how many liters of 0.100 M HCL would be required to react completely with 5.00 grams of calcium hydroxide?

1.35

To determine the number of liters of 0.100 M HCl required to react completely with 5.00 grams of calcium hydroxide, you need to follow these steps:

Step 1: Write the balanced chemical equation for the reaction.

Ca(OH)2 + 2HCl -> CaCl2 + 2H2O

Step 2: Calculate the molar mass of Ca(OH)2.

Ca: 40.08 g/mol
O: 16.00 g/mol (2 atoms)
H: 1.01 g/mol (2 atoms)

Molar mass of Ca(OH)2 = 40.08 + (16.00 * 2) + (1.01 * 2) = 74.09 g/mol

Step 3: Calculate the number of moles of Ca(OH)2.

Number of moles = mass / molar mass
Number of moles = 5.00 g / 74.09 g/mol

Step 4: Convert moles of Ca(OH)2 to moles of HCl using the stoichiometry of the balanced equation.

From the balanced equation, we see that 1 mole of Ca(OH)2 reacts with 2 moles of HCl.

Number of moles HCl = (number of moles Ca(OH)2) * 2

Step 5: Calculate the volume of 0.100 M HCl required using the molarity equation.

Molarity (M) = moles / volume (L)

Number of moles HCl = (0.100 M) * (volume HCl in liters)

Rearranging the equation:

volume HCl in liters = (number of moles HCl) / (0.100 M)

Step 6: Calculate the volume of HCl.

volume HCl in liters = (number of moles HCl) / (0.100 M)

Now, let's calculate the values.

Number of moles Ca(OH)2 = 5.00 g / 74.09 g/mol = 0.067 moles Ca(OH)2

Number of moles HCl = 0.067 moles Ca(OH)2 * 2 = 0.134 moles HCl

Volume HCl in liters = (0.134 moles HCl) / (0.100 M) = 1.34 liters

Therefore, you would need 1.34 liters of 0.100 M HCl to react completely with 5.00 grams of calcium hydroxide.

To determine the quantity of 0.100 M HCL (hydrochloric acid) needed to react completely with 5.00 grams of calcium hydroxide (Ca(OH)2), you need to use stoichiometry and the balanced chemical equation.

Step 1: Write the balanced chemical equation for the reaction between HCL and Ca(OH)2:
2HCl + Ca(OH)2 → CaCl2 + 2H2O

Step 2: Determine the molar mass of Ca(OH)2:
Ca: 1 atom x 40.08 g/mol = 40.08 g/mol
O: 2 atoms x 16.00 g/mol = 32.00 g/mol
H: 2 atoms x 1.01 g/mol = 2.02 g/mol

Total molar mass of Ca(OH)2: 40.08 + 32.00 + 2.02 + 2.02 = 76.12 g/mol

Step 3: Convert the given mass of Ca(OH)2 to moles:
5.00 g / 76.12 g/mol = 0.0656 mol Ca(OH)2

Step 4: Using the balanced chemical equation, determine the mole ratio between HCl and Ca(OH)2:
From the balanced equation, 2 moles of HCl react with 1 mole of Ca(OH)2.

So, 0.0656 mol Ca(OH)2 * (2 mol HCl / 1 mol Ca(OH)2) = 0.1312 mol HCl

Step 5: Finally, calculate the volume of 0.100 M HCl solution required to react completely with the calculated moles of HCl:
Volume (L) = Moles / Molarity
Volume (L) = 0.1312 mol / 0.100 mol/L
Volume (L) = 1.312 L or 1312 mL

Therefore, you would require 1.312 liters (or 1312 mL) of 0.100 M HCl to react completely with 5.00 grams of calcium hydroxide.

Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O

mols Ca(OH)2 = grams/molar mass = ??
mols HCl needed = mols Ca(OH)2 x (2 mols HCl/1 mol Ca(OH)2) = mols Ca(OH)2 x (2/1) = xx mols HCl
Molarity HCl = mols/L.
You know molarity and mols. Solve for Liters HCl. Check my