Part A Rank the following compounds in order of decreasing acid strength using p

Question

Part A

Rank the following compounds in order of decreasing acid strength using periodic trends.

Rank the acids from strongest to weakest. To rank items as equivalent, overlap them.

Part B

Without consulting the table of acid-dissociation constants, match the following acids to the given Ka1 values.

Drag the appropriate items to their respective bins.

Part C

Identify the Lewis acid in the following reaction: Cr3+(aq)+6H2O(aq)Cr(H2O)63+(aq)

Part D

Classify each of the following as a Lewis acid or a Lewis base

Explanation / Answer

Part A

Stronger the acid (HA), stronger will be it's capacity to donate H+ or in other words greater will be stabilty of A -.

So the ranking of the below compounds as acids from strongest to weakest will be as follows.

HI < HCl < H2S < LiH

Actuallly LiH is a strong base and releases H- .

Part B: Ka1 values not given in the question

Sulfuric acid (H2SO4) is a stronger acid than Sulfurous acid (H2SO3). Sulfuric acid is a diproticacid, meaning that it yields two protons (H+) per molecule when it dissociates in water. Again, H2S is a much weaker acid.

Now, stronger the acid , more willl be the value of Ka1  (acid dissociation constant)

So the ranking of the below compounds with decreasing Ka1 (acid dissociation constant) will be as follows.

H2SO4 < H2SO3 < H2S

Part C

Identify the Lewis acid in the following reaction: Cr3+(aq)+6H2O(aq)Cr(H2O)63+(aq)

We know, Lewis acids accept pairs of electrons. Here, Cr3+is accepting lone pair of electrons from6 molecules of H2O.

So Cr3+ is the Lewis acid in the above equation.

Part D:

Lewis bases donate pairs of electrons whereas Lewis acids accept pairs of electrons

So, (CH3)3N , CH3OH, H-, Br- , NO2- are Lewis bases because they donate pair of electrons

and AlCl3 , Ag+ are Lewis acids because accept pairs of electrons.

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