Yes OH is in fact a Bronsted base making H3O a acid
HI is a Bronsted acid because in water, it donates a proton (HI + H2O --> H3O+ + I-)
SO4-2 ion is a Bronsted base because it may accept two H+ ions and forms H2SO4.
Average tap water scores a 7 on the pH scale. So it's not really either.
It is a Bronsted-Lowery base because the carbonyl oxygens will readily accept a proton.
Water can act as both a Brรธnsted-Lowry acid and base. As an acid, it donates a proton (H+) to a base; as a base, it accepts a proton from an acid. This ability is due to its amphiprotic nature.
Yes, bicarbonate (HCO3-) can act as both a Bronsted-Lowry acid and a base. As an acid, it donates a proton (H+) to another substance, while as a base, it accepts a proton. This ability to both donate and accept protons makes it amphiprotic.
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According to this concept an acid is a compound which donates a proton (H+). for example, HA + H2O ------------> A- + H3O+ acid water base hydronium ion
It is a Bronsted-Lowery base because the carbonyl oxygens will readily accept a proton.
Water can act as both a Brรธnsted-Lowry acid and base. As an acid, it donates a proton (H+) to a base; as a base, it accepts a proton from an acid. This ability is due to its amphiprotic nature.
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.
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According to this concept an acid is a compound which donates a proton (H+). for example, HA + H2O ------------> A- + H3O+ acid water base hydronium ion
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.
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 )
Ammonia Reaction Isn't SYNTHESIS REACTION?
Yes, bicarbonate (HCO3-) can act as both a Bronsted-Lowry acid and a base. As an acid, it donates a proton (H+) to another substance, while as a base, it accepts a proton. This ability to both donate and accept protons makes it amphiprotic.
Lithium Oxide is a base because when it is added to an acid for example Hydrochloric Acid (HCL) it is neutralised. Acid + Base is a neutralisation reaction. + Plus look at Arhenius's explanation on the theory of acid reactions and Bronsted lowry's theory on acids and bases. Because somewhere in there they talk about somthing that might help you a bit more if you are not confident with my answer.
acid is hbr and the base is h2o
C. Bronsted-Lowry base. In the given reaction, the carbonate ion (CO3^2-) accepts a proton (H+) from water, forming bicarbonate (HCO3-) and hydroxide (OH-) ions. Since the carbonate ion is gaining a proton, it is acting as a Bronsted-Lowry base.