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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.
What is true of the bronsted-lowry base?
A Bronsted-Lowery base accepts H+ ions
How can one determine a Bronsted-Lowry acid and base?
A Bronsted-Lowry acid is a substance that donates a proton (H) in a chemical reaction, while a Bronsted-Lowry base is a substance that accepts a proton. To determine if a substance is a Bronsted-Lowry acid or base, you can look at its behavior in a reaction - if it donates a proton, it is an acid, and if it accepts a proton, it is a base.
How can you justify that NH3 is bronsted Lowry base but not arrhenius base?
NH3 acts as a Bronsted-Lowry base because it can accept a proton (H+) to form the NH4+ ion. In contrast, NH3 does not produce hydroxide ions (OH-) in solution, which is a defining characteristic of an Arrhenius base.
In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
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.
What is true of the bronsted-lowry base?
A Bronsted-Lowery base accepts H+ ions
What are the bronsted - lowry definition of acid and base?
Arrhenius: Acid is a proton (H+) donor. Base is a -OH^- (hydroxyl) donor.B-L: Acid is a proton donor. Base is a proton acceptor.
How can one determine a Bronsted-Lowry acid and base?
A Bronsted-Lowry acid is a substance that donates a proton (H) in a chemical reaction, while a Bronsted-Lowry base is a substance that accepts a proton. To determine if a substance is a Bronsted-Lowry acid or base, you can look at its behavior in a reaction - if it donates a proton, it is an acid, and if it accepts a proton, it is a base.
How can you justify that NH3 is bronsted Lowry base but not arrhenius base?
NH3 acts as a Bronsted-Lowry base because it can accept a proton (H+) to form the NH4+ ion. In contrast, NH3 does not produce hydroxide ions (OH-) in solution, which is a defining characteristic of an Arrhenius base.
In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
Why is methylamine a bronsted-lowry base but not an arrhenius base?
Methylamine is a Bronsted-Lowry base because it can accept a proton (H+) to form its conjugate acid. It is not considered an Arrhenius base because it does not exclusively produce hydroxide ions (OH-) when dissolved in water, which is the defining characteristic of an Arrhenius base.
How does the Bronsted-Lowry definition of an acid differ from the Arrhenius definition of an acid?
The Bronsted-Lowry definition includes substances that donate protons, not just in aqueous solutions like the Arrhenius definition. This allows for a broader range of acidic substances to be classified. Additionally, Bronsted-Lowry acids can exist in non-aqueous environments, unlike Arrhenius acids which are limited to aqueous solutions.
Is sulfuric acid a bronsted-lowry acid or base?
As the name sulfuric acid might indicate, it is a bronsted-lowry acid.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
Is h3o an example of a bronsted lowry base?
No, H3O+ is an example of a Bronsted-Lowry acid because it can donate a proton. A Bronsted-Lowry base would be a substance that can accept a proton.
What is true about bronsted-lowry base?
A conjugate base is considered the deprotonated acid.
