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never [62]
2 years ago
11

What is the molarity of a solution prepared by dissolving 198 g of BaBr2 in 2.00 liters of solution?

Chemistry
1 answer:
Vikki [24]2 years ago
8 0

Answer:

The molarity of the solution is 0.335 \frac{moles}{liter}

Explanation:

Molar concentration is a measure of the concentration of a solute in a solution, be it some molecular, ionic, or atomic species.

Molarity is the number of moles of solute that are dissolved in a certain volume and is calculated by:

Molarity=\frac{number of moles of solute}{volume}

Molarity is expressed in units \frac{moles}{liter}.

Being the molar mass of BaBr2 equal to 297.14 g/mole, that is to say that 1 mole contains 297.14 grams, the mass of 198 grams are contained in:

198 grams*\frac{1 mole}{297.14 grams} = 0.67 moles

So:

  • number of moles of solute= 0.67 moles
  • volume= 2 L

Replacing in the definition of molarity:

Molarity=\frac{0.67 moles}{2 L}

Solving:  

Molarity= 0.335 \frac{moles}{liter}

<u><em>The molarity of the solution is 0.335 </em></u>\frac{moles}{liter}<u><em></em></u>

<u><em></em></u>

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Calculate the volume of 4.50 mol of SO2 (g) measured at STP. At STP: P = 101.3 kPa, T = 273.15 K A. 87.3 L B. 101 L C. 127 L D.
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Answer:

B

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Explanation:

We use the ideal gas relation

PV = nRT

P = pressure = 101.3KPa

V = volume = ?

n = number of moles = 4.5moles

T = Temperature = 273.15K

R = molar gas constant = 8.314J/mol.k

Rearranging the equation to make V the subject of the formula yields :

V = nRT/P

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8 0
3 years ago
If a lab requires each a lab group (3 students) to have 25 ml of a solution and it takes 15 grams of AgNO₃ cuprous nitrate, to m
pochemuha

Answer:

0.375 grams are needed to make 25 mL solution.

Explanation:

Mass of AgNO_3 cuprous nitrate required to make 1 l of solution = 15 g.

1 L = 1000 mL

Mass of AgNO_3 cuprous nitrate required to make 1000 mL of solution = 15 g

Mass of AgNO_3 cuprous nitrate required to make 1 mL of solution:

=\frac{15}{1000} g

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0.375 grams are needed to make 25 mL solution.

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3 years ago
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