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Aloiza [94]
2 years ago
6

Which statement about London’s desperation forces is true

Chemistry
1 answer:
djyliett [7]2 years ago
8 0
It's the weakest of all the intermolecular forces present in chemistry . the London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

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The most dangerous form of skin cancer which is often caused by over exposure to ultraviolet radiation is what?
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UV exposure that leads to sunburn is proven in developing melanoma, the most dangerous of the three most common types of skin cancer.
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57. The orbitals of an atom are distinguished from each other on the basis of their size, shape, and orientation in
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False they are distinguished by probability
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What is the density of a material if its mass is 32 grams and its volume is 8 milliliters
vagabundo [1.1K]

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4 kilograms/liters

Explanation:

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Which is a characteristic of mixtures?
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The correct answer is "They can be separated by physical processes"

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PbSO4 has a Ksp = 1.3 * 10-8 (mol/L)2.
Oduvanchick [21]

i. The dissolution of PbSO₄ in water entails its ionizing into its constituent ions:

\mathrm{PbSO_{4}}(aq) \rightleftharpoons \mathrm{Pb^{2+}}(aq)+\mathrm{SO_4^{2-}}(aq).

---

ii. Given the dissolution of some substance

xA{(s)} \rightleftharpoons yB{(aq)} + zC{(aq)},

the Ksp, or the solubility product constant, of the preceding equation takes the general form

K_{sp} = [B]^y [C]^z.

The concentrations of pure solids (like substance A) and liquids are excluded from the equilibrium expression.

So, given our dissociation equation in question i., our Ksp expression would be written as:

K_{sp} = \mathrm{[Pb^{2+}] [SO_4^{2-}]}.

---

iii. Presumably, what we're being asked for here is the <em>molar </em>solubility of PbSO4 (at the standard 25 °C, as Ksp is temperature dependent). We have all the information needed to calculate the molar solubility. Since the Ksp tells us the ratio of equilibrium concentrations of PbSO4 in solution, we can consider either [Pb2+] or [SO4^2-] as equivalent to our molar solubility (since the concentration of either ion is the extent to which solid PbSO4 will dissociate or dissolve in water).

We know that Ksp = [Pb2+][SO4^2-], and we are given the value of the Ksp of for PbSO4 as 1.3 × 10⁻⁸. Since the molar ratio between the two ions are the same, we can use an equivalent variable to represent both:

1.3 \times 10^{-8} = s \times s = s^2 \\s = \sqrt{1.3 \times 10^{-8}} = 1.14 \times 10^{-4} \text{ mol/L}.

So, the molar solubility of PbSO4 is 1.1 × 10⁻⁴ mol/L. The answer is given to two significant figures since the Ksp is given to two significant figures.

8 0
3 years ago
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