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Convert Ph To Hydrogen Ion Concentration
On the method of converting pH and hydrogen ion concentration
There is a current issue related to the conversion of pH and hydrogen ion concentration. The degree of acid and base in the surface solution is closely related to the concentration of hydrogen ions, which cannot be ignored.
If you want to understand the reason, first understand its meaning. The concentration of hydrogen ions in a solution determines the nature of its acid and base. The setting of pH is a logarithmic method to briefly represent the concentration of hydrogen ions. If the pH value drops, the concentration of hydrogen ions rises; if the pH value rises, the concentration of hydrogen ions decreases, and the two change in reverse.
As for the conversion method, there are rules. If the pH is known, find the hydrogen ion concentration ($[H ^ +] $), and calculate it with the formula $[H ^ +] = 10 ^ {-pH} $. For example, if the pH of a solution is 3, substituting the formula, then $[H ^ +] = 10 ^ {-3} mol/L $. This is the method of changing the pH to find the hydrogen ion concentration.
Conversely, if the hydrogen ion concentration is known, find the pH value, and calculate it with $pH = -\ lg [H ^ +] $. Let the hydrogen ion concentration of a solution be 10 dollars ^ {-5} mol/L $, and substitute it into the formula to get $pH = -\ lg (10 ^ {-5}) = 5 $. From this perspective, the conversion of pH and hydrogen ion concentration is the foundation of chemistry and is useful in experiments and production. Scholars must be familiar with it and study its methods carefully in order to be able to handle related matters with ease.
There is a current issue related to the conversion of pH and hydrogen ion concentration. The degree of acid and base in the surface solution is closely related to the concentration of hydrogen ions, which cannot be ignored.
If you want to understand the reason, first understand its meaning. The concentration of hydrogen ions in a solution determines the nature of its acid and base. The setting of pH is a logarithmic method to briefly represent the concentration of hydrogen ions. If the pH value drops, the concentration of hydrogen ions rises; if the pH value rises, the concentration of hydrogen ions decreases, and the two change in reverse.
As for the conversion method, there are rules. If the pH is known, find the hydrogen ion concentration ($[H ^ +] $), and calculate it with the formula $[H ^ +] = 10 ^ {-pH} $. For example, if the pH of a solution is 3, substituting the formula, then $[H ^ +] = 10 ^ {-3} mol/L $. This is the method of changing the pH to find the hydrogen ion concentration.
Conversely, if the hydrogen ion concentration is known, find the pH value, and calculate it with $pH = -\ lg [H ^ +] $. Let the hydrogen ion concentration of a solution be 10 dollars ^ {-5} mol/L $, and substitute it into the formula to get $pH = -\ lg (10 ^ {-5}) = 5 $. From this perspective, the conversion of pH and hydrogen ion concentration is the foundation of chemistry and is useful in experiments and production. Scholars must be familiar with it and study its methods carefully in order to be able to handle related matters with ease.
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