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No. Although all Bronsted-Lowry acids with H+ protons are also Lewis acids, Lewis acid classification is usually reserved for substances like CO2 and BF3 that don't have protons.
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What ion do acidic compounds contain?
At least one H+ ion, called proton, and one anion which remains when the proton is donated to a base or to a water molecule: H3O+ (hydronium) is formed, lowering pH of the water.The above isn't actually wrong, though it's worth noting that that's actually a description of a particular type of acid (an Arrhenius or possibly Brønsted-Lowry acid). Lewis acids use a more general definition and are not required to contain any particular ion... any electron pair acceptor is a Lewis acid. (All Lewis acids are Brønsted acids, but not all Brønsted acids are Lewis acids.)
What do hydrochloric acid sulfuric acid nitric acid phosphoric acid have in common?
They are all strong acids and they dissociate ( at least the first proton ) completely in solution.
What do all acids contain?
Acids contain the cation H+ (or COOH-) and an anion or radical.
What is a substance which yields an anion plus a proton?
All acids yield a proton and a anion. For eg: HCl -------> H+ + Cl- H2SO4 --------> H+ + SO42-HNO3 ---------> H+ + NO3-
What atom or element is common to all acids?
Hydrogen is found in all acids. A Strong acid is one which can produce a high concentration of hydrogen ions. When acids touch metal hydrogen gas is emitted XD
All acids ionise in water to give?
All Arrhenius acids ionize in water to give H+ ions. While Lewis acids are proton donors.
What ion do acidic compounds contain?
At least one H+ ion, called proton, and one anion which remains when the proton is donated to a base or to a water molecule: H3O+ (hydronium) is formed, lowering pH of the water.The above isn't actually wrong, though it's worth noting that that's actually a description of a particular type of acid (an Arrhenius or possibly Brønsted-Lowry acid). Lewis acids use a more general definition and are not required to contain any particular ion... any electron pair acceptor is a Lewis acid. (All Lewis acids are Brønsted acids, but not all Brønsted acids are Lewis acids.)
What accepts a hydrogen ion from another compound?
All the Lewis acids accept hydrogen ion or proton from any othercompound having acidic hydrogen.
What do hydrochloric acid sulfuric acid nitric acid phosphoric acid have in common?
They are all strong acids and they dissociate ( at least the first proton ) completely in solution.
Why is the Brønsted-Lowry definition of acids more general than the Arrhenius definition?
A Brønsted-Lowry base accepts H+ ions.
What do all acids contain?
Acids contain the cation H+ (or COOH-) and an anion or radical.
Why all molecules with protons are not acids?
Assuming the Brønsted-Lowry definition of acids and bases, an acid is a molecule that donates a proton. While all atoms -- and therefore all molecules -- contain protons, not all are capable of donating them. Those that cannot donate a proton are not considered an acid under this terminology.
What does acids contain?
All acids contain at least one hydrogen ion.
What is a substance which yields an anion plus a proton?
All acids yield a proton and a anion. For eg: HCl -------> H+ + Cl- H2SO4 --------> H+ + SO42-HNO3 ---------> H+ + NO3-
Name the proton donor species which react with Grignard Reagent to give alkanes?
Such species include water, alcohols and all the acids.
Does The Brönsted concept describes a base as a proton donor in a reaction?
The Bronsted-Lowry theory of acids and bases states that acids are proton donors and bases are proton acceptors. The easiest example of this is mixing hydrochloric acid (HCl) with sodium hydroxide (NaOH). The acid donates a proton to water, forming hydronium (H3O+) and chloride (Cl-) ions, while the base splits into sodium (Na+) and hydroxide (OH-) ions. Hydronium and hydroxide are what actually "carry" the acidity/basicity, i.e. they are what react in an acid-base neutralization reaction, not the donating ions. The sodium and chloride ions stay stable in solution very well until the solution is evaporated, leaving pure table salt. If exactly equal amounts of HCl and NaOH are mixed, the pH will be exactly neutral (7). Bronsted-Lowry theory applies to more complex situations than the classic model, but it is helpful to remember that ALL theories of acids and bases will work for the simple example I listed above. Arrhenius (classic) acids increase hydronium concentration. Bronsted-Lowry acids are proton donors. Lewis acids are electron acceptors. Bases have opposite effects of acids as described by each of these three theories.
How can you tell acid from the base?
The currently accepted theory is the Lewis acid-base theory A Lewis base is an electron donor and a Lewis acid is a electron acceptor. Whether a compound is acid or base may not be obvious at first and difficult to work out. There are rules for working this out but you probably dont have to know them Generally, all you would probably have to know is that an acid is a proton [H+] donor and a base is proton acceptor
