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.
Ammonia (NH3) --> can become NH2- or NH4+ Water (H2O) --> can become OH- or H3O+
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.
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
Ammonia Reaction Isn't SYNTHESIS REACTION?
It is a Bronsted-Lowery base because the carbonyl oxygens will readily accept a proton.
Ammonia (NH3) --> can become NH2- or NH4+ Water (H2O) --> can become OH- or H3O+
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.
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.
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?
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
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
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-