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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+
Is FeBr3 a Bronsted Lowery base?
It is a Bronsted-Lowery base because the carbonyl oxygens will readily accept a proton.
Is HCO3 both a bronsted acid and base?
Oh, dude, HCO3 is like that ultimate multitasker in the chemistry world. It can totally be a Bronsted acid or base depending on the situation. So yeah, it's like a chameleon of the chemical world, just doing its thing, not caring too much about labels.
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.
What are examples of acids and base?
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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+
Which is a conjugate acid base pair in the following equation HS- plus H2O equals S-2 plus H30?
This is a Bronsted question. Hs- is the acid in this which makes H2O a base. Therefore S-2 is the conjugate base and the H3O+ hydronium ion is the conjugate acid.
Does A base is a compound that produces OH ions in solution?
There are Bronsted-Lowry bases and Lewis bases... Brønsted bases accept protons (H+) and Lewis bases donate electrons... So something like H2O + H2O--> H3O (hydronium) + -OH would mean that H2O is a Bronsted base and acid. You have to look at it in context.
Is FeBr3 a Bronsted Lowery base?
It is a Bronsted-Lowery base because the carbonyl oxygens will readily accept a proton.
Is HCO3 both a bronsted acid and base?
Oh, dude, HCO3 is like that ultimate multitasker in the chemistry world. It can totally be a Bronsted acid or base depending on the situation. So yeah, it's like a chameleon of the chemical world, just doing its thing, not caring too much about labels.
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.
What are examples of acids and base?
removing the my new software from my computer. then after suddenly receive that program from recycle bin. The software is most participator of our computer. Its crates a lot of lose data in computer.
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 H2O Brønsted-Lowry acid or base?
H2O can act as both a Brønsted-Lowry acid and base. As an acid, it can donate a proton by giving away a hydrogen ion. As a base, it can accept a proton by taking on a hydrogen ion. This makes H2O amphiprotic.
What is the acid and what is the base in the reaction HBr H2O - Br- H2O?
In the reaction, HBr donates a proton (H+) to H2O, making HBr the acid and H2O the base. The resulting products are Br- (conjugate base of HBr) and H3O+ (conjugate acid of H2O).
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 is a species that acts both an acid and a base?
Such organic species are alcohols and inorganic species include bicarbonate, bisulphate and biphosphate ions.
