Calculate the OH and the pH of a solution with an [H] = 5.6 x 10-¹0 M at 25 °C. [OH-] = 1.8 x10-5 pH = 9.26 Calculate the H* and the pH of a solution with an |OH| = 0.059 M at 25 °C. |H+| = 1.69 X10-13 pH = 12.77 Calculate the H* and the OH- of a solution with a pH = 2.70 at 25 °C. 2 X10 1.99 *1011 TOOLS JOH = M M M M
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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.
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![Calculate the [OH") and the pH of a solution with an [H*] = 5.6 × 10¯¹º M at 25 °C.
[OH-] = 1.8 x10-5
pH =
Calculate the H*) and the pH of a solution with an |OH" | = 0,059 M at 25 °C.
169 X10
pli=
Calculate the [H*| and the |OH¯| of a solution with a pH
2.70 al 25 "C
-3
JOH-] =
|OH|
1.99 ×1(11
TOOLS
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