"pH ( pee-AYCH), also referred to as acidity, historically denotes 'potential of hydrogen' (or 'power of hydrogen'). It is a scale used to specify the acidity or basicity of an aqueous solution."
This topic covers the pH scale and how it is used to measure the acidity or basicity of a substance.
Introduction to acids and bases: This covers the basic definitions of acids and bases and their properties.
pH scale: This covers the concept of pH and its importance in understanding the strength of an acid or base solution.
Acid-base reactions: This covers the chemical reactions between acids and bases.
Acid-base indicators: This covers the use of indicators to measure pH.
Strength of acids and bases: This covers the concept of strong and weak acids and bases.
Acid-base equilibrium: This covers chemical equilibrium between acids and bases.
Bronsted-Lowry theory: This covers the theory of acids and bases proposed by Bronsted and Lowry.
Lewis theory: This covers the theory of acids and bases proposed by Lewis.
Neutralization reactions: This covers the chemical reaction between an acid and a base that produces a neutral solution.
Salts: This covers the formation of salts from acid-base reactions.
Buffer solutions: This covers the use of buffer solutions to maintain a stable pH.
pH measurement: This covers the devices and techniques used to measure pH.
Acid rain: This covers the effects of acid rain on the environment.
Household acids and bases: This covers the common household acids and bases and their uses.
Organic acids and bases: This covers the acids and bases found in organic compounds.
"Acidic solutions (solutions with higher concentrations of hydrogen (H+) ions) are measured to have lower pH values than basic or alkaline solutions."
"The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution." -OR- "The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution."
"pH = -log(a[H+]) ≈ -log([H+])" (Note: This answer provides the mathematical formula for calculating pH.)
"At 25 °C (77°F), solutions with a pH less than 7 are acidic, and solutions with a pH greater than 7 are basic. Solutions with a pH of 7 at 25 °C are neutral."
"The neutral value of the pH depends on the temperature and is lower than 7 if the temperature increases above 25 °C."
"The pH range is commonly given as zero to 14, but a pH value can be less than 0 for very concentrated strong acids or greater than 14 for very concentrated strong bases."
"The pH scale is traceable to a set of standard solutions whose pH is established by international agreement."
"Primary pH standard values are determined using a concentration cell with transference by measuring the potential difference between a hydrogen electrode and a standard electrode such as the silver chloride electrode."
"The pH of aqueous solutions can be measured with a glass electrode and a pH meter or a color-changing indicator."
"Measurements of pH are important in chemistry, agronomy, medicine, water treatment, and many other applications."
"Measurements of pH are important in chemistry, agronomy, medicine, water treatment, and many other applications."
"Acidic solutions (solutions with higher concentrations of hydrogen (H+) ions) are measured to have lower pH values than basic or alkaline solutions."
"The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution."
"The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution."
"Solutions with a pH of 7 at 25 °C are neutral (i.e., have the same concentration of H+ ions as OH− ions, i.e., the same as pure water)."
"The neutral value of the pH depends on the temperature and is lower than 7 if the temperature increases above 25 °C."
"A pH value can be less than 0 for very concentrated strong acids."
"A pH value can be greater than 14 for very concentrated strong bases."
"The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution."