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how many grams of zinc chloride are needed to make 4.0 molar solution with a total volume of 1.0 l​

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Answer: Approximately 545.12 grams of zinc chloride

Explanation: To determine the mass of zinc chloride needed to make a 4.0 Molar solution with a total volume of 1.0 L, we need to use the formula:

Molarity (M) = Moles of solute / Volume of solution (in liters)

Rearranging the formula, we can solve for the moles of solute:

Moles of solute = Molarity × Volume of solution

Given:

Molarity (M) = 4.0 M

Volume of solution = 1.0 L

Moles of solute = 4.0 M × 1.0 L = 4.0 moles

Now, to find the mass of zinc chloride, we need to know its molar mass. The molar mass of zinc chloride (ZnCl2) can be calculated as follows:

Molar mass of ZnCl2 = (Atomic mass of zinc) + 2 × (Atomic mass of chlorine)

Molar mass of ZnCl2 = (65.38 g/mol) + 2 × (35.45 g/mol)

Molar mass of ZnCl2 ≈ 136.28 g/mol

Finally, we can calculate the mass of zinc chloride needed using the equation:

Mass of zinc chloride = Moles of solute × Molar mass of zinc chloride

Mass of zinc chloride = 4.0 moles × 136.28 g/mol ≈ 545.12 g

Approximately 545.12 grams of zinc chloride

User Krulik
by
8.6k points
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Answer:

You need 546.2 grams of zinc chloride to make a 4.0 molar solution with a total volume of 1.0 liters.

1 mole of ZnCl2 = 136.3 grams

4.0 moles of ZnCl2 = 136.3 x 4.0 = 546.2 grams

User Michael Shum
by
8.2k points

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