Some weak acids and their conjugate bases Acid (Proton Donor) Conjugate Base (Proton Acceptor) pKa Ką (M) НСООН HCOO +H+ 3.75 1.78 x 10-4 Formic acid Formate ion CH3COOH Acetic acid CH;CO0 Acetate ion +H* 4.76 1.74 x 10-5 OH OH +H* 3.86 1.38 x 10-4 CH3CH-COO CH3CH-COOH Lactic acid Lactate ion H;PO4 Phosphoric acid H,PO, Dihydrogen phosphate ion +H+ 2.14 7.24 x 10-3 H,PO, Dihydrogen phosphate ion HPO,?- Monohydrogen phosphate ion +H* 6.86 1.38 x 10-7 HPO2- Monohydrogen phosphate ion PO, +H+ 12.4 3.98 x 10-13 Phosphate ion H2CO3 Carbonic acid HCO3 Bicarbonate ion +H* 6.3* 5.1 x 10-7* HCO3 Bicarbonate ion co2- Carbonate ion +H* 10.25 5.62 x 10-11 C6H5OH Phenol +H+ 9.89 1.29 x 10-10 Phenolate ion NH4 NH3 +H+ 9.25 5.62 x 10-10 Ammonium ion Ammonia 1 1 1 1 111
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.
You need to make a buffer whose pH is 7.0, and you can choose from the weak acids shown. Briefly explain your choice
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