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What else can I help you with?
Is NH4 plus a bronsted acid?
The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
IS NH4 A BRONSTEAD ACID OR BASE?
NH3 is a bronsted base. It has a lone pair.
Which if the following is an example of a bronsted-lowry acid?
Substances that can act both as an acid and as a base are called
What is the conjugate base for acid NH4 plus?
The conjugate base for acid NH4+ is NH3 (ammonia). When NH4+ loses a proton, it forms NH3, which can act as a weak base in a chemical reaction.
Can NH3 function as a bronsted-lowry base?
Yes, NH3 can function as a Bronsted-Lowry base because it can accept a proton (H+) to form its conjugate acid, NH4+ (ammonium ion). In this reaction, NH3 acts as a proton acceptor.
Is NH4 plus a bronsted acid?
The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
IS NH4 A BRONSTEAD ACID OR BASE?
NH3 is a bronsted base. It has a lone pair.
Is ammonium ion NH4 a Bronsted-Lowry base?
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
What is the conjugate acid of NH3?
NH4+ is NH3's conjugate acid. NH3 accepts H+ to become a Bronsted-Lowry base.
Which if the following is an example of a bronsted-lowry acid?
Substances that can act both as an acid and as a base are called
What is the conjugate base for acid NH4 plus?
The conjugate base for acid NH4+ is NH3 (ammonia). When NH4+ loses a proton, it forms NH3, which can act as a weak base in a chemical reaction.
Can NH3 function as a bronsted-lowry base?
Yes, NH3 can function as a Bronsted-Lowry base because it can accept a proton (H+) to form its conjugate acid, NH4+ (ammonium ion). In this reaction, NH3 acts as a proton acceptor.
Is NH3 a bronsted acid or base?
Well, darling, NH3 is a bronsted base. It's like the friend who always has your back and is ready to donate a proton at a moment's notice. So, if you're looking for some basic chemistry knowledge, NH3 is your go-to base buddy.
What is an example of a bronsted-lowry base?
An example of a Brønsted-Lowry base is ammonia (NH3). It can accept a proton (H+) to form its conjugate acid, ammonium ion (NH4+).
How would you write an equation that demonstrates the properties of acids and bases as defined by Bronsted and Lowry?
An equation demonstrating Bronsted-Lowry acid-base properties can be written as HA + B -> A- + HB+, where HA is the acid donating a proton (H+), B is the base accepting the proton, A- is the conjugate base formed by the acid losing the proton, and HB+ is the conjugate acid formed by the base accepting the proton. This equation shows the transfer of a proton from an acid to a base, following the Bronsted-Lowry definition of acids and bases.
Is NH3 an acid or a base?
well NH3 is a base that reacts with H2O to get NH4 + OH- NH3+ H2O-->NH4+ + OH- A conjugate base is the species formed when a Bronsted- Lowry base accepts a proton. NH4+ is the conjugate acid of NH3
Which are the two bronsted-lowry acids in NH3 plus H2ONH4 plus plus OH-?
In the reaction involving NH3 (ammonia) and H2O (water), the two Brønsted-Lowry acids are H2O and NH4+ (ammonium ion). H2O donates a proton (H+) to NH3, forming NH4+ and OH-. Thus, H2O acts as an acid by donating a proton, and NH4+ is the resultant acid formed in the reaction.
