0
No, not all substances that are Arrhenius acids or bases are also Bronsted-Lowry acids or bases. Arrhenius acids and bases are defined based on their ability to increase the concentration of hydrogen ions or hydroxide ions in solution, while Bronsted-Lowry acids and bases are defined based on their ability to donate or accept a proton. Some substances can be Arrhenius acids or bases without being Bronsted-Lowry acids or bases, and vice versa.
What else can I help you with?
An arrhenius acid is an bronsted lowry acid bt an arrhenius base is NT a bronsted lowry base?
Yes, that's correct. An Arrhenius acid releases H+ ions in water, making it a Bronsted-Lowry acid. On the other hand, an Arrhenius base releases OH- ions in water but may not necessarily donate or accept protons in other reactions, so it is not always considered a Bronsted-Lowry base.
Could a bronsted-lowry acid not be an arrhenius acid?
Yes, a Brønsted-Lowry acid can be a different concept from an Arrhenius acid. While both concepts define acids based on their ability to donate protons, the Arrhenius definition is limited to substances that produce H+ ions in aqueous solutions, whereas the Brønsted-Lowry definition extends to reactions that occur in non-aqueous solvents.
Are all Brnsted-Lowry bases also considered Arrhenius bases?
Yes, all Brnsted-Lowry bases are also considered Arrhenius bases.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
A Bronsted-Lowry base is a?
A Brønsted-Lowry base is a substance that can accept a proton (H+) in a chemical reaction. This definition focuses on the transfer of protons between substances, with the base receiving a proton from an acid.
An arrhenius acid is an bronsted lowry acid bt an arrhenius base is NT a bronsted lowry base?
Yes, that's correct. An Arrhenius acid releases H+ ions in water, making it a Bronsted-Lowry acid. On the other hand, an Arrhenius base releases OH- ions in water but may not necessarily donate or accept protons in other reactions, so it is not always considered a Bronsted-Lowry base.
Could a bronsted-lowry acid not be an arrhenius acid?
Yes, a Brønsted-Lowry acid can be a different concept from an Arrhenius acid. While both concepts define acids based on their ability to donate protons, the Arrhenius definition is limited to substances that produce H+ ions in aqueous solutions, whereas the Brønsted-Lowry definition extends to reactions that occur in non-aqueous solvents.
Are all Brnsted-Lowry bases also considered Arrhenius bases?
Yes, all Brnsted-Lowry bases are also considered Arrhenius bases.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
A Bronsted-Lowry base is a?
A Brønsted-Lowry base is a substance that can accept a proton (H+) in a chemical reaction. This definition focuses on the transfer of protons between substances, with the base receiving a proton from an acid.
What of the three acid definitions is the broadest?
The Bronsted-Lowry acid definition is considered the broadest because it not only includes the donation of a proton, like the Arrhenius definition, but also considers the transfer of a proton to a base. This allows for a wider range of substances to be classified as acids.
How did bronsted and lowry change the definition of an acid?
Bronsted and Lowry expanded the definition of an acid from just donating a proton to also include the ability to accept a pair of electrons. This broader definition includes reactions where molecules can both donate and accept protons, leading to a more comprehensive understanding of acid-base reactions.
What is true of a Brønsted-Lowry acid?
A Brønsted-Lowry acid is a substance that donates a proton (H+ ion) in a chemical reaction. It can also be defined as a substance that increases the concentration of H+ ions in a solution.
Is H3BO3 an acid or a base?
No, it is a niether bronsted lowry base nor bronsted acid. It is a lewis acid because it can accept electron pairs. For this to be a bronsted lowry acid, it would have to donate a proton, which this molecule is incapable of due to its electronic deficiency. I hope this helps.
How can you justify that bronsted-lowery concept of acid and base?
The Brønsted-Lowry concept defines an acid as a proton donor and a base as a proton acceptor, which allows for a broader range of substances to be classified as acids and bases compared to the Arrhenius definition. This concept also explains acid-base reactions involving solvent molecules as proton donors or acceptors without requiring water as the solvent, making it versatile and widely applicable in different chemical systems. Furthermore, the Brønsted-Lowry concept accounts for the transfer of protons in reactions, providing a fundamental understanding of how acids and bases interact.
How do you know if a molecule is a base or an acid?
In brief: It could be done by measuring its pH level. Descriptive: There are a few ways to define an acid or a base: Arrhenius Defined acids and bases this way: Arrhenius Acids form H+ in solution Arrhenius Bases form OH- in solution Bronsted and Lowry defined acids and bases this way: Bronsted-Lowry Acids donate an H+ in solution Bronsted-Lowry Bases accept an H+ in solution OR in more general terms: Lewis defined acids and bases this way: Lewis Acids are defined as: Electron pair acceptors Lewis Bases are defined as: Electron pair donors As the user above me has already stated, you can also measure its pH. pH measures the concentration of Hydronium ions in a solution (H3O+) (it is NOT H+; H+ does not really exist by itself in this form). pH measurements range from 0 to 14 at the temperature of 298 K (25 centigrade). IF: pH < 7, it is acidic. pH = 7, it is neutral; neither acidic nor basic pH > 7, it is basic.
What did Svante Arrhenius do?
Svante Arrhenius was a Swedish scientist known for his work in physical chemistry. He was the first to propose the theory of electrolytic dissociation, which explains how substances dissolve in water to form ions. Arrhenius also made significant contributions to the understanding of acids and bases, winning the Nobel Prize in Chemistry in 1903 for his work.
