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uysha [10]
3 years ago
7

What is the molar mass caci2

Chemistry
1 answer:
prohojiy [21]3 years ago
7 0

Answer:

Since the molar mass of Calcium is 40.08 g and the molar mass of Chlorine is 35.45, it would be 40.08g+35.45g+35.45g (with 2 Chlorines according to the subscript.) That leaves you with 110.98 g.

Explanation:

Hope it helps you

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The Henry's law constant (kH) for O2 in water at 20°C is 1.28e-3 mol/l atm. How many grams of O2 will dissolve in 3.5 L of H2O t
Sophie [7]

Answer : The mass of O_2 dissolved will be, 0.2365 grams

Explanation :

First we have to calculate the concentration of O_2.

As we know that,

C_{O_2}=k_H\times p_{O_2}

where,

C_{O_2} = concentration of O_2 = ?

p_{O_2} = partial pressure of O_2 = 1.65 atm

k_H = Henry's law constant = 1.28\times 10^{-3}mole/L.atm

Now put all the given values in the above formula, we get:

C_{O_2}=(1.28\times 10^{-3}mole/L.atm)\times (1.65atm)

C_{O_2}=2.112\times 10^{-3}mole/L

The concentration of O_2 = 2.112\times 10^{-3}mole/L

Now we have to calculate the moles of O_2

\text{Moles of }O_2=\text{Concentration of }O_2\times \text{volume of solution}

\text{Moles of }O_2=(2.112\times 10^{-3}mole/L)\times (3.5L)=7.392\times 10^{-3}mole

Now we have to calculate the mass of O_2

\text{Mass of }O_2=\text{Moles of }O_2\times \text{Molar mass of }O_2

\text{Mass of }O_2=(7.392\times 10^{-3}mole)\times (32g/mole)=0.2365g

Therefore, the mass of O_2 dissolved will be, 0.2365 grams

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<em>∴ V before dilution = (MV) after dilution / M before dilution</em> = (0.15 M)(500.0 mL)/(0.50 M) = <em>150.0 mL.</em>

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