molar solubility

(noun)

The number of moles of a substance (the solute) that can be dissolved per liter of solution before the solution becomes saturated.

Related Terms

Examples of molar solubility in the following topics:

  • Molar Solubility and Relative Solubility

    • Molar solubility is the number of moles of a solute that can be dissolved per liter of solution before the solution becomes saturated.
    • The relation between the molar solubility and the solubility product means that one can be used to find the other.
    • What is the molar solubility?
    • Compare their molar solubilities in water at 25 °C.
    • Calculate the molar solubility of a compound in water and the relative molar solubility of compounds

  • Effect of a Common Ion on Solubility

    • Adding a common ion decreases the solubility of a solute, causing it to precipitate.
    • With such a small solubility product for CaF2, you can predict its solubility << 0.10 moles per liter.
    • If our prediction is valid, we can simplify the solubility-product equation:
    • Lithium hydroxide forms less-soluble lithium carbonate, which precipitates because of the common ion effect.
    • Calculate the molar solubility of a compound in solution containing a common ion.

  • Complex Ion Equilibria and Solubility

    • Formation of a complex ion between a metal cation and a ligand can increase salt solubility.
    • In this case, square brackets are used to indicate concentration in mol/liter or molarity (M).
    • In this equation, the measured absorbance (A) is related to the molar absorptivity constant (ε), the path length (b), and the molar concentration (c) of the absorbing species.
    • Formation of a chemical complex has an effect on solubility.
    • This will increase the solubility of AgCl in solution.

  • Using Molarity in Calculations of Solutions

    • In chemistry, molar concentration, or molarity, is defined as moles of solute per total liters of solution.
    • The SI unit for molarity is is mol/m3; however, you will almost always encounter molarity with the units of mol/L.
    • This video demonstrates practice problems with molarity, calculating the moles and liters to find the molar concentration.
    • Use molarity to convert between mass and volume in a solution.
    • This video looks at how to use molarity as a conversion factor.

  • Molar Mass of Gas

    • To find the molar mass of a mixture of gases, you need to take into account the molar mass of each gas in the mixture, as well as their relative proportion.
    • The average molar mass of a mixture of gases is equal to the sum of the mole fractions of each gas, multiplied by their respective molar masses:
    • where m is the mass of the gas, and M is the molar mass.
    • Finally, putting the equation in terms of molar mass, we have:
    • What is the molar mass of the gas?

  • Solubility

    • The degree of solubility ranges widely depending on the substances, from infinitely soluble (fully miscible), such as ethanol in water, to poorly soluble, such as silver chloride in water.
    • The solubility of gases displays the opposite relationship with temperature; that is, as temperature increases, gas solubility tends to decrease.
    • In contrast, a non-polar solute such as naphthalene is insoluble in water, moderately soluble in methanol, and highly soluble in benzene.
    • The solubility chart shows the solubility of many salts.
    • The solubilities of salts formed from cations on the left and anions on the top are designated as: soluble (S), insoluble (I), or slightly soluble (sS).

  • Mass-to-Mole Conversions

    • Mass-to-mole conversions can be facilitated by employing the molar mass as a conversion ratio.
    • The compound's molar mass is necessary when converting from grams to moles.
    • For a single element, the molar mass is equivalent to its atomic weight multiplied by the molar mass constant (1 g/mol).
    • For a compound, the molar mass is the sum of the atomic weights of each element in the compound multiplied by the molar mass constant.
    • The molar mass of water is 18 g/mol.

  • Molar Ratios

    • Molar ratios, or conversion factors, identify the number of moles of each reactant needed to form a certain number of moles of each product.
    • From this reaction equation, it is possible to deduce the following molar ratios:
    • These molar ratios can also be expressed as fractions.
    • These molar ratios will be very important for quantitative chemistry calculations that will be discussed in later concepts.
    • Calculate the molar ratio between two substances given their balanced reaction

  • Molar Mass of Compounds

    • The molar mass of a particular substance is the mass of one mole of that substance.
    • The characteristic molar mass of an element is simply the atomic mass in g/mol.
    • However, molar mass can also be calculated by multiplying the atomic mass in amu by the molar mass constant (1 g/mol).
    • The molar mass of NaCl is 58.44 g/mol.
    • This video shows how to calculate the molar mass for several compounds using their chemical formulas.

  • Solid Solubility and Temperature

    • Solubility often depends on temperature; the solubility of many substances increases with increasing temperature.
    • The solubility of a given solute in a given solvent typically depends on temperature.
    • Many salts show a large increase in solubility with temperature.
    • Some solutes exhibit solubility that is fairly independent of temperature.
    • A useful application of solubility is recrystallizaton.