How many milliliters of a 0.66 M HCl solution

are needed to react completely with 1.9 g of
zinc to form zinc(II) chloride?

WISH I NKEW....I HATE MAROON

Yep

To determine the number of milliliters (mL) of a solution needed to react completely with a given mass of a substance, we need to use the concept of molarity and the stoichiometry of the chemical equation.

First, let's write the balanced chemical equation for the reaction between HCl and zinc (Zn):

Zn + 2HCl → ZnCl2 + H2

From the balanced equation, we can see that 1 mole of zinc reacts with 2 moles of HCl to form 1 mole of zinc chloride (ZnCl2). Now, let's calculate the moles of zinc in 1.9 g:

The molar mass of zinc (Zn) is 65.38 g/mol.
Moles of Zn = Mass of Zn / Molar mass of Zn
Moles of Zn = 1.9 g / 65.38 g/mol

Next, let's use the stoichiometry of the balanced equation to determine the moles of HCl required to react with the calculated moles of zinc:

Moles of HCl = Moles of Zn x (2 moles of HCl / 1 mole of Zn)

Now, we can calculate the volume (in liters) of the HCl solution using the molarity (0.66 M) and the moles of HCl:

Volume (in liters) = Moles of HCl / Molarity

Finally, we convert the volume from liters to milliliters by multiplying by 1000:

Volume (in milliliters) = Volume (in liters) x 1000

By following these steps and plugging in the values, you can calculate the number of milliliters of the 0.66 M HCl solution needed to react completely with 1.9 g of zinc to form zinc(II) chloride.