reach the equivalence point with 30 mL of titrant. So, we have M1 = 0.05 M and V1 = 30 mL (which we'll convert to L by dividing by 1000).

Now, to get the moles of acid used, we'll rearrange the equation: M2 = (M1V1) / V2.

Since we want to find the amount of acid in grams, we'll use moles of acid to do the conversion. The molar mass of the unknown acid is given as around 400 g/mol.

Putting it all together, let's calculate!

M2 = (0.05 M * (30 mL / 1000)) / V2

Now, I need one more piece of information. What's the volume of the unknown acid used during titration?

To calculate the amount (in grams) of the unknown acid used for titration, you need to consider the molar ratio between the acid and base. Let's follow these steps:

Step 1: Determine the volume of the base used for titration.
Given that the desired volume of titrant (base) is 30 mL, this will be the volume of the base used for the titration.

Step 2: Calculate the number of moles of the base used.
Since the base concentration is 0.05 M (moles per liter), we can use the formula:
moles = concentration (M) × volume (L)
moles = 0.05 M × 0.030 L
moles = 0.0015 mol

Step 3: Determine the molar ratio between the base and the acid.
According to the balanced chemical equation for the reaction between the acid and the base, there is a 1:1 molar ratio. This means that for every 1 mole of base, there is 1 mole of acid.

Step 4: Calculate the number of moles of the unknown acid used.
Since the molar ratio is 1:1, the number of moles of the unknown acid used is also 0.0015 mol.

Step 5: Calculate the mass of the unknown acid used.
To find the mass of the unknown acid, we can use the formula:
mass (g) = moles × molar mass (g/mol)
mass (g) = 0.0015 mol × 400 g/mol
mass (g) = 0.6 g

Therefore, approximately 0.6 grams of the unknown acid was used for the titration.

To calculate the amount of the unknown acid used for titration, we need to use the concept of molarity and the balanced chemical equation of the reaction.

First, let's understand the balanced chemical equation for the reaction between the base and acid. Let's assume the acid is denoted as HA and the base as BOH. The balanced chemical equation for the reaction is:

HA + BOH -> BA + H2O

Where HA is the unknown acid, BOH is the base, BA is the salt formed, and H2O is water.

The stoichiometry of the reaction indicates that one mole of HA reacts with one mole of BOH to form one mole of BA.

Given that the base concentration (BOH) is 0.05 M and the volume of base (titrant) used is 30 mL, we need to calculate the moles of base used in the reaction:

moles of base (BOH) = molarity x volume in liters
= 0.05 mol/L x 30 mL / 1000 mL/L
= 0.0015 mol

According to the stoichiometry of the reaction, the moles of unknown acid (HA) are equal to the moles of base (BOH) used. Therefore, we have:

moles of unknown acid (HA) = 0.0015 mol

Now, to calculate the amount of unknown acid in grams, we can use the molar mass of the unknown acid (around 400 g/mol):

grams of unknown acid (HA) = moles of unknown acid x molar mass
= 0.0015 mol x 400 g/mol
= 0.6 grams

Therefore, approximately 0.6 grams of the unknown acid would be used for the titration.

millimoles base 0.05M x 30 mL = about 1.5 = 0.0015 mols.

mols acid = 0.0015.
mol = grams acid/molar mass acid. You know molar mass and mol; solve for grams.