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3 years ago

Rank the following solutes in order of increasing entropy when 0.0100 moles of each dissolve in 1.00 liter of water.

Chemistry

1 answer:

vichka [17]3 years ago

4 0

Answer:

<em>The rank of the solutes in order of increasing entropy is</em>:

<em>CH₃OH < NaBr < CaCl₂ < Cr(NO₃)₃</em>

Explanation:

Assuming temperature and other conditions are the same, you can qualititatively precict the relative increase of entropy, when a given amount of solute dissolves in a fixed aomount of water, by looking at the number of particles (molecules or ions) that are formed.

The particles of solute that, prior to get dissolved, are pure and orderly separated, will be very scattered after the dissolution, increasing, consequently, the degree of randomness or dissorder of the system.

Also, the greater the number of particles formed from each unit formula, the greater the degree of disorder and the greater the entropy.

Hence, being the entropy a measure of the radnomness of the system, you can predict that the greater the number of particles (molecules or ions) dissolved, the greater the entropy.

Now look at the dissociation of each given solute:

CaCl₂ → Ca²⁺ + 2Cl⁻ : 3 ions are formed.

CH₃OH: is a molecular compound, so 1 molecule is dispersed.

Cr(NO₃)₃ → Cr³⁺ + 3 NO₃⁻: 4 ions are formed.

NaBr → Na⁺ + Br⁻ : 2 ions are formed.

Then, the rank in order of increasing entropy, is:

1 < 2 < 3 < 4

CH₃OH < NaBr < CaCl₂ < Cr(NO₃)₃

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The pH of a saturated solution of a metal hydroxide MOH is 10.15. Calculate the Ksp for this compound.

Airida [17]

Answer:

$Ksp=2.00x10^{-8}$

Explanation:

Hello!

In this case, since the pH of the given metal is 10.15, we can compute the pOH as shown below:

$pOH=14-pH=14-10.15=3.85$

Now, we compute the concentration of hydroxyl ions in solution:

$[OH^-]=10^{-pOH}=10^{-3.95}=1.41x10^{-4}M$

Now, since this hydroxide has the form MOH, we infer the concentration of OH- equals the concentration of M^+ at equilibrium, assuming the following ionization reaction:

$MOH(s)\rightarrow M^+(aq)+OH^-(aq)$

Whose equilibrium expression is:

$Ksp=[M^+][OH^-]$

Therefore, the Ksp for the saturated solution turns out:

$Ksp=1.41x10^{-4}*1.41x10^{-4}\\\\Ksp=2.00x10^{-8}$

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2 years ago

Water vapor particles are most likely to phase change into liquid particles if the vapor particles come into contact with

dalvyx [7]

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15. Calculate the hydrogen ion concentration of a

deff fn [24]

Answer:

Explanation:

pH = − log [H+] , we can solve for [H+] as,

− pH = log [H+] ,

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so PH =2.4 in you case is

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zavuch27 [327]

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2 years ago

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