ANACHEM

• Analysis


  The process of determining the level of any or all components in a material system
• Analytical Science


  The science that deals with the identification and quantification of the components of material systems
• Qualitative Analysis


  • An analysis that establishes the chemical identity of the species
• Analytical Chemistry


  A branch of chemistry that deals with the separation, identification, and quantification of chemical compounds
• Quantitative Analysis


  • An analysis that determines the relative amounts of analytes in numerical terms
• Analytical Strategy


  The process involving many individual steps by which an analyte's identity or concentration in a sample is determined
• Scientific Notation


  A numerical system in which numbers are expressed in the form A x 10^n where A is a number with a single nonzero digit to the left of the decimal place and n is a whole number. The exponent for the exponential term is equal to the number of places the decimal point has been moved. Positive (+) n means a large number so the decimal moves to the right by n places. Negative (-) n means a small number so the decimal moves to the left by n places
• Prefixes for Units

  • giga- (G) - 10^9
  • mega- (M) - 10^6
  • kilo- (K) - 10^3
  • deci- (d) - 10^-1
  • centi- (c) - 10^-2
  • milli- (m) - 10^-3
  • micro (µ) - 10^-6
  • nano- (n) - 10^-9
  • pico- (p) - 10^-12
• Fundamental Units of Measurement


  • Mass: Kilogram (kg)
  • Length: Meter (m)
  • Time: Second (s)
  • Temperature: Kelvin (K)
  • Amount of Substance: Mole (mol)
  • Electric current: Ampere (A)
  • Luminous intensity: Candela (cd)
• # of spaces moved by decimal = exponent
• Positive (+) n means a large number so the decimal moves to the right by n places
• Exponent = # of spaces to be moved by decimal
• Scientific notation to standard notation

  • 8.0123698 x 10^5 -> 801236.98
  • 5.08 x 10^-5 -> 0.0000508
• Negative (-) n means a small number so the decimal moves to the left by n places
• Standard notation to scientific notation

  • 801236.98 -> 8.0123698 x 10^5
  • 0.0000508 -> 5.08 x 10^-5
• Significant Figures

  • 0.0141 has three significant figures
  • 3.063 has four significant figures
  • 0.001004 has four significant figures
  • 56.00 has four significant figures
  • 0.05050 has four significant figures
  • 59,000,000 has two significant figures
  • 6010 has three significant figures
• Converting from scientific notation to standard notation

  1. If the exponent is positive, you will have a large number (>1) and move the decimal to the right

  2. If the exponent is negative, you will have a small number (<1) and move the decimal to the left
• Solution Properties: A substance that is d
• In measurements, there is always some amount of uncertainty
• Term is equal to the number of places the decimal point has been moved
• Converting from standard notation to scientific notation

  1. If the number is one or greater, you will have a positive exponent and move the decimal to the left

  2. If the number is less than one, you will have a negative exponent and move the decimal to the right
• Percent solutions


  • Weight/Volume (w/v) % solutions
  • Volume/Volume % solutions
  • Weight/weight (w/w) % solutions
• Weight/weight (w/w) % solutions

  • weight of solute / weight of solution x 100
• Examples of significant figures

  • 59,000,000 has two significant figures
  • 6010 has three significant figures
• Decimal point is PRESENT in the number
• Molality (m)


  Expressed as the amount of solute per 1 kg of solvent
• Relationship between Molarity and Normality

  • Normality = molarity x valence
  • Molarity = Normality / valence
• Weight/Volume (w/v) % solutions

  • weight of solute (g) / volume of solution (mL) x 100
• Normality (N)


  Number of equivalent weight per 1 liter of solution
• Zeros at the end of a number are NOT SIGNIFICANT if the number LACKS an explicitly shown decimal point
• Molarity (M)


  • Expressed as the number of moles per 1 L of solution
  • A 1.0 M solution contains 1.0 mole of solute per liter of solution
• Examples of significant figures

  • 56.00 has four significant figures
  • 0.05050 has four significant figures
• Volume/Volume % solutions

  • volume of solute / volume of solution x 100
• Solution Properties

  • A substance that is dissolved in a liquid is called a solute
  • The liquid in which the solute is dissolved is the solvent
  • Together they represent a solution
• Systematic error


  Error that occurs predictably once a pattern of recognition is established; predictable errors of the same sign and magnitude
• Standard deviation

  A measure of dispersion of a group of values around the mean
• Coefficient of variation

  The SD divided by mean expressed as a percentage
• Random error


  Error that occurs unpredictably due to poor precision
• Accuracy


  How closely a measure value agrees with a true or expected value
• Statistical calculations


  Mathematical methods used to analyze data