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Leya [2.2K]
3 years ago
5

Calculate the molar solubility of CaF2 at 25°C in a solution that is 0.010 M in Ca(NO3)2. The Ksp for CaF2 is 3.9 x 10-11.

Chemistry
1 answer:
madreJ [45]3 years ago
4 0

Answer:

Molar \ solubility=3.12x10^{-5}M

Explanation:

Hello,

In this case, for the dissociation of calcium fluoride:

CaF_2(s)\rightleftharpoons Ca^{2+}+2F^-

The equilibrium expression is:

Ksp=[Ca^{2+}][F^-]^2

In such a way, via the ICE procedure, including an initial concentration of calcium of 0.01 M (due to the calcium nitrate solution), the reaction extent x is computed as follows:

3.9x10^{-11}=(0.01+x)(2*x)^2\\\\x=0.0000312M

Thus, the molar solubility equals the reaction extent x, therefore:

Molar \ solubility=3.12x10^{-5}M

Regards.

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lidiya [134]

Mass of water vapor produced : 0.90 g

<h3>Further explanation</h3>

Given

0.10 g of hydrogen reacted with 0.80 g of oxygen

Required

mass of water vapor produced

Solution

Reaction

2H₂ + O ⇒ 2H₂O

If we refer to the law of conservation of mass which states that the mass before and after the reaction is the same, then the mass of water vapor formed as a product is:

mass reactants = mass products

mass of Hydrogen + mass of Oxygen = mass of water vapor

0.1 g + 0.8 g = 0.90 g

Or we can also solve<em> by using stochiometry</em> (using the concept of moles) to find the mass of water vapor

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2 years ago
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The volume of a sample of a gas at 273 c is 200.0 l. if the volume is decreased to 100.0 l at constant pressure, what will be th
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Alenkasestr [34]

<u>Answer:</u> The sample of Cobalt-60 isotope must be replaced in January 2027

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Rate law expression for first order kinetics is given by the equation:

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Putting values in above equation, we get:

0.132=\frac{2.303}{t}\log\frac{100}{25}\\\\t=10.5yrs

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