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pogonyaev
3 years ago
14

EXAMPLES OF PURE SUBSTANCES

Chemistry
1 answer:
ser-zykov [4K]3 years ago
3 0

Answer: Water, tin, sulfur, sucrose, salt, and etc.

Explanation: The photo has more examples

You might be interested in
1. Water vapor has_________ energy because it is a __________.
natulia [17]
Water vapor has more energy because it is a gas :)
4 0
3 years ago
A chemist must dilute 97.1 ml of aqueous magnesium fluoride solution until the concentration falls to 389 microMolarity . He'll
mojhsa [17]

Answer:

0.302L

Explanation:

<em>...97.1mL of 1.21m M aqueous magnesium fluoride solution</em>

<em />

In this problem the chemist is disolving a solution from 1.21mM = 1.21x10⁻³M, to 389μM = 389x10⁻⁶M. That means the solution must be diluted:

1.21x10⁻³M / 389x10⁻⁶M = 3.11 times

As the initial volume of the original concentration is 97.1mL, the final volume must be:

97.1mL * 3.11 = 302.0mL =

0.302L

6 0
3 years ago
What is the mass of 0. 513 mol Al2O3? Give your answer to the correct number of significant figures. (Molar mass of Al2O3 = 102.
Margarita [4]

The mass of a 0.513 mol of Al2O3 is 52.33g.

HOW TO CALCULATE MASS:

The mass of a substance can be calculated by multiplying the molar mass of the substance by its number of moles. That is;

mass of Al2O3 = no. of moles of Al2O3 × molar mass of Al2O3

According to this question, there are 0.513 moles of Al2O3.

Mass of Al2O3 = 0.513 × 102

Mass of Al2O3 = 52.33g

Therefore, the mass of a 0.513 mol of Al2O3 is 52.33g.

Learn more about mass calculations at: brainly.com/question/8101390?referrer=searchResults

7 0
2 years ago
Brass is a solid solution composed of zinc and copper. Brass is classified as a (n): A.colloid B.suspension C.solution D.alloy
melamori03 [73]
Brass is an alloy, or a combination of two (or more) metals.
4 0
3 years ago
If 0.2 g of nitrobenzene are added to 10.9 g of naphthalene, calculate the molality of the solution. (given: molar mass of nitro
In-s [12.5K]

Molality is defined as 1 mole of a solute in 1 kg of solvent.  

Molality=

\frac{Number of moles of solute}{Mass of solvent in kg}

Number of moles of solute, n=  

\frac{Given mass of the substance}{Molar mass of the substance}

Given mass of the nitrobenzene=0.2 g

Molar mass of the substance= 123.06 g mol⁻¹

Number of moles of nitrobenzene,  

n= \frac{0.2 }{123.06}

Number of moles of nitrobenzene, n= 0.0016  mol

Mass of 10.9 g of naphthalene in kg=0.0109  

Molality= \frac{0.0016}{0.0109 }

Molality= 0.146 m

7 0
3 years ago
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