The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, pH = -log[H,O+] Assuming each solution to be 0.10 mol L, rank the following aqueous solutions in order of decreasing pH In neutral solutions at 25 °C, [H3O+] = 10-7 mol L- and pH = 7. As [H3O+] increases, pH decreases, so acidic solutions have a pH of less than seven. Basic solutions have a pH greater than seven. The hydroxide and hydronium ion concentrations are related by the ion- product constant of water, Ku, as follows: Rank the solutions from the highest to lowest pH To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help Ku = 1.0 x 10 14 = [H3O+][OH ] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the K expression that PН + рОН — 14. HCI HOCI N,H4 NaOH Ba(OH)2 Highest pH Lowest pH O The correct ranking cannot be determined. Submit
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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