Table 4.1 pk, Values for Some Organic and Inorganic Acids Acld Formula PK. Conjugate Base CH,CH, Weaker Ethane CH,CH, 51 Stronger conjugate base acid Ethylene CH,=CH, 44 CH=CH Ammonia NH, 38 NH, Hydrogen H, 35 H Acetylene HC=CH 25 HC=C CH,CH,OH CH,CH,0 Ethanol 15.9 Water H,0 15.7 но CH,NH, Methylammonlum lon 10.64 CH,NH, Bicarbonate lon HCO, 10.33 co,?- CH,0 Phenol CH,OH 9.95 Ammontum fon NH, 9.24 NH, Hydrogen sulfide H,S 7.04 HS Pyridinlum C,H,NH 5.2 C,H,N Benzoie acid CH,COOH 4.19 CH,COO Hydrogen fluoride HF 3.2 F- Stronger acid Weaker Phosphorie acid H,PO, 2,1 H,PO, conjugate base p-Toluenesulfonic acid CH,C,H,SO,H CH,C,H,SO, 0.7 Nitric acid HNO, -1.5 NO, Hydronium ion H,0* -1.74 H,0 Sulfuric acid H,SO, -5.2 HSO, Hydrogen chloride HCI -7 CI Hydrogen bromlde HBr -8 Br Hydrogen lodide HI -9.9 CH,CH,O- + HCI
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.
complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids
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