Name: ph and poh in water
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 41 s
Channel: JoVE

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pH Scale

The concentration of hydronium ions in an aqueous solution is usually written with negative exponents and can be as small as 1 &#215; 10&#8722;14 M. The pH scale was developed by chemist Soren Sorenson in 1909 as a more convenient way to quickly compare the acidity of different solutions.
The pH of a solution is the negative logarithm of its hydronium ion concentration. For example, a solution with 1 &#215; 10&#8722;5 M hydronium concentration has a pH of 5. The greater the hydronium ion concentration of a solution, the lower its pH.
As pH is expressed on a logarithmic scale, a single-unit change corresponds to a 10-fold increase or decrease of the hydronium ion concentration. A solution with a pH of 3 will have ten times more hydronium ions than a solution with a pH 4 and one hundred times more than a solution with a pH of 5.
An acidic solution has a higher concentration of hydronium ions than hydroxide ions and a pH less than 7, whereas a basic solution has a lower concentration of hydronium ions than hydroxide ions and a pH greater than 7.
A neutral solution with an equal concentration of hydronium and hydroxide ions has a pH of 7.
The concentration of hydroxide ions can also be expressed as pOH. pOH is the negative logarithm of the hydroxide ion concentration. The higher the hydroxide ion concentration, the lower its pOH value.
A pH or pOH value of an aqueous solution ranges from 0 &#8211; 14. This is because KW, the equilibrium constant for the autoionization of water, is equal to 1 &#215; 10&#8722;14. 
Taking the negative log of both sides of the equation results in an equation where pKW is equal to the sum of pH and pOH. Since the negative log of 1 &#215; 10&#8722;14 is 14, the sum of the pH and pOH of an aqueous solution will always be 14. This can be used to determine the pH value when the pOH value is known and vice versa.
For example, a solution with a pOH of 10 has a pH of 4.

ph scale

Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution&#8217;s properties and the chemical behaviors of its other solutes. Two different solutions can differ in their hydronium or hydroxide ion concentrations by a million, billion, or even trillion times. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. The pH of a solution is therefore defined as shown here, where [H3O+] is the molar concentration of hydronium ion in the solution:
 <img alt="Hammett equation diagram for electronic effects analysis, featuring resonance and inductive symbols." src="/files/ftp_upload/11397/11397_Equation_1.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Chemical structure of paracetamol molecule, illustrating atomic bonds, planar conformation." />
Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression:
 <img alt="Static equilibrium concept with &#931;Fx=0, &#931;Fy=0 diagram, showing forces, moments, support reactions." src="/files/ftp_upload/11397/11397_Equation_2.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Thermal cycle diagram showing Brayton cycle stages and state points labeled in flow process chart." />
Likewise, the hydroxide ion molarity may be expressed as a p-function or pOH:
 <img alt="Chemical reaction mechanism: aromatic nitration, electrophilic substitution diagram with nitrogen dioxide." src="/files/ftp_upload/11397/11397_Equation_3.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Static equilibrium diagram with &#931;Fx=0 and MA=0; force vectors, beam, pivot point shown." />
or
 <img alt="DNA sequence diagram with nucleotide symbols A, T, C, G in gene editing context for educational use." src="/files/ftp_upload/11397/11397_Equation4.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Vapor-liquid equilibrium diagram; isotherm, pressure-composition; distillation analysis." />
Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the KW expression:
 <img alt="Linear static equilibrium diagram with forces, &#931;Fx=0, &#931;Fy=0, illustrating balance of forces." src="/files/ftp_upload/11397/11397_Equation_5.png" style="height: 135px;" data-altupdatedat="1754904545000" data-alt="Chromatography system diagram; protein purification process; shows elution column and analyte flow." />
At 25 &#176;C, the value of KW is 1.0 &#215; 10&#8722;14, and so:
 <img alt="Fractional distillation apparatus diagram; separating liquid mixtures by heating and condensation." src="/files/ftp_upload/11397/11397_Equation_6.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Static equilibrium equations diagram with &#931;Fx=0, &#931;Fy=0, MA=0 for educational research use." />
The hydronium ion molarity in pure water (or any neutral solution) is 1.0 &#215; 10&#8722;7 M at 25 &#176;C. The pH and pOH of a neutral solution at this temperature are therefore:
 <img alt="Polysaccharide structure, glycogen molecule diagram, branching glucose units for energy storage exploration." src="/files/ftp_upload/11397/11397_Equation_7.png" style="height: 95px;" data-altupdatedat="1754904545000" data-alt="Static equilibrium equations diagram with forces &#931;Fx=0, &#931;Fy=0, moment MA=0 for analysis." />
And so, at this temperature, acidic solutions are those with hydronium ion molarities greater than 1.0 &#215; 10&#8722;7 M and hydroxide ion molarities less than 1.0 &#215; 10&#8722;7 M (corresponding to pH values less than 7.00 and pOH values greater than 7.00). Basic solutions are those with hydronium ion molarities less than 1.0 &#215; 10&#8722;7 M and hydroxide ion molarities greater than 1.0 &#215; 10&#8722;7 M (corresponding to pH values greater than 7.00 and pOH values less than 7.00).
Since the autoionization constant KW is temperature dependent, these correlations between pH values and the acidic/neutral/basic adjectives will be different at temperatures other than 25 &#176;C. For example, the hydronium molarity of pure water at 80&#176;C is 4.9 &#215; 10&#8722;7 M, which corresponds to pH and pOH values of:
 <img alt="Chemical equilibrium graph; reaction equation aA + bB &#8596; cC + dD; concentration changes." src="/files/ftp_upload/11397/11397_Equation_8.png" style="height: 95px;" data-altupdatedat="1754904545000" data-alt="Chomsky hierarchy diagram illustrating formal grammar classification and language hierarchy." />
At this temperature, neutral solutions exhibit pH = pOH = 6.31, acidic solutions exhibit pH less than 6.31 and pOH greater than 6.31, whereas basic solutions exhibit pH greater than 6.31 and pOH less than 6.31. This distinction can be important when studying certain processes that occur at other temperatures, such as enzyme reactions in warm-blooded organisms at a temperature around 36 &#8211; 40 &#176;C. Unless otherwise noted, references to pH values are presumed to be those at 25 &#176;C.
This text is adapted from<a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"> Openstax, Chemistry 2e, Section 14.2: pH and pOH.</a>

Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as ...

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Acids and Bases

KEY TERMS AND CONCEPTS

ph and poh in water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down.

Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w relationship.

At 25 °C, K w is 1.0 × 10−14. In pure water, or any neutral solution at this temperature, the hydronium ion concentration is 1.0 × 10−7 M. That gives pH = 7.00 and pOH = 7.00.

At 25 °C, acidic solutions have hydronium ion concentrations greater than 1.0 × 10−7 M and hydroxide ion concentrations less than 1.0 × 10−7 M. This means acidic solutions have pH values below 7.00 and pOH values above 7.00. Basic solutions show the opposite pattern, with pH above 7.00 and pOH below 7.00.

The link between pH and acidity changes with temperature because K w changes with temperature. For example, pure water at 80 °C has a hydronium ion concentration of 4.9 × 10−7 M, which gives pH and pOH values of 6.31. At this temperature, neutral solutions have pH = pOH = 6.31, acidic solutions have pH below 6.31, and basic solutions have pH above 6.31.

This temperature effect matters in processes that happen away from 25 °C, including enzyme reactions in warm-blooded organisms at about 36–40 °C. Unless another temperature is stated, pH values are usually assumed to refer to 25 °C.

pH and pOH in Water

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Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

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Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

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Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

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determining the ph of salt solutions

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acid/base strengths and dissociation constants

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Acid and Base Strength in Water

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lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how hydronium and hydroxide ion levels define pH and pOH, why neutral water changes with temperature, and how acidic or basic solutions are identified.

pH and pOH in Water | JoVE K12

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pH and pOH in Water

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