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acid + base = conjucate base + conjugate acid (apex)
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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.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
What is considered as a Bronsted-Lowry base?
A Bronsted-Lowry base is a substance that is a proton acceptor. This means it can accept a proton (H+) from another substance in a chemical reaction. Examples of Bronsted-Lowry bases include hydroxide ions (OH-) and ammonia (NH3).
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-
Is PbI2 a Bronsted-Lowry acid?
No, PbI2 is not a Bronsted-Lowry acid. Bronsted-Lowry acids are substances that donate a proton (H+ ion) in a reaction, whereas PbI2 is lead iodide, which does not contain any hydrogen ions to donate.
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.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
What is considered as a Bronsted-Lowry base?
A Bronsted-Lowry base is a substance that is a proton acceptor. This means it can accept a proton (H+) from another substance in a chemical reaction. Examples of Bronsted-Lowry bases include hydroxide ions (OH-) and ammonia (NH3).
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-
What are the characteristics of Bronsted-Lowry base?
A Bronsted-Lowry base is a substance that accepts a proton in a chemical reaction. It can donate a pair of electrons to form a new bond with a proton. In water, Bronsted-Lowry bases can form hydroxide ions (OH-) when they accept a proton.
Is PbI2 a Bronsted-Lowry acid?
No, PbI2 is not a Bronsted-Lowry acid. Bronsted-Lowry acids are substances that donate a proton (H+ ion) in a reaction, whereas PbI2 is lead iodide, which does not contain any hydrogen ions to donate.
What is true of Bronsted-Lowry acid?
A Bronsted-Lowry Acid Donates H+ ions
What is a true Bronsted-Lowry acid?
A Bronsted-Lowry Acid Donates H+ ions
What is true of a bronsted Lowery base?
A Bronsted-Lowry base is a substance that can accept a proton or donate an electron pair. It is a proton acceptor in a chemical reaction.
What is the definition of a bronsted-Lowry base?
A Bronsted-Lowry base is a proton acceptor.
What is true of the bronsted-lowry base?
A Bronsted-Lowery base accepts H+ ions
Is ammonium ion NH4 a Bronsted-Lowry base?
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
