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Aug 14, 2020 · The acid–base strength of a molecule depends strongly on its structure. The weaker the A–H or B–H+ bond, the more likely it is to dissociate to form an \(H^+\) ion. In addition, any factor that stabilizes the lone pair on the conjugate base favors the dissociation of \(H^+\), making the conjugate acid a stronger acid.
- Lewis Acids and Bases
Because \(\ce{HF}\) is a weak acid, fluoride salts behave as...
- Polyprotic Acids
Solution. As indicated by the ionization constants, H 2 CO 3...
- Strong Acids and Strong Bases
Evaluate solution pH and pOH of strong acids or bases. Acids...
- Lewis Acids and Bases
Feb 11, 2021 · Because fluoride is the least stable (most basic) of the halide conjugate bases, HF is the least acidic of the haloacids, only slightly stronger than acetic acid. HI, with a pK a of about -9, is one the strongest acids known. More importantly to the study of biological organic chemistry, this trend tells us that thiols are more acidic than ...
- Factor #1 – charge.
- Factor #2 – The Role of The Atom
- Factor #3 – Resonance
- Factor #4 – Inductive Effects
- Factor #5 – Orbitals
Removal of a proton, H+ , decreases the formal charge on an atom or molecule by one unit. This is, of course, easiest to do when an atom bears a charge of +1 in the first place, and becomes progressively more difficult as the overall charge becomes negative. The acidity trends reflect this: Note that once a conjugate base (B-) is negative, a second...
This point causes a lot of confusion due to the presence of two seemingly conflicting trends. Here’s the first point: acidity increases as we go across a row in the periodic table. This makes sense, right? It makes sense that HF is more electronegative than H2O, NH3, and CH4due to the greater electronegativity of fluorine versus oxygen, nitrogen, a...
A huge stabilizing factor for a conjugate base is if the negative charge can be delocalized through resonance. The classic examples are with phenol (C6H5OH) which is about a million times more acidic than water, and with acetic acid (pKaof ~4). Watch out though – it isn’t enough for a π system to simply be adjacent to a proton – the electrons of th...
Electronegative atoms can draw negative charge toward themselves, which can lead to considerable stabilization of conjugate bases. Check out these examples: Predictably, this effect is going to be related to two major factors: 1) the electronegativity of the element (the more electronegative, the more acidic) and the distance between the electroneg...
Again, the acidity relates nicely to the stability of the conjugate base. And the stability of the conjugate base depends on how well it can accomodate its newfound pair of electrons. In an effect akin to electronegativity, the more s character in the orbital, the closer the electrons will be to the nucleus, and the lower in energy (= stable! ) the...
Jul 12, 2023 · Evaluate solution pH and pOH of strong acids or bases. Acids and bases that are completely ionized when dissolved in water are called strong acids and strong bases There are only a few strong acids and bases, and everyone should know their names and properties. These acids are often used in industry and everyday life.
Jul 3, 2019 · HI: hydroiodic acid. HClO 4: perchloric acid. If the acid is 100 percent dissociated in solutions of 1.0 M or less, it is called strong. Sulfuric acid is considered strong only in its first dissociation step; 100 percent dissociation isn't true as solutions become more concentrated. H 2 SO 4 → H + + HSO 4-.
- Anne Marie Helmenstine, Ph.D.
Answers. A strong acid or base is 100% ionized in aqueous solution; a weak acid or base is less than 100% ionized. The overall reaction progress stops because the reverse process balances out the forward process. pH is a measure of the hydrogen ion concentration.
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Properties of Strong Acids and Bases [1-5] Strong Acids. Strong acids are characterized by the symbol HA, where H is the hydrogen atom, and A is an electronegative atom or species to which hydrogen is attached. Strong acids are good proton donors and can remain in an aqueous solution.
