difficulties recognizing weak acids and bases

[Samantha Hoegl Roy 2C]

I still have difficulties figuring out if a substance is a weak acid or base; for example, NH3. Does anyone have any advice and tips to make it easier?

[David Effio 1H]

So one dead giveaway of a wake acid or base is the presence of acidity or basicity constant (Ka or Kb respectively). Only a weak acid/base would have one of these. A chemical reaction involving a weak acid/base would have a double arrow, as some of the reactants would form back from the product through the reverse reaction

A giveaway for strong acids or bases would be that a strong acid/base is completely dissociated, meaning all of the acid or base will become its conjugate base or acid, leaving a concentration of 0 of the reactant. This can be determined by looking at the formula and seeing that the arrow is only pointing in the right direction, no double arrows.
Note, this is also why strong acids and bases do not have a Ka or Kb value, as dividing the resulting product concentration by the reactant concentration of 0 is not possible.

Strong acids usually have a pH of 0-1, as the resulting H30+ concentration is usually very large, while weak acids usually have a pH a little higher, as not all the acid dissociated into its conjugate base and a proton.

I hope that helps!

[mcredi]

Honestly, it is helpful to memorize them so the strong acids are hydrochloric acid, nitric acid, sulfuric acid, hydrobromic acid, hydroiodic acid, perchloric acid, and chloric acid. The only weak acid formed by the reaction between hydrogen and a halogen is hydrofluoric acid.

[Henry Dudley 1G]

So one dead giveaway of a wake acid or base is the presence of acidity or basicity constant (Ka or Kb respectively). Only a weak acid/base would have one of these. A chemical reaction involving a weak acid/base would have a double arrow, as some of the reactants would form back from the product through the reverse reaction

A giveaway for strong acids or bases would be that a strong acid/base is completely dissociated, meaning all of the acid or base will become its conjugate base or acid, leaving a concentration of 0 of the reactant. This can be determined by looking at the formula and seeing that the arrow is only pointing in the right direction, no double arrows.
Note, this is also why strong acids and bases do not have a Ka or Kb value, as dividing the resulting product concentration by the reactant concentration of 0 is not possible.

Strong acids usually have a pH of 0-1, as the resulting H30+ concentration is usually very large, while weak acids usually have a pH a little higher, as not all the acid dissociated into its conjugate base and a proton.

I hope that helps!

So for all of the problems with a given Ka or Kb value we are dealing with a weak acid or weak base?

[Swetha Ampabathina1I]

Most likely yes you will be dealing with weak acids and bases.

[Andrew Bennecke]

If a substance can donate or accept H+ atoms or lone e- pairs, it is most likely a weak acid or base. The only exceptions would be the strong acids (HCl, HF,HBr, etc.) and the strong bases (Group 1 or 2 elements + OH- ion).

[Charles Hood Disc 1C]

It can help to draw a Lewis structure and look for any lone pairs, or any hydrogens that could be donated.

[005199302]

Just a note: it is helpful to remember that nitrogen with a lone pair means it's a weak base

[daniella_knight1I]

If you see a Ka or Kb constant that's a giveaway. If not you'll have to draw out the lewis structure and look at the lone pairs to determine if it's a weak acid or base.

[505106414]

If you see a Ka or Kb constant that's a giveaway. If not you'll have to draw out the lewis structure and look at the lone pairs to determine if it's a weak acid or base.

Just clarifying that if you see a constant it is most likely a weak acid, not a strong one.