Rank the compounds below in order of increasing acidity. " COH HO HO O2N Relevant Information: Kw= [H,O"] [OH]=1x 10-at 25 °C !! Strong Weak pH + pOH = 14 at 25 °C : pX =-log X Acid pH = -logC, 12 pH = -log(C,K] pK. + pK, - 14 at 25 °C for conjugate pairs Base POH = -logC, 1/2 %3D pOH = -log(C,K pH = pK, +log 4] [HA] !3! TA SA SA He 14.003 10 Ne 10. 12 4.0 40 20.1 is IN 4341012 13 AI SI 263 28 30 30 145 103 12 Na Mg 22 2431 CC Ar 20 Ca Sc TI 33 Cr Ma Fe 54 24 14 Co NI Cu Za Ga Ge As Se Br Kr 19.10 40.0 44447.041200 4 N11 93 s 4339 72 2 4 T NT o
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.
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