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Margarita [4]
3 years ago
11

You can purchase hydrochloric acid in a concentrated form that is 37.0% HCl by mass and that has a density of 1.20 g/mL. Describ

e exactly how to prepare 2.85 L of 0.500 M HCl from the concentrated solution.
Chemistry
1 answer:
Snowcat [4.5K]3 years ago
3 0

Answer:

We take 117mL of the 37.0% by mass solution of HCl, and we complete with water to a final volume of 2.85L

Explanation:

First of all, we calculate the molarity of concentrated solution.

37% by mass means that 37 g of solute are contained in 100 g of solution.

So density which apply for solution, help us to determine the volume of solution.

Solution density = Solution mass / Solution volume

1.20 g/mL = 100 g / Solution volume → 100 g / 1.20 g/mL = 83.3mL

Then 37 g of HCl are contained in 83.3 mL. Let's calculate the molarity (mol/L)

37 g / 37.45 g/mol = 1.01 mol

83.3 mL . 1 L/1000mL = 0.0833 L

1.01 mol / 0.0833L = 12.2 M

Let's apply the dilution formula

Conc. M . Conc. volume = Diluted M . diluted volume

12.2 M . Concentrated volume = 0.5 M . 2.85L  

Concentrated volume = ( 0.5 M . 2.85L) / 12.2 M → 0.1168 L ≅ 0.117L

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Answer:

Explanation:

Method 1 proportion

1 mole of chromium is 52 grams

11.9 moles = x grams

1/11.9 = 52/x                    Cross multiply

x = 11.9 * 52

x = 618.8                         grams

Now I have used an approximate mass for Chromium. The answer you get here is expected to reflect the weigth given on your periodic table Use that to get your answer. You should give a number very close to mine. Round to 3 places as in 619.

Method Two  Formula

mols = given mass / molecular mass

11.9 = given mass /  51.9961          Multiply both sides by  51.9961

11.9 *51.9961  = given mass            

given mass = 618.75

given mass = 619

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Answer:

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