Three samples of an unknown acid are titrated with 0.4901 M NaOH. The average equivalent weight of the acid using the data below is g/equiv

mass of unknown vol NaOH
trial 1: 1.02 27.72
trial 2: .522 14.22
trial 3: .742 20.02

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Three samples of an unknown acid are titrated with 0.4901 M NaOH. The average equivalent weight of the acid using the data below is g/equiv ?

the mass of unknown for trial 1 is 1.02, trial 2 is 0.522, trial 3 is 0.742
volume of NaOH in trial 1 is 27.72, trial 2 is 14.22, and trial 3 is 20.02

To find the average equivalent weight of the unknown acid, we need to calculate the number of equivalents of acid used in each trial.

The number of equivalents (neq) can be calculated using the formula:

neq = (volume of NaOH in mL x molarity of NaOH) / 1000

Let's calculate the number of equivalents for each trial:

Trial 1:
neq1 = (27.72 mL x 0.4901 M) / 1000 = 0.0135698922 neq

Trial 2:
neq2 = (14.22 mL x 0.4901 M) / 1000 = 0.0069701422 neq

Trial 3:
neq3 = (20.02 mL x 0.4901 M) / 1000 = 0.0098039022 neq

Next, we calculate the weight in grams per equivalent:

For Trial 1:
g/equiv1 = mass of unknown / neq1 = 1.02 g / 0.0135698922 neq = 75.1823178 g/equiv

For Trial 2:
g/equiv2 = mass of unknown / neq2 = 0.522 g / 0.0069701422 neq = 74.9103809 g/equiv

For Trial 3:
g/equiv3 = mass of unknown / neq3 = 0.742 g / 0.0098039022 neq = 75.4898418 g/equiv

Now, we calculate the average equivalent weight:

Average g/equiv = (g/equiv1 + g/equiv2 + g/equiv3) / 3
= (75.1823178 g/equiv + 74.9103809 g/equiv + 75.4898418 g/equiv) / 3
= 225.5825405 g/equiv / 3
= 75.1941802 g/equiv

Therefore, the average equivalent weight of the unknown acid is approximately 75.194 g/equiv.