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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+
What is the Bronsted-Lowry definition of acid?
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
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.
What is the conjugate base and acid of H2SO3 according to Bronstad-lowry?
The conjugate base of H2SO3 is HSO3- and the conjugate acid is H3O+.
Bronsted and Lowry defined an acid as a substance that protons in a reaction with a base?
The Brønsted-Lowry acid-base theory was discovered in 1923 by two independent people. Jahannes Brønsted Thomas Lowry. In this theory an acid base reaction is one that involves the transfer of a hydrogen ion (H+) from one substance to another. The acid donates the ion while the bases accepts it.ExampleHCl + H2O → H3O+ + Cl- Hydrochloric acid (HCl) is an acid because it donated a proton (hydrogen) to the water creating a hydronium ion.NH3 + H2O → NH4+ + OH-Ammonia (NH3) is a base because it accepts a proton from the water molecule to form ammonium.
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+
What is the Bronsted-Lowry definition of acid?
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
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)
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 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.
What is the conjugate base and acid of H2SO3 according to Bronstad-lowry?
The conjugate base of H2SO3 is HSO3- and the conjugate acid is H3O+.
Bronsted and Lowry defined an acid as a substance that protons in a reaction with a base?
The Brønsted-Lowry acid-base theory was discovered in 1923 by two independent people. Jahannes Brønsted Thomas Lowry. In this theory an acid base reaction is one that involves the transfer of a hydrogen ion (H+) from one substance to another. The acid donates the ion while the bases accepts it.ExampleHCl + H2O → H3O+ + Cl- Hydrochloric acid (HCl) is an acid because it donated a proton (hydrogen) to the water creating a hydronium ion.NH3 + H2O → NH4+ + OH-Ammonia (NH3) is a base because it accepts a proton from the water molecule to form ammonium.
What ions would you expect to find when an acid dissolves in water what ions would expect to find when a base dissolves in water?
This is not a simple answer but nevertheless a complete one according to the Bronsted-Lowry acid / base theory. Acid in water: H3O+ ions from the acid (as proton donor to a water molecule) and the conjugated base anion (negative) as the left over part of the original acid molecule. Example: HCl + H2O --> H3O+ + Cl- Base in water: Most bases are negative anions from basic salts. You'll find in solution (some) OH- ions (together with (base)- ions) and the accompanying metal ion (together with some conjugated acid). Example of acetate base: NaF + H2O --> Na+ + F- + OH- + HF Example of an exception, ammonia: NH3(g) + H2O --> NH4+ + OH-
What ions would you expect to find when an acid dissolves in water what ions would you expect to find when a base dissolves n water?
This is not a simple answer but nevertheless a complete one according to the Bronsted-Lowry acid / base theory. Acid in water: H3O+ ions from the acid (as proton donor to a water molecule) and the conjugated base anion (negative) as the left over part of the original acid molecule. Example: HCl + H2O --> H3O+ + Cl- Base in water: Most bases are negative anions from basic salts. You'll find in solution (some) OH- ions (together with (base)- ions) and the accompanying metal ion (together with some conjugated acid). Example of acetate base: NaF + H2O --> Na+ + F- + OH- + HF Example of an exception, ammonia: NH3(g) + H2O --> NH4+ + OH-
What ions would you expect to find when an acid dissolves in water what ions would you expect to find when a base dissolves in water?
This is not a simple answer but nevertheless a complete one according to the Bronsted-Lowry acid / base theory. Acid in water: H3O+ ions from the acid (as proton donor to a water molecule) and the conjugated base anion (negative) as the left over part of the original acid molecule. Example: HCl + H2O --> H3O+ + Cl- Base in water: Most bases are negative anions from basic salts. You'll find in solution (some) OH- ions (together with (base)- ions) and the accompanying metal ion (together with some conjugated acid). Example of acetate base: NaF + H2O --> Na+ + F- + OH- + HF Example of an exception, ammonia: NH3(g) + H2O --> NH4+ + OH-
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.
What is the base of H3O plus is water or not?
The conjugate base for the hydronium ion (H3O+) is indeed water
