CHEM

• Concentrated


  The amount of solute is relatively high
• Concentration Units


  • Percent by Mass
  • Percent by Volume
  • Mole Fraction
  • Molality
  • Molarity
  • Parts per Million
• Percent by mass (%) = (mass of solute / total mass) x 100%
• Mole fraction (Xi) = (number of moles of i / total number of moles)

  
• Percent by volume (% v/v) = (volume of solute / total volume) x 100%
• Molality (m) = (number of moles of solute / kg solvent)
• Parts per million (ppm) = (number of parts of solute / 1,000,000 parts of solution)
• Molarity (M) = (number of moles of solute / liters solution)
• Solutions are homogeneous mixtures that have uniform composition throughout the mixture.
• Stoichiometry is the quantitative relationship between reactants and products.
• Normality (N) = (equivalents of solute / liter solution)
• The concentration of a solution is determined by dividing the amount of solute present by the volume of the solution.
• The law of conservation of matter states that matter cannot be created or destroyed.
• The law of conservation of mass states that matter cannot be created or destroyed during chemical reactions.
• Mass percent = (mass of solute / mass of solution) x 100%
• A balanced equation shows equal numbers of atoms on both sides of an equation.
• Concentration can be expressed as mass percent, mole fraction, molality, ppm, or molarity.
• Concentration can be expressed as mass/volume or mole/volume.
• Homogenous mixture - A substance composed of two or more substances mixed together so thoroughly that they appear to have no visible boundaries between them.
• Stoichiometry refers to the quantitative relationships between the amounts of substances involved in a reaction.
• Atomic number = # protons + # neutrons
• Chemical equations are used to represent chemical reactions, with reactants shown on the left side and products on the right side separated by an arrow.
• A balanced equation shows equal numbers of atoms on both sides, while an unbalanced equation does not have equal numbers of atoms on both sides.
• Stoichiometry refers to the quantitative relationships between reactants and products in chemical reactions.
• Limiting reagent is the substance whose moles run out first when all reactants have been consumed.
• Chemical equations are used to represent chemical changes, with reactants listed above the arrow and products below it.
• An unbalanced equation does not have equal numbers of atoms on both sides of the equation.
• Heterogenous mixture - A substance made up of two or more different types of particles which do not mix well together.
• Solutions are homogeneous mixtures with uniform composition throughout the mixture.
• In a chemical reaction, the total amount of matter remains constant but changes its composition.
• Balancing chemical equations involves adjusting the coefficients until both sides contain equal numbers of each type of atom.
• The coefficients in front of formulas indicate how many atoms of each element are present in one formula unit.
• The periodic table is organized by increasing atomic number (proton count).
• The law of conservation of matter states that matter cannot be created nor destroyed, only transformed from one form into another.
• Isotopes are different forms of the same element with the same atomic number but different mass numbers.
• Colloid - A heterogeneous mixture where the dispersed phase is larger than 1 nm but smaller than 1 micrometer.
• Mass is conserved during a chemical reaction.
• In a chemical reaction, the total mass of all elements present at the beginning is equal to the total mass of all elements present at the end.
• Colloid - A heterogeneous mixture where the dispersed phase is larger than 1 nm but smaller than 1 micrometer.
• Mass number = # protons + # neutrons