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Paul [167]
3 years ago
8

A detailed explanation, one paragraph of the colligative property being discussed and why that property changes the way that it

does when the amount of solute is increased.
A detailed description, at least one paragraph, of a real-world application of the colligative property, including an explanation of how this application of the colligative property is important or useful to those affected. The real-world example must be one that was not mentioned in the lesson.
Chemistry
1 answer:
levacccp [35]3 years ago
6 0
<span>
You can do it on the icing of roads, reverse osmosis for desalination of water, dissolved CO2 in soda cans, osmotic pressure involving blood vessels and IV solutions, etc.</span>
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Answer:skin cream

Explanation:

the independent variable is the variable that is always changed or manipulated. in this case the skin cream is the independent variable.

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Why are zeppelin filled with hydrogen a bad idea?
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the fire that destroyed due to the extremely flammable aluminium /iron oxide  based  applied to the outer skin of the craft. This was struck by lightning and caught fire well before the hydrogen ignited.

Explanation:

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Complete the following statements about the functions of the digestive system. The starts an involuntary swallowing action when
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pharynx esophagus peristalsis chyme

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3 years ago
An analytical chemist is titrating of a solution of ethylamine with a solution of . The of ethylamine is . Calculate the pH of t
Elenna [48]

Answer:

pH=11.

Explanation:

Hello!

In this case, since the data is not given, it is possible to use a similar problem like:

"An analytical chemist is titrating 185.0 mL of a 0.7500 M solution of ethylamine(C2HNH2) with a 0.4800 M solution of HNO3.ThepK,of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 114.4 mL of the HNO3 solution to it"

Thus, for the reaction:

C_2H_5NH_2+H^+\rightleftharpoons C_2H_5NH_4^+

Tt is possible to compute the remaining moles of ethylamine via the following subtraction:

n_{ethylamine}=0.1850L*0.7500mol/L=0.1365mol\\\\n_{acid}=0.1144L*0.4800mol/L=0.0549mol\\\\n_{ethylamine}^{remaining}=0.1365mol-0.0549mol=0.0816mol

Thus, the concentration of ethylamine in solution is:

[ethylamine]=\frac{0.0816mol}{0.1850L+0.1144L}=0.2725M

Now, we can also infer that some salt is formed, and has the following concentration:

[salt]=\frac{0.0549mol}{0.1850L+0.1144L}=0.1834M

Therefore, we can use the Henderson-Hasselbach equation to compute the resulting pOH first:

pOH=pKb+log(\frac{[salt]}{[base]} )\\\\pOH=3.19+log(\frac{0.1834M}{0.2725M})\\\\pOH=3.0

Finally, the pH turns out to be:

pH=14-pOH=14-3\\\\pH=11

NOTE: keep in mind that if you have different values, you can just change them and follow the very same process here.

Best regards!

4 0
3 years ago
Which two conditions can limit the usefulness of the kinetic-molecular theory in describing gas behavior?
love history [14]

Answer:

low pressure and medium temperature

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3 years ago
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