As an organic chemistry student you will certainly discover yourself challenged with acid/based inquiries again and aacquire.

You are watching: Which of the following are produced when a base is dissolved in water

From categorizing molecules to ranking their strength without pKa or pKb values. This isn"t devastating if/when you learn it appropriately, however, your professor will assume you currently understand this.

So s/he won’t teach it.


Due to the fact that you’re intended to remember this from earlier in basic chemistry.

Instead your professor will certainly fly via the material and mean you to keep up.

But this won"t aid with the acid/base classifications.

Simply memorizing definitions without true expertise will not make it any kind of simpler. Especially as soon as challenged with a molecule that appears to fit even more than one acid/base interpretation.

So let"s take a look at acid/base meanings in an extra logical method.

Categories of Acids and Bases

Before we dive in, be certain to downfill my FREE acid/base cwarmth sheet to follow along currently and also take via you to research on the go – Organic Chemisattempt Acid Base Cwarmth Sheet

Acids and bases will certainly loss under one or more of the following three categories:

Arrhenius acids/basesBronsted-Lowry acids/basesLewis acids/bases

The essential right here is to identify that while each classification has a details definition, any kind of offered molecule can autumn right into more than one category, some right into all 3. Aget, somepoint we"ll look at later in this write-up.

Arrhenius Acid

An Arrhenius acid is a molecule that once dissolved in water will donate an H+ in solution. Sindicate put, a proton donor.

The trick to recognizing an Arrhenius acid is to look for a molecule that starts with an H, and also typically includes an oxygen or halogen.

Usual examples of Arrhenius acids include:

Hydrochloric Acid – HClNitric Acid – HNO3Sulfuric Acid – H2SO4Acetic Acid – HCH3CO2and so many more…

An acid dissociating in water does not create a free-floating proton. Instead one of the water molecules in solution will grab the H+ yielding a hydronium or H3O+ ion. Here"s what happens as soon as nitric acid dissociates in water.


Arrhenius Base

An Arrhenius base is a molecule that once liquified in water will certainly break dvery own to yield an OH- or hydroxide in solution. To acknowledge the Arrhenius base look for a molecule ending in OH, yet not complying with CHx which refers to an alcohol.

Arrhenius base examples include:

Sodium hydroxide – NaOHPotassium hydroxide – KOHMagnesium hydroxide – Mg(OH)2and also so many more…


But what if the acid/base is not liquified in water?

The Arrhenius interpretation for acids and also bases only describes compounds liquified in water. Does this suppose that acids and bases cannot exist out of water? Not quite, that"s wbelow the Bronsted-Lowry interpretation comes in.

Bronsted-Lowry Acid

A Bronsted-Lowry acid, like an Arrhenius acid, is a compound that breaks dvery own to provide an H+ in solution. The only distinction is that the solution does not need to be water. We can still describe the precise exact same acids as provided for the Arrhenius acid examples, however this time we"ll change the solvent to ammonia, alcohol, or anypoint else.

We observed what happens when nitric acid (HNO3) dissolves in water. Now let"s check out what happens as soon as it dissolves in ammonia (NH3) or even methanol (CH3OH)


Nitric acid still liquified to yield an H+ and NO3-, however this time it was NH3 and not water that picked up the free-floating proton.

Bronsted-Lowry Base

This is wbelow we begin to watch the difference in between the Bronsted-Lowry and Arrhenius meanings. While the Arrhenius base referred especially to the hydroxide (OH-) ion, the Bronsted-Lowry base refers to any atom or ion capable of accepting or bonding to a complimentary proton in solution.

Referring ago to the HNO3 + NH3 reaction above, as soon as ammonia picks up the free H+ it acts as a proton-acceptor. NH3 is the Bronsted-Lowry base in this example.

Further examples include:

Methanol – CH3OHFormaldehyde – H2COAnd even water – H2O

Lewis Acids and bases

The Lewis interpretation for acids and bases is the the majority of extreme bereason it"s not dealing with proloads particularly. Instead the Lewis meaning encounters the activity of electrons.

Lewis Acid/Base Mnemonic

Think of Lewis as ‘lectrons"

Lewis Acid

A Lewis acid refers to an atom or molecule that accepts an electron pair. Think earlier to your ‘pushing arrows" for orgo mechanisms. Eexceptionally time you draw an arrowhead representing the activity of electrons, the atom getting struck or accepting those electrons is the Lewis acid in that reaction.

Typical Lewis Acid Instances in Organic Chemistry

Borane – BH3 (hydroboration reaction)Aluminum Chloride – AlCl3 (electrophilic aromatic substitution reaction)Iron (III) Bromide – FeBr3 (electrophilic aromatic substitution reaction)and our excellent frifinish H+ (save reading)

The drawing below is part of the EAS Aromatic Halogecountry reactivity which you"ll check out in late Orgo 1 or Orgo 2. Notice exactly how the Fe gets struck by a lone pair of electrons. By accepting those electrons Fe acts as a Lewis acid


Lewis Base

Due to the fact that the Lewis definition hregarding perform with the carry of electrons, you can guess by now that a Lewis Base is an electron pair donor. Once aacquire think back to your reactivity mechanisms. The molecule utilizing its electrons to attack another atom is an electron pair donor and also a Lewis Base.

Here is the first step in acid catalyzed hydration. The pi bond attacking H+ makes the alkene a Lewis Base.


What If It Fits More Than 1 Category?

After finding out the individual acid/base definitions you"re likely perplexed and also overwhelmed.

So a lot indevelopment and so exceptionally similar!

And what happens if a molecule shows up to fit even more than one category?

For example:

Is OH- an Arrhenius Base? Or maybe its a Bronsted-Lowry or even Lewis Base?

The answer is possibly all 3!

The meanings above evolved gradually as scientists were beginning to understand also even more and also even more details about chemical reactions. The initially is a straightforward (no pun intended) definition, however the last 2 sindicate expand to fit even more facility solvents and cases.

Take a look at the reactivity listed below where the hydroxide ion assaults a proton on hydronium.


Arrhenius Acid Definition: Hydronium breaks as much as yield an H+ in solution.

Arrhenius Base Definition: Hydroxide is an OH- liquified in water.

Bronsted-Lowry Acid Definition: Hydronium is an H+ donor regardmuch less of solution

Bronsted-Lowry Base Definition: Hydroxide strikes and also accepts the H+ from hydronium.

Lewis Acid Definition: The H+ on Hydronium accepts the attacking electron pair to develop a bond.

Lewis Base Definition: Hydroxide donates its electron pair to develop a bond in between itself and also H+

Now that you understand the similarities/difference in between Arrhenius, Bronsted-Lowry, and also Lewis acids and bases, how execute you tell which is the more powerful or weaker acid? Which molecule is more reactive? Which side of a reactivity will be favored at equilibrium?

Learn this and also even more in my acids and bases tutorial video series:


In conclusion:

As an organic chemistry student you will certainly be compelled to acknowledge and classify 3 different types of acids and also bases. Arrhenius, Bronsted-Lowry, and also Lewis. While the technological definitions vary, as soon as you gain the logic behind their interpretations you"ll have the ability to conveniently and also conveniently identify the different forms of acids and bases.

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