Density Problems Worksheet for 9th - 12th Grade | Lesson Planet - Free Printable

You're right — the image you uploaded is a Chemistry: Density Problems worksheet. Since I can’t see or process images directly, I’ll solve all 6 problems based on the text you’ve provided (which appears to be a clear transcription of the worksheet). I’ll walk through each problem step-by-step with explanations.

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🧪 Problem 1:

> The density of ethanol is 0.789 g/mL. What is the mass of 200.0 mL of ethanol?

Formula:
Density = Mass / Volume → Mass = Density × Volume

Plug in values:
Mass = 0.789 g/mL × 200.0 mL
Mass = 157.8 g

✔ Answer: 157.8 g

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🧪 Problem 2:

> A 23.74 g sample of a substance occupies a volume of 2.00 cm³. Find its density in g/cm³.

Formula:
Density = Mass / Volume

Plug in values:
Density = 23.74 g / 2.00 cm³
Density = 11.87 g/cm³

✔ Answer: 11.87 g/cm³

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🧪 Problem 3:

> Some common substances, except gas (it has a density of 0.000186 g/mL), have the volume occupied by 500.0 g is 400.0 mL. Find their density.

Wait — this wording is a bit ambiguous. Let’s interpret:

It says “except gas (density = 0.000186 g/mL)” — so we’re not talking about gas here. Then it says “have the volume occupied by 500.0 g is 400.0 mL”.

So:
Mass = 500.0 g
Volume = 400.0 mL

Formula:
Density = Mass / Volume

Density = 500.0 g / 400.0 mL = 1.25 g/mL

✔ Answer: 1.25 g/mL

*(Note: The gas part is likely just extra info to distract or clarify that we’re dealing with non-gas substances.)*

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🧪 Problem 4:

> Find the volume that 352.0 g of carbon tetrachloride (CCl₄) will occupy if it has a density of 1.59 g/mL.

Formula:
Density = Mass / Volume → Volume = Mass / Density

Volume = 352.0 g / 1.59 g/mL ≈ 221.38 mL

✔ Answer: 221.4 mL (rounded to one decimal place as per typical significant figures)

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🧪 Problem 5:

> The density of ethanol is 0.789 g/mL. If you have 250.0 mL of ethanol, what is the mass?

This is similar to Problem 1.

Mass = Density × Volume
Mass = 0.789 g/mL × 250.0 mL = 197.25 g

✔ Answer: 197.3 g (rounded to one decimal place)

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🧪 Problem 6:

> Which of the following liquids are miscible? If the volume of each liquid measured is 100.0 mL, which would have the greatest mass?

A. Methanol (CH₃OH), density = 0.791 g/mL
B. Sulfuric acid (H₂SO₄), density = 1.830 g/mL
C. Water (H₂O), density = 1.000 g/mL
D. Mercury (Hg), density = 13.55 g/mL

*(Note: Mercury is a liquid metal, so it counts here.)*

#### Part 1: Which are miscible?
“Miscible” means they mix completely in all proportions.

- Methanol and water → ✔ Miscible (both polar, hydrogen bonding)
- Sulfuric acid and water → ✔ Miscible (highly soluble, forms hydrates)
- Mercury → ✘ Immiscible with water, methanol, sulfuric acid (metallic, non-polar)
- Methanol and sulfuric acid → ✔ Generally miscible (though may react)

But since the question says “which of the following liquids are miscible?” without specifying pairs, and mercury is clearly immiscible with the others, we can say:

✔ Methanol, Sulfuric Acid, and Water are miscible with each other. Mercury is not miscible with them.

#### Part 2: Which has the greatest mass for 100.0 mL?

Mass = Density × Volume → Since volume is same (100.0 mL), the one with highest density has greatest mass.

Densities:
- Methanol: 0.791 g/mL → Mass = 79.1 g
- Sulfuric acid: 1.830 g/mL → Mass = 183.0 g
- Water: 1.000 g/mL → Mass = 100.0 g
- Mercury: 13.55 g/mL → Mass = 1355 g

✔ Answer: Mercury has the greatest mass (1355 g)

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## ✔ Final Answers Summary:

1. 157.8 g
2. 11.87 g/cm³
3. 1.25 g/mL
4. 221.4 mL
5. 197.3 g
6.
- Miscible: Methanol, Sulfuric Acid, Water (Mercury is immiscible)
- Greatest mass: Mercury (1355 g)

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