Presentation on theme: "Modern Theories of Acids & Bases The Arrhenius and Bronsted-Lowry Theories."— Presentation transcript:
Modern Theories of Acids & Bases The Arrhenius and Bronsted-Lowry Theories
Acids & Bases Acids and bases are special kinds of electrolytes. Like all electrolytes they break up into charged particles. What sets them apart from each other, and other electrolytes is the way that they break up.
Arrhenius Acids Svente Arrhenius (who first proposed the theory of ionization) identified acids as substances that ionize in water to produce hydronium ion. For example: HCl + H 2 O H 3 O + + Cl - Any substance that ionizes in water to produce hydronium ion can be classified as an acid.
H 3 O + (aka H + ) The hydronium ion is also known as a hydrogen ion. This allows us to shorten the ionization reactions for acids. The following equations represent the same chemical change: HCl + H2O H3O+ + Cl- and HCl H+ + Cl- However, it should be understood that H + is an abbreviation for the hydronium ion. H + ions DO NOT exist in water solution but are snatched up by water molecules to form hydronium ions.
Arrhenius Base Svente Arrhenius also identified bases as substances that ionize in water to produce hydroxide ion. For example: NaOH Na + + OH - Any substance that ionizes in water to produce hydroxide ion can be classified as a base.
Salts Ionic substances that break up in solution to produce ions other than hydronium and hydroxide ions. NaCl (s) Na + (aq) + Cl - (aq) KNO 3 (s) K + (aq) + NO 3 - (aq) Li 2 SO 4 (s) 2 Li + (aq) + SO 4 2- (aq) Salts are made up of positive (metal) and negative (non- metallic or polyatomic) ions. The more familiar you become with Table E, the easier it will be for you to identify salts.
Salts Salts are generally defined as ionic substances that PRIMARILY produce positive and negative ions other than hydronium or hydroxide when they dissolve in water.
Practice Identify each of the following as acids/bases/salts and show how they ionize : 1.HC 2 H 3 O 2 2.K 2 SO 4 3.KOH 4.LiOH 5.HNO 3 Acid HC 2 H 3 O 2 H + + C 2 H 3 O 2 - Acid HNO 3 H + + NO 3 - Base KOH K + + OH - Base LiOH Li + + OH - Salt K 2 SO 4 2K+ + SO 4 2-
Properties of Acids Neutralize bases to form a salt and water Have a sour taste (example: citric acid, vinegar) React with active metals to produce a salt plus hydrogen gas. Have pH’s less than 7 Affect indicators Why? All acids have the following properties : Because all acids have H3O+ ions present!
Properties of Bases Neutralize acids to form a salt and water Have a bitter taste (example: unsweetened chocolate, heroin) Are slippery. React with fats/oils to form soap (saponification) Have pH’s greater than 7 / Affect indicators Why? All bases have the following properties : Because all bases have OH - ions present!
Bronsted-Lowry Acids & Bases Another theory of acids & bases
Not everyone was happy with Arrhenius’s definition A major problem with the Arrhenius definition of acids and bases is that it limits acids and bases to water (aqueous) solutions. Since an acid requires water to ionize and form hydronium ions, there can be no Arrhenius acids unless water is involved as the solvent.
Relationship between the two models Arrhenius Acids/Bases only exist in water solutions. Bronsted- Lowry Acids/Bases can exist when no water is present All Arrhenius acids and bases can also be classified as Bronsted-Lowry acids and bases.
Bronsted-Lowry Definitions Bronsted and Lowry felt that this was too limiting, since there are many non-aqueous systems (no water is present). They came up with the following definitions for acids and bases. An acid is a proton (H + ion) donor A base is a proton acceptor
An example In the reaction below there are no Arrhenius acids or bases present (because no hydronium ions or hydroxide ions are formed). However, the HCl is acting as a Bronsted- Lowry acid because it is giving a H + ion to the NH 3 (which is acting as a H + ion acceptor - a base)
Acid & Bases are Roles In the Bronsted-Lowry definition, substances are classified as acids or bases depending on how they behave in a given situation. This means that the same substance can act as a acid in one reaction (by donating a proton) while acting as a base in another reaction
HCl as a proton donor Consider the following reaction: Since the HCl gives up a H+ ion to the water it is acting as a Bronsted-Lowry acid. In the process of donating the proton it also forms a hydronium ion, and that makes it an Arrhenius acid as well.
Water as a base But what does that make the water molecule? Since the water molecule is accepting the H+ ion, it is acting as a Bronsted-Lowry base. Since there is no hydroxide ion (OH-) formed, the water is not acting as an Arrhenius base in this reaction.
Ammonia as a base Let’s look at another example: Here the ammonia molecule is accepting a H+ ion and therefore is acting as an Bronsted-Lowry base. However, in the process of reacting with the water it is also forming a hydroxide ion. That makes the ammonia an Arrhenius base as well.
But what about the water? Since the water is giving up a H+ ion, it is acting as a Bronsted-Lowry acid. Since it does not form hydronium ions, it is NOT acting an Arrhenius acid.
So is water an acid or a base? In one example, we said that water was acting as a base, and in another example we said that it was acting as an acid. Some of you may be confused by this because you are thinking of acids and bases as being like boys and girls. Boys are boys and girls are girls, and they can’t switch back and forth. However, acids and bases are NOT like this.
Teacher-student model Teachers give off information (like acids give off protons) Students accept information (like bases accept protons) Sometimes teachers are students, and sometimes students are teachers Teacher and students are roles that individuals play depending on the situation. Acid and base are roles that molecules play in a particular chemical reaction. In different reactions they may play different roles.
Amphoteric/Amphiprotic Sometimes a molecule can donate a proton (act as an acid) and sometimes it can accept a proton (act as a base). Molecules that have this ability to act as both an acid and a base are called amphoteric or amphiprotic. Water is the most common example of an amphoteric substance.
Reality check For each of the following reactions identify any Bronsted- Lowry acids and bases. HNO 3 + H 2 O H 3 O + + NO 3 - HNO 3 + NH 3 NH 4 + + NO 3 - S 2- + H 2 O HS - + OH - HS - + OH - S 2- + H-OH HS - + HCl H 2 S + Cl - Are any of the substances above amphoteric? acid base
Strong/Weak Acids Acids can be either strong electrolytes or weak electrolytes. Strong acids (such as HCl) completely break up into their ions: HCl (aq) H + (aq) + Cl - (aq) Weak acids (such as HC 2 H 3 O 2 ) only partially break up into their ions: HC 2 H 3 O 2 H + (aq) + C 2 H 3 O 2 - (aq ) Weak acids don’t completely break up because they go to equilibrium!
Acid-base equilibrium Many acid base reactions go to equilibrium, that is they have both a forward and reverse reactions For instance, acetic acid (HC 2 H 3 O 2 ) reacts with water to form hydronium ion and acetate ion.
The reverse reaction However, the acetic acid only partially ionizes because a reverse reaction takes place preventing the forward reaction from reaching completion. In the reverse reaction, the Hydronium ion acts as an acid (a proton donor) while the acetate ion acts as the base.
Conjugate Acid-Bases When a substance donates a proton, the substance that is left is its conjugative base: Notice that the conjugative base is accepting a proton in the reverse reaction. Every acid has a conjugative base
Conjugative Acid-Base Pairs 2 When a substance accepts a proton, the substance that is formed is its conjugative acid: Notice that the conjugative acid is donating a proton in the reverse reaction. Every base has a conjugative acid
Strong/Weak Bases Bases can be either strong electrolytes or weak electrolytes. Strong bases (such as NaOH) completely break up into their ions: NaOH (aq) Na + (aq) + OH - (aq) Weak bases (such as NH 3 ) only partially break up into their ions: NH 3 (aq) + H 2 O NH 4 + (aq) + OH - (aq ) Weak bases don’t completely break up because they go to equilibrium!
Identify the amphoteric substances in this chart.
Types of Salts Salts can be classified as being: neutral acidic Basic How a salt is classified depends upon whether secondary reactions between the ions making up the salt and water form either hydronium or hydroxide ions.
Determining the type of salt The type of salt for a particular salt can be determined experimentally by testing the salt solution with universal indicator paper. –neutral salts will have a pH of 7 –acidic salts will have a pH of less than 7 –basic salts will have a pH of greater than 7 Typically, the pH values of salt solutions will be closer to 7 than that of acids or bases.
Predicting the type of salt All salts can be considered to be formed from their “parent” acid and base by means of the neutralization reaction. Acid + Base Salt + Water The type of salt can be theoretically predicted based on the properties of the “parent” acid and the “parent” base.
Neutral Salts Neutral salts are formed from a reaction between a strong acid and a strong base. (Remember neutralization reactions are double replacement reactions.) For instance, HCl + NaOH NaCl + HOH (since HCl is a strong acid and NaOH is a strong base, NaCl is a neutral salt.)
Acidic Salts Acidic salts are formed from a strong acid and a weak base. For instance, HCl + NH 4 OH NH 4 Cl + HOH (since HCl is a strong acid and NH 4 OH is a weak base, NH 4 Cl is an acidic salt.)
Basic Salts Basic salts are formed from a weak acid and a strong base. For instance, HC 2 H 3 O 2 + NaOH NaC 2 H 3 O 2 + HOH (since HC 2 H 3 O 2 is a weak acid and NaOH is a strong base, NaC 2 H 3 O 2 is a basic salt.)
Strong and weak acids In predicting the type of salt it is helpful to remember the three strong acids: HCl – hydrochloric acid HNO 3 – nitric acid H 2 SO 4 – sulfuric acid Most other acids are weak. Acetic acid (HC 2 H 3 O 2 ) is the most common weak acid discussed in Regents chemistry.
Strong and Weak Bases For bases, the Group I hydroxides are all strong bases. LiOH – lithium hydroxide NaOH – sodium hydroxide KOH – potassium hydroxide Most other hydroxides can be considered as weak bases. Ammonia or Ammonium hydroxide (NH 3 or NH 4 OH) is the most common weak base discussed in Regents chemistry.
Try these Identify the parent acid and base for the following salts, identify them as strong or weak and predict the type of salt formed.