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bixtya [17]
4 years ago
7

What would be the saturation concentration (mole/L) of oxygen (O2) in a river in winter when the air temperature is 0°C if the H

enry's law constant at this temperature is 2.28 × 10-3 mole/L-atm? What would the answer be in units of mg/L?
Chemistry
1 answer:
kolbaska11 [484]4 years ago
7 0

20.21*10^-4 mg/L is the concentration.

Explanation:

Given:  

Pressure=1 atm.

Temperature=  0 degrees

Volume percent of air is 21%

Henry's Law constant K = 2.28 x 10^-3 mole/L-atm

The partial pressure of oxygen is 0.21 atm.

By Henry's law:

Concentration= K X Partial pressure

                        =  2.28*10^-3 *0.21

                          =  4.79*10^-4 moles/litre

Since, at STP 1 mole of oxygen occupies volume of 22.4L

concentration =mass/volume

     mass                  =  4.79*10^-4-4*22.4

                                 = 20.21*10^-4 mg

    20.21*10^-4 mg/L is the concentration.

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Explanation:

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8 0
3 years ago
What mass of potassium bromide (in grams) do you need to make 250.0 mL of a 1.50 M potassium bromide solution?
Vedmedyk [2.9K]

Answer:

44.63g

Explanation:

First, let us calculate the number of mole of KBr in 1.50M KBr solution.

This is illustrated below:

Data obtained from the question include:

Volume of solution = 250mL = 250/1000 = 0.25L

Molarity of solution = 1.50M

Mole of solute (KBr) =.?

Molarity is simply mole of solute per unit litre of solution

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Mole = Molarity x Volume

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Mass of KBr =?

Mass = number of mole x molar Mass

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Mass of KBr = 44.63g

Therefore, 44.63g of KBr is needed to make 250.0mL of 1.50 M potassium bromide (KBr) solution

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