Name: strong acids, strong bases, and ph
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 22 s
Channel: JoVE

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Strong Acid and Base Solutions

Strong acids dissociate completely in water. For example, nitric acid dissociates completely into hydronium ions and nitrate ions. As the hydronium ions generated from the autoionization of water are negligible, the concentration of the hydronium ions in water is equal to the concentration of the strong acid.
The pH of these solutions can be determined using the initial concentration of the strong acid.
For example, in a 0.10 molar HCl solution, HCl will dissociate completely into the hydronium ions and chloride ions, and therefore the hydronium ion concentration of the solution will also be 0.10 molar. By taking the negative logarithm of this concentration, the pH of the solution is equal to one.
Conversely, the pH of a solution can be used to determine the hydronium ion concentration of a solution. For example, for a solution of pH 3.60, its hydronium ion concentration can be determined by solving the equation 3.60 is equal to the negative log of the hydronium ion concentration.
To solve for the concentration, multiply both sides by negative one, and then take the antilog of both sides. The hydronium ion concentration equals 2.5 times ten to the negative four molar.
Strong bases that are group one metal hydroxides, like sodium hydroxide and potassium hydroxide, dissociate completely into solution. For example, 0.20 molar sodium hydroxide will dissociate completely in water and produce 0.20 molar sodium ions and 0.20 molar hydroxide ions.
However, group two metal hydroxides, like barium hydroxide and calcium hydroxide, produce two moles of hydroxide ions for each mole of base. For example, 0.020 molar calcium hydroxide will dissociate completely in water and will produce 0.020 molar calcium ions and 0.040 molar hydroxide ions.
Ionic metal oxides, like sodium oxide and calcium oxide, are also strong bases. Their oxide ion reacts with water and produces hydroxide ions.
The concentration of hydroxide ions can be used to calculate a pOH and pH of the solution. For example, a five times ten to the negative five molar potassium hydroxide solution has an equal amount of hydroxide ions as strong base and therefore has a pOH of 4.30.
Like pH, a pOH of the solution can also be used to determine hydroxide ion concentration by solving the equation: pOH equals the negative log of the hydroxide ion concentration.
Since pH plus pOH is equal to 14 and the pOH is 4.3, the pH of the solution is 9.7.

strong acid and base solutions

A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
<img alt="Blackbody radiation formula derivation, equations and symbols, physics diagram." src="/files/ftp_upload/11399/11399_Equation_1.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Static equilibrium diagram, &#931;Fx=0, depicting forces and moments for structural analysis." />
On the other hand, a strong base is a compound that dissociates completely in an aqueous solution and produces hydroxide ions. For example, 0.015 M KOH, a group 1 metal hydroxide, will dissociate completely and produce 0.015 M of OH- and 0.015 M of K+.
<img alt="Equilibrium of rigid bodies diagram, illustrating &#931;Fx=0, torque equations, structural analysis." src="/files/ftp_upload/11399/11399_Equation_2.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Static equilibrium diagram; &#931;Fy=0, &#931;Fx=0; demonstrates force balance with force vectors and angles." />
Group 2 metal hydroxides, like barium hydroxide [Ba(OH)2] and strontium hydroxide [Sr(OH)2], are also strong bases and possess two hydroxide ions. This causes them to produce a more basic solution compared to NaOH or KOH at the same concentration. For example, 0.015 M Ba(OH)2 produces 0.015 M Ba+ and 0.030 M hydroxide.
<img alt="Titration setup diagram with burette, beaker, and reaction equation in acid-base chemistry." src="/files/ftp_upload/11399/11399_Equation_3.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Dynamic pressure equation: Bernoulli&#8217;s principle diagram with fluid flow; visualizes physics concepts." />
As strong acids and bases dissociate completely, molar ratios can be used to determine their hydronium and hydroxide concentrations, which in turn can be used to calculate the pH or pOH of a solution. For example, a 0.030 M HCl solution will produce 0.03 M hydronium ions. Therefore the pH of this solution will be
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The pOH of the same solution can be determined using the formula
<img alt="Chromatography process: analyte retention time in column; result analysis diagram." src="/files/ftp_upload/11399/11399_Equation_5.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="DNA structure diagram with nucleotide bases, illustrating gene sequence and molecular components." />
As the pH of the solution is 1.52, its pOH can be calculated as
<img alt="Double-slit experiment diagram, interference pattern, wave-particle duality principle." src="/files/ftp_upload/11399/11399_Equation_6.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="mRNA transcription process, DNA to RNA conversion, diagram, genetic expression overview, biology concept." />
Similarly, the concentration of hydroxide ions produced by strong bases can be used to determine the pOH of a solution using the equation
<img alt="Static equilibrium, &#931;Fx=0, force vector diagram, illustrating free body force analysis, mechanics." src="/files/ftp_upload/11399/11399_Equation_7.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="DNA sequencing; GCTGAACGTATC base sequence; alignment diagram; genetic analysis process." />
The above equation can also be used to determine the hydroxide ion concentration when pOH is known. For example, if the pOH of a solution is 3.00,
<img alt="Chemical reaction mechanism diagram shows electrophilic addition of HBr to propene." src="/files/ftp_upload/11399/11399_Equation_8.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Neutralization reaction equation diagram: HCl(aq) + NaOH(aq) &#8594; NaCl(aq) + H2O(l)." />
Multiplication of both sides by &#8722;1 gives
<img alt="Static equilibrium equations &#931;Fx=0, diagram with forces, balancing physics concepts." src="/files/ftp_upload/11399/11399_Equation_9.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Capillary electrophoresis schematic with DNA separation apparatus and voltage application process." />
Now, take the antilog of both sides
<img alt="Chromatography: Thin Layer, Rf Values, Stationary Phase, Solvent Front, Organic Compound Separation." src="/files/ftp_upload/11399/11399_Equation_10.png" style="height: 90px;" data-altupdatedat="1754904545000" data-alt="E=mc&#178; equation, formula for mass-energy equivalence theory, diagram for educational use." />
Thus, the hydronium ion concentration of the solution with pOH 3 is 1.0 &#215; 10&#8722;3 M. A similar method can be used to determine the hydronium ion concentration of a solution if its pH is known.

A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial ...

Education

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Acids and Bases

KEY TERMS AND CONCEPTS

strong acids, strong bases, and ph

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio.

For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates completely. It produces 0.015 M OH- and 0.015 M K+.

Some group 2 metal hydroxides are also strong bases. Barium hydroxide, Ba(OH)2, and strontium hydroxide, Sr(OH)2, each contain two hydroxide ions. That means they create a more basic solution than NaOH or KOH at the same concentration. For example, 0.015 M Ba(OH)2 produces 0.015 M Ba+ and 0.030 M hydroxide.

The ion concentrations from strong acids and strong bases can be used to calculate pH and pOH. A 0.030 M HCl solution produces 0.03 M hydronium ions, so its pH can be found from that concentration. The same pH value can then be used to determine pOH. If the pH is 1.52, the pOH can be calculated from the relationship between them.

The same idea works for strong bases. The hydroxide ion concentration can be used to find pOH with the equation for pOH, and the equation can also be used in reverse when pOH is known. For example, if the pOH of a solution is 3.00, multiplying by -1 and taking the antilog gives a hydronium ion concentration of 1.0 × 10^-3 M. The same method can be used to find hydronium ion concentration when pH is known.

Strong Acids, Strong Bases, and pH

bronsted-lowry acids and bases

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...

water: a bronsted-lowry acid and base

Water as an Amphiprotic Substance

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 scale

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...

relative strengths of conjugate acid-base pairs

relative-strengths-of-conjugate-acid-base-pairs

How Ka and Kb Show Acid-Base Strength

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...

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

weak base solutions

Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

mixtures of acids

pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

ions as acids and bases

Salt Hydrolysis and pH of Solutions

Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

determining the ph of salt solutions

Salt Hydrolysis and pH in Solutions

Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

acidbase-strengths-and-dissociation-constants

Acid and Base Strength in Water

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

acid strength and molecular structure

How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

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 strong acids and strong bases dissociate completely in water and how their ion concentrations are used to calculate pH and pOH.

Strong Acids, Strong Bases, and pH | JoVE K12

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Strong Acids, Strong Bases, and pH

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