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nataly862011 [7]

3 years ago

9

What is an isotope? How does one isotope differ from another isotope

2 answers:

vova2212 [387]3 years ago

8 0

Isotopes are different versions of a specific element.

Every atom/element is defined by its protons. So if it has 1 proton it's hydrogen no matter what, if it has 2 protons it's helium no matter what and so on. If you know the number of protons, you know the element.

You can change the number of neutrons in the nucleus and you'll get isotopes. Atoms that have different numbers of neutrons are isotopes of each other. It's important to understand that the element is the same but one is going to be a little bit heavier or lighter than another.

Shtirlitz [24]3 years ago

5 0

An isotope is an atom with a unique number of neutrons. Isotopes can differ from each other because of their number of neutrons.

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I need A through D, I have no idea on what I'm supposed to do

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The density of an aqueous solution of nitric acid is 1.64 g/mL and the concentration is 1.85 M. What is the concentration of thi

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Answer:

Mass % of the solution = 7.1067 %

Explanation:

Given :

Molarity of nitric acid solution = 1.85 M

Density of the solution = 1.64 g/mL

<u>Molarity of a solution is defined as the number of moles of solute present in 1 liter of the solution.</u>

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

Lets, consider the volume of the solution = 1 L

Thus,

Moles of nitric acid present in the solution:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Moles of Nitric acid=Molarity \times {Volume\ of\ the\ solution}$

So,

Moles of Nitric acid = 1.85 moles

Molar mass of nitric acid = 63 g/mol

The mass of Nitric acid can be find out by using mole formula as:

$moles=\frac{Mass\ taken}{Molar\ mass}$

Thus,

$Mass\ of\ Nitric\ acid=Moles \times Molar mass}$

$Mass\ of\ Nitric\ acid=1.85 g \times 63 g/mol}$

<u>Mass of Nitric acid = 116.55 g</u>

Also,

$Density=\frac{Mass}{Volume}$

Given : Density = 1.64 g/mL

Also, 1 L = 10³ mL

Volume of the solution is 1000 mL

So, mass of the solution:

$Mass\ of\ the\ solution=Density \times {Volume\ of\ the\ solution}$

$Mass\ of\ the\ solution=1.64 g/mL \times {1000 mL}$

<u>Mass of the solution = 1640 g</u>

Mass % is defined as the mass of solute in 100 g of the solution. The formula for the calculation of mass % is shown below:

$Mass \% =\frac{Mass\ of\ the\ solute}{Mass\ of\ the\ solution} \times {100}$

So,

$Mass \%=\frac{116.55}{1640} \times {100}$

<u>Mass % = 7.1067 %</u>

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