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sergejj [24]
3 years ago
10

0.200 grams of HCl is dissolved in 0.801 grams water. The density of the solution formed is 1.10 g/mL. What is the molarity of t

he solution
Chemistry
1 answer:
alina1380 [7]3 years ago
6 0

Answer:

M=6.03M

Explanation:

Hello,

In this case, since the molarity is computed by:

M=\frac{n_{solute}}{V_{solution}}

Whereas the solute is the hydrochloric acid, we compute the corresponding moles with its molar mass (36.45 g/mol):

n_{solute}=0.200gHCl*\frac{1molHCl}{36.45gHCl} =0.00549molHCl

Next, since the solution contains both HCl and water, we compute the volume in liters by using its density:

V_{solution}=(0.200+0.801)g*\frac{1mL}{1.10g} *\frac{1L}{1000mL} =9.1x10^{-4}L

Therefore, the molarity turns out:

M=\frac{0.00549mol}{9.1x10^{-4}L}\\ \\M=6.03M

Regards.

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An aqueous potassium carbonate solution is made by dissolving 5.51 moles of K 2 CO 3 in sufficient water so that the final volum
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Answer:

1.67mol/L

Explanation:

Data obtained from the question include:

Mole of solute (K2CO3) = 5.51 moles

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Molarity is simply the mole of solute per unit litre of the solution. It can be expressed mathematically as:

Molarity = mole of solute /Volume of solution

Molarity = 5.51 mol/3.30 L

Molarity = 1.67mol/L

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In general, ionic compounds are hard solids at ambient temperatures but they shatter fairly easily. How do these two properties
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Electrovalent compounds posses:

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This is the transfer of valence electrons from metals to non metals to form ionic compounds. It also refers to a chemical bond formed between two ions with opposite charges.

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7 0
2 years ago
Calculate the mass of each element in the
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Answer:

For Mass N, Mass H, and Mass O, the mass is 28.0 g N, 4.0 g H, and 48.0 g respectively

Explanation:

The computation of the mass of each element is given below:

As we know that

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Now we multiply each of above  by the molar masses

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= 1.0 g/mol × 4

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3 years ago
How many moles of aluminum oxide would form if 12.5 moles of aluminum burned​
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<h3>Al + O2 -> Al2O3</h3>

Balance it:

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So you need 2 Al and 3 O2 to make 2 Al2O3 (aluminum oxide).

I'm going to assume you have all the O2 you need.

Since 2 mols of Al is needed to make 2 mols of the product, it's a 1:1 ratio. You get as much aluminum oxide for as much aluminum you burn.

So 12.5 mols if there is not a lack of the O2.

7 0
3 years ago
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