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Why can water act as an acid or a base in a bronsted lowry reaction?
Because a bronsted-lowry acid donates proton such as ( H+ ) and water can donate H+ such as ( H2O + NH3 ---> NH4+ + OH- ) here water donated H+ to ammonia to produce NH4 ( which is an acid )
Is an acid and a base both reactants?
Yes, in a chemical reaction, an acid and a base are both considered reactants. They react with each other in a neutralization reaction, typically producing water and a salt. This interaction is fundamental in acid-base chemistry, where the acid donates protons (H⁺), and the base accepts them.
Is AlOH3 an acid or a base?
Al(OH)3 is a base (Aluminum hyroxide)
What is used for fertilizer an acid or a base?
its either base or both because i put acid on a worksheet and got it wrong
Is pure water an acid a base neither or both?
baking powder
Is sulfuric acid a bronsted acid bronsted base or both?
Sulfuric acid is a Bronsted acid because it donates a proton (H+) in an acid-base reaction. It can act as a proton donor but not as a proton acceptor, which is the characteristic of a Bronsted base.
Is H2O Bronsted acid or base or both?
H2O can act as both a Bronsted acid and a Bronsted base. As an acid, it can donate a proton (H+) to another species, and as a base, it can accept a proton. The role it plays depends on the context of the reaction.
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.
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
Which compound can act as both a bronsted-lowry acid and a bronstey-lowry base?
Ammonia (NH3) --> can become NH2- or NH4+ Water (H2O) --> can become OH- or H3O+
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.
Is HCO3 both a bronsted acid and base?
HCO3- is both an acid and a base. It can donate a "proton" (hydrogen ion) as follows:HCO3(-) = H(+) + CO3(-2)orHCO3(-) + OH(-) = H2O + CO3(-2)It can also absorb a proton:HCO3(-) + H(+) = H2CO3Which occurs depends on the pH of the solution. The pKa values are given here:What_is_pka_value_for_sodium_bicarbonateH2CO3 is known as "carbonic acid". It can decompose into water and carbon dioxideH2CO3 = H2O + CO2
Why can water act as an acid or a base in a bronsted lowry reaction?
Because a bronsted-lowry acid donates proton such as ( H+ ) and water can donate H+ such as ( H2O + NH3 ---> NH4+ + OH- ) here water donated H+ to ammonia to produce NH4 ( which is an acid )
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.
Is ammonia amphoteric according to bronsted lawry concept?
No, according to the Brønsted-Lowry concept, an amphoteric substance can act as both an acid and a base. Ammonia (NH3) is a weak base, as it can accept a proton (H+) to form its conjugate acid NH4+. It does not have the ability to donate a proton, so it is not considered amphoteric according to the Brønsted-Lowry concept.
Is AI an acid or base?
Aluminium is not an acid or a base, but it does react with both acids and alkalis.
What kind of substance accepts an electron pairs?
Lewis acid like Al3+, I2Bronsted-Lowry acids like H3O+But not Bronsted-Lowry bases like OH- or S2- and not Lewis base like NH3 because they can NOT accept an electron pair (octet rule)
