Arrange these acids in terms of increasing acidity:

CH3COOH, NH3+CH2COOH, CH3CONHCH2COOH

My answer is CH3COOH,CH3CONHCH2COOH,NH3+CH2COOH .

Is this correct Dr.Bob?

It appears to me that you have them reversed.

But Dr.Bob,from what I refer,NH3+CH2COOH is the strongest acid since it has both acid and NH3 protonated.Acetic acid is a weak acid,I'm not sure about the CH3CONHCH2COOH. That's what confuses me

Yes, your answer is correct. To determine the increasing acidity of the given acids, we need to consider the relative strengths of their conjugate bases. The stronger the conjugate base, the weaker the acid.

Let's analyze each acid individually:

1. CH3COOH (acetic acid): Acetic acid is a weak acid. Its conjugate base, acetate (CH3COO-), is relatively stable and doesn't readily donate a proton, making acetic acid a weaker acid compared to the other acids in the list.

2. CH3CONHCH2COOH (glycine): Glycine is an amphoteric compound, meaning it can act as both an acid and a base. In this case, the amino group (NH2) can act as a proton donor, making glycine slightly more acidic than acetic acid.

3. NH3+CH2COOH (ammonium glycinate): This compound is derived from the reaction between ammonia (NH3) and glycine, resulting in the formation of a salt. The presence of the ammonium ion (NH4+) makes this compound more acidic compared to acetic acid and glycine.

Therefore, your arrangement is correct: CH3COOH (acetic acid) is the weakest acid, followed by CH3CONHCH2COOH (glycine), and NH3+CH2COOH (ammonium glycinate) is the strongest acid among the three.