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loris [4]
3 years ago
14

If 6.5 L of water is added to 4.5 L of a 2.8 M Ca(OH)2 solution, what is the molarity of the new solution?

Chemistry
1 answer:
Mila [183]3 years ago
6 0
Find moles of Ca(OH)2 first:

moles = 2.8 x 4.5 = 12.6

Now,
   After addition, new volume =  6.5 + 4.5 = 11.0

So, new molarity =  12.6 / 11 = 1.145
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Helpppp pleaseee ill give brainliest
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Answer:

The answers are in the explanation.

Explanation:

The energy required to convert 10g of ice at -10°C to water vapor at 120°C is obtained per stages as follows:

Increasing temperature of ice from -10°C - 0°C:

Q = S*ΔT*m

Q is energy, S specific heat of ice = 2.06J/g°C, ΔT is change in temperature = 0°C - -10°C = 10°C and m is mass of ice = 10g

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Q = 206J

Change from solid to liquid:

The heat of fusion of water is 333.55J/g. That means 1g of ice requires 333.55J to be converted in liquid. 10g requires:

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Increasing temperature of liquid water from 0°C - 100°C:

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The heat of vaporization of water is 2260J/g. That means 1g of liquid water requires 2260J to be converted in gas. 10g requires:

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Increasing temperature of gas water from 100°C - 120°C:

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Q is energy, S specific heat of gaseous water = 1.87J/g°C, ΔT is change in temperature = 20°C and m is mass of water = 10g

Q = 1.87J/g°C*20°C*10g

Q = 374J

Total Energy:

206J + 3335.5 J + 4180J + 22600J + 374J =

30695.5J =

30.7kJ

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