Question

If 1.08 g of an acid is required for 37.18 ml of NaOH solution for titration, what is the appropriate concentration?

a) 0.029 g/ml
b) 0.041 g/ml
c) 0.052 g/ml
d) 0.029 ml/g

Answer 1

To find the appropriate concentration of the acid used in the titration, we need to calculate the number of moles of the acid. However, without knowing the molar mass of the acid, we cannot determine the concentration accurately.

Step-by-step explanation:

To find the appropriate concentration of the acid, we need to calculate the number of moles of the acid used in the titration. First, we convert the volume of the NaOH solution from milliliters (mL) to liters (L): 37.18 mL = 0.03718 L. Next, we calculate the number of moles of the acid:

moles = mass / molar mass

Assuming the acid is monoprotic (forms 1 mole of H+ ions), we can use the relationship between moles of acid and moles of NaOH to determine the concentration of the acid:

concentration = moles of acid / volume of NaOH solution (in liters)

Plugging in the values, we have:

concentration = (1.08 g / molar mass of acid) / 0.03718 L

Since we don't know the molar mass of the acid, we can't calculate the concentration of the acid accurately. Therefore, none of the given answer choices (a, b, c, d) can be determined without more information.