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notka56 [123]
3 years ago
9

Water is denser than oil. When frozen, the oil sinks to the bottom. Why?

Chemistry
1 answer:
sammy [17]3 years ago
6 0

Answer: When water freezes it gets larger and becomes a solid but it still weighs the same as when it was a liquid form. When it becomes larger it takes up space but makes it less dense. Ok so getting to the point- oil unlike water becomes more dense when frozen so this is why oil sinks in water. Sorry if this was confusing but I hope it helped have a great day and god bless you :3

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list the 7 continents and circle the only one that doesn't have any. glacier on it? the areas convered with glacier sill be. whi
diamong [38]

Africa.

Europe.

Asia.

North America.

South America.

Australia (or Oceania)  THE ONLY CONTINENT WITHOUT GLACIERS!!

Antarctica.

7 0
3 years ago
Express the concentration of a 0.0390 M aqueous solution of fluoride, F − , in mass percentage and in parts per million (ppm). A
Vadim26 [7]

Answer:

Mass percentage → 0.074 %

[F⁻] = 741 ppm

Explanation:

Aqueous solution of flouride → [F⁻] = 0.0390 M

It means that in 1L of solution, we have 0.0390 moles of F⁻

We need the mass of solution and the mass of 0.0390 moles of F⁻

Mass of solution can be determined by density:

1g/mL = Mass of solution / 1000 mL

Note: 1L = 1000mL

Mass of solution: 1000 g

Moles of F⁻ → 0.0390 moles . 19g /1 mol = 0.741 g

Mass percentage → (Mass of solute / Mass of solution) . 100

(0.741 g / 1000 g) . 100 = 0.074 %

Ppm = mass of solute . 10⁶ / mass of solution (mg/kg)

0.741 g . 1000 mg/1g = 741 mg

1000 g . 1 kg/1000 g = 1kg

741 mg/1kg = 741 ppm

5 0
3 years ago
what is the pH of a solution that results when 0.010mol HNO3 is added to 500.ml of a solution that is 0.10M in aqueous ammonia a
WARRIOR [948]

Answer : The  

pH of a solution is, 8.56

Explanation : Given,

K_b=1.8\times 10^{-5}

Concentration of ammonia (base) = 0.10 M

Concentration of ammonium nitrate (salt) = 0.55 M

First we have to calculate the value of pK_b.

The expression used for the calculation of pK_b is,

pK_b=-\log (K_b)

Now put the value of K_b in this expression, we get:

pK_b=-\log (1.8\times 10^{-5})

pK_b=5-\log (1.8)

pK_b=4.7

Now we have to calculate the pOH of buffer.

Using Henderson Hesselbach equation :

pOH=pK_b+\log \frac{[Salt]}{[Base]}

Now put all the given values in this expression, we get:

pOH=4.7+\log (\frac{0.55}{0.10})

pOH=5.44

The pOH of buffer is 5.44

Now we have to calculate the pH of a solution.

pH+pOH=14\\\\pH+5.44=14\\\\pH=14-5.44\\\\pH=8.56

Thus, the pH of a solution is, 8.56

8 0
3 years ago
How many moles of carbon dioxide are formed after reacting completely with 20. moles of calcium carbonate?
adoni [48]

Answer:

20. mol

Explanation:

i got it right on my quiz

3 0
3 years ago
HELP PLS THIS IS DUE IN 15 MINUTES PLS PLS PLS!!! I WILL MARK BRAINLIEST IWTH THE BEST ANSWER!!!
jarptica [38.1K]

Answer:

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Explanation:

7 0
2 years ago
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