Table 18.2 Ka Values for Some Monoprotic Acids at 25°C Name (Formula) Lewis Structure* к Iodic acid (HIO,) н-о—1—0 1.6X10-1 :0: Chlorous acid (HCi,) H-Ö-i-ö 1.12X10 Nitrous acid (HNO,) H-Ö-N=Ö 7.1X10+ Hydrofluoric acid (HF) H-E: 6.8X104 :O: Formic acid (HCOOH) H-C-ö-H 1.8X10 4 :O: Benzoic acid (C,H,COOH) C-0-H 6.3x103 H :0: Acetic acid (CH,COOH) Н-С c-ö-H 1.8X103 Н н H :0: Propanoic acid (CH,CH,COOH) Н-с- C-0-H 1.3X10 Hypochlorous acid (HCIO) н-б-бн 2.9x10-* Hypobromous acid (HBRO) н-о— б 2.3x10- Hydrocyanic acid (HCN) 6.2x10-10 H-CEN: Phenol (C,H,OH) O-ö-H 1.0x10-10 Hypoiodous acid (HIO) н-б- 2.3X1011 "Red type indicates the ionizable proton; structures have zero formal charge. ACID STRENGTH
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
(a) Use Table 18.a or Apendix C to calculate the Kb of the iodate ion, IO3-?
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