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Salts contains ions that may affect the pH in aqueous solutions in both acidic and basic directions.
It is possible to predict whether an aqueous solution of a salt with both basic and acidic properties will be basic, acidic or neutral by comparing the K
a value for the acidic ion with the K b value for the basic ion.
See also Strong and weak acids and bases and Buffer solutions, as well as pKa of inorganic acids and bases, pKa of phenols, alcohols and carboxylic acids and pKa of amines, diamines and cyclic organic nitrogen compounds.
Acid vs. Basic Ion
K a vs K b
Basic or acidic
a > K b < 7
a < K b > 7
a = K b 7
This table summarizes the acid-base properties of aqueous solutions of various salts:
For full table -
rotate the screen!
Aqueous Salt Solutions - Acid and Base Properties
Type of salt
pH of solution
BaCl 2, KCl, CaNO 3, Na 2SO 4
Neither acts as an acid or a base
NaF, KCHOO, NaHCO 3
Anion acts as a base Cation has no effect on pH
Conjugate acid of weak base
NH 4Br, NH 4NO 3,
Cation acts as an acid Anion has no effect on pH
Conjugate acid of weak base
Conjugate base of weak acid
NH 4CN, NH 4CH 3COO
Acidic if Ka > Kb Basic if Kb > Ka Neutral if Ka = Kb
Cation acts as an acid Anion acts as a base
Highly charged metal ion
Al(NO 3) 3, CrCl 3
Hydrated cations acts as an acid Anions has no effect on pH
Material properties of gases, fluids and solids - densities, specific heats, viscosities and more.
pH range vs. color change for acid and base indicators - together with pKa and structures of the indicators.
pH values of acids like sulfuric, acetic and more..
Molweight, melting and boiling point, density, pKa-values, as well as number of carbon and hydrogen atoms in molecules are given for 150 different alcohols and acids.
Values for the negative logarithm of the acid dissociation constant, pKa, of the conjugated acid of amines, diamines and cyclic organic nitrogen compounds, shown together with the molecular structure of the acids.
pH values for bases like sodium hydroxide, ammonia and more.
Definitions, explanations and examples of how to make buffer solutions.
Values for the negative logarithm of the acid dissociation constant, pKa, of inorganic acids and bases, as well as hydrated metal ions.
For oxygen containing organic compounds this is given: pKa (the negative logarithm of the acid dissociation constant), molecular structures, molar weights, density and melting and boiling points.
The most common strong acids and bases, and some examples of weak acids and bases, together with definition of strong and weak acids and bases.
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