liter

(noun)

A non-SI metric system unit of volume equal to 1 cubic decimeter (dm3), 1,000 cubic centimeters (cm3) or 1/1,000 cubic meter (m3)

Related Terms

Examples of liter in the following topics:

  • Using Molarity in Calculations of Solutions

    • In chemistry, molar concentration, or molarity, is defined as moles of solute per total liters of solution.
    • The reason for this is because one liter of solution usually contains either slightly more or slightly less than 1 liter of solvent, due to the presence of the solute.
    • What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters of solution?
    • Molarity is a measurement of concentration, with units of mol solute per liter solution.
    • Also, molarity is a ratio that describes the moles of solute per liter of solution.

  • Molarity

    • In chemistry, concentration of a solution is often measured in molarity (M), which is the number of moles of solute per liter of solution.
    • A solution that contains 1 mole of solute per 1 liter of solution (1 mol/L) is called "one Molar" or 1 M.
    • To calculate the molarity of a solution, the number of moles of solute must be divided by the total liters of solution produced.
    • The volume does not need to be converted to liters yet because both sides of the equation use mL.
    • Notice that all of the units for volume have been converted to liters.

  • Gas Stoichiometry

    • Shows how to use stoichiometry to convert from grams of a gas to liters of a gas.

  • Properties of Oxygen

    • At 25 °C and 1 standard atmosphere (101.3 kPa) of air, freshwater contains about 6.04 milliliters (mL) of oxygen per liter, whereas seawater contains about 4.95 mL per liter.
    • At 5 °C the solubility increases to 9.0 mL (50 percent more than at 25 °C) per liter for water and 7.2 mL (45 percent more) per liter for sea water.

  • 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.
    • Molar solubility, which is directly related to the solubility product, is the number of moles of the solute that can be dissolved per liter of solution before the solution becomes saturated.
    • The units are molarity (M), or mole liter-1 (mol/L).

  • Effect of a Common Ion on Solubility

    • With such a small solubility product for CaF2, you can predict its solubility << 0.10 moles per liter.
    • The 2s term is << 0.10 moles per liter, and therefore:

  • Calculating Changes in a Buffer Solution

    • Calculate the change in pH when 0.001 mole of hydrochloric acid (HCl) is added to a liter of solution, assuming that the volume increase upon adding the HCl is negligible.
    • Compare this to the pH if the same amount of HCl is added to a liter of pure water.
    • What is the pH if 0.0020 M of solid sodium hydroxide (NaOH) is added to a liter of buffer?

  • Molecular Geometries

    • Tetra- signifies four, and -hedral relates to a face of a solid; "tetrahedral" literally means "having four faces. " This shape is found when there are four bonds all on one central atom, with no lone electron pairs.
    • Octa- signifies eight, and -hedral relates to a face of a solid, so "octahedral" literally means "having eight faces."

  • UV-Visible Absorption Spectra

    • (where A= absorbance, c = sample concentration in moles/liter & l = length of light path through the sample in cm. )
    • If the isoprene spectrum below was obtained from a dilute hexane solution (c = 4 * 10-5 moles per liter) in a 1 cm sample cuvette, a simple calculation using the above formula indicates a molar absorptivity of 20,000 at the maximum absorption wavelength.

  • Predicting the Direction of a Reaction

    • Example 1: If 1.0 x 10-2 moles of hydrogen gas and 1.0 x 10-2 moles of iodine gas are placed in a 1-liter flask at 448 °C with 2.0 x 10-3 moles of HI , will more HI be produced?