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vlada-n [284]
3 years ago
13

At 25 °c, only 0.0100 mol of the generic salt ab2 is soluble in 1.00 l of water. what is the ksp of the salt at 25 °c? ab2(s)↽−−

⇀a2+(aq)+2b−(aq)
Chemistry
1 answer:
Assoli18 [71]3 years ago
4 0
Where the solubility product Ksp is applied where salts don't fully dissolve in a solvent.

and when the reaction equation is:

AB2(s) ↔ A2+(Aq)  + 2 B-(aq)

so we have the Ksp expression = [A2+][B-]^2

when we assume [A2+] = X = 0.01 M 


and [B-] = 2X = 2*0.01 M = 0.02 M

So by substitution:

Ksp = 0.01 * (0.02)^2

       = 4 x 10^-6
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<u>Answer:</u> The correct answer is Option b.

<u>Explanation:</u>

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We are given:

m=30g\\\Delta T=[40-0]^oC=40^oC\\q=?J

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q=30g\times 4.186J/g^oC\times 40^oC

q = 5023.2 J

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We are given:

m=40g\\\Delta T=[40-30]^oC=10^oC\\q=?J

Putting values in equation 1, we get:

q=40g\times 4.186J/g^oC\times 10^oC

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Hence, the amount of heat gained in Trial 1 about 3347 J more than the heat released in Trial 2.

Thus, the correct answer is Option b.

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