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Study Notes

pH: A Measure of Acidity or Basicity of Aqueous Solutions

pH is a scale used to specify the acidity or basicity of an aqueous solution.
The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution.
Acidic solutions have lower pH values than basic or alkaline solutions.
Solutions with a pH less than 7 are acidic, solutions with a pH greater than 7 are basic, and solutions with a pH of 7 are neutral.
The 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.
pH values can be measured with a glass electrode and a pH meter or a color-changing indicator.
The first electronic method for measuring pH was invented by Arnold Orville Beckman in 1934.
pH is defined as the decimal logarithm of the reciprocal of the hydrogen ion activity, aH+.
The pH scale ranges from 0 to 14, with a pH of 7 indicating neutrality, values less than 7 indicating acidity, and values greater than 7 indicating basicity.
pH can be measured using indicators, which change color depending on the pH of the solution they are in.
pH values can be measured in non-aqueous solutions, but they are based on a different scale from aqueous pH values.pH Scale: Definition, Applications, and Calculations
The pH scale is a measure of acidity or basicity of an aqueous solution.
The pH scale ranges from 0 to 14, with 7 being neutral.
The unified absolute pH scale is a new approach to measuring pH, based on the absolute chemical potential of the proton.
The measurement of pH can become difficult at extremely acidic or alkaline conditions, such as below pH 2.5 or above pH 10.5.
In living organisms, the pH of various body fluids, cellular compartments, and organs is tightly regulated to maintain a state of acid-base balance known as acid–base homeostasis.
The pH of seawater is typically limited to a range between 7.4 and 8.5, and there is evidence of ongoing ocean acidification caused by carbon dioxide emissions.
Strong acids and bases are compounds that are essentially fully dissociated in water.
Weak acids and bases can be treated using the formalism of acid dissociation constant.
Water itself is a weak acid and a weak base and must be taken into account at high pH and low solute concentration.
The pH of a solution is defined as the negative logarithm of the concentration of H+, and the pOH is defined as the negative logarithm of the concentration of OH-.
When calculating the pH of a solution containing acids and/or bases, a chemical speciation calculation is used to determine the concentration of all chemical species present in the solution.
The United States Department of Agriculture Natural Resources Conservation Service classifies soil pH ranges based on soil parent material, erosional effects, climate, and vegetation.Calculating pH Using Equilibrium Constants
The pH of a solution can be calculated using equilibrium constants.
The concentration of hydrogen ions (H+) can be calculated using the ionization constant (Kw) of water, which is 10^-14 M^2 at 25°C.
The general method for calculating pH involves writing mass-balance equations for each reagent in the system, which includes equilibrium constants.
There are three non-linear simultaneous equations in the three unknowns [A], [B], and [H], which can be solved using computer programs.
This method is applicable to systems with multiple reagents or when many complexes are formed.
Polyprotic acids are also amenable to spreadsheet calculations.
Stability constants are defined as a quotient of concentrations, not activities.
Activities are used when more complicated expressions are required.
The calculation of hydrogen ion concentrations is a key element in determining equilibrium constants by potentiometric titration.
The concentration of hydroxide ions (OH-) can also be calculated using the ionization constant of water.
The pH of a solution can be used to calculate the concentration of many other species in the solution.
Computer programs are available to perform these calculations.

Description

Do you know what pH is and how it is measured? Test your knowledge with our quiz on pH: A Measure of Acidity or Basicity of Aqueous Solutions. Learn about the pH scale, the history of pH measurement, and how to calculate pH using equilibrium constants. This quiz will challenge your understanding of pH and its applications in various fields. Don't miss the chance to improve your knowledge on this fundamental concept in chemistry.