Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 5.4 g of iron are to be dissolved in 1.1 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?

To find the minimum volume of the HCl solution required to react with all of the iron, we need to determine the number of moles of iron present and then use the stoichiometry of the reaction to find the amount of HCl solution needed.

First, let's calculate the number of moles of iron in 5.4 g of iron. We can use the molar mass of iron (Fe) to convert from grams to moles. The molar mass of iron is 55.85 g/mol.

Number of moles of iron = mass of iron / molar mass of iron
= 5.4 g / 55.85 g/mol
= 0.0965 mol (rounded to four decimal places)

According to the balanced chemical equation, 1 mole of iron reacts with 2 moles of HCl to produce 1 mole of H2 gas and 1 mole of Fe2+ ions.

Therefore, the number of moles of HCl required to react with 0.0965 mol of iron is twice that amount, or 2 * 0.0965 mol = 0.193 mol.

Now, we can use the definition of molarity to find the volume of 1.1 M HCl solution needed:

Molarity (M) = moles / volume (in liters)

Rearranging the equation, we get:

Volume (in liters) = moles / Molarity

Volume (in liters) = 0.193 mol / 1.1 M
= 0.1755 L (rounded to four decimal places)

Finally, we need to convert the volume from liters to milliliters. There are 1000 milliliters (mL) in 1 liter.

Volume (in mL) = volume (in liters) * 1000
= 0.1755 L * 1000
= 175.5 mL

Therefore, the minimum volume of the HCl solution required to react with all of the iron is 175.5 mL.