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    Slide 1

    Calculations Used in AnalyticalChemistry

    Chapter 4

    Slide 2

    Topics

    International System of Units / SI Units

    Mass and Weight

    The Mole

    Units of Concentrations of solutions

    Stoichiometry

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    Slide 3

    Seven SI BASE UNITS

    Table 4-1, p.72

    Derived units:All other units can be derived from the seven base units

    Slide 4

    Examples of Derived Units

    1 Joule=?

    1 Newton=?

    1 volt=?

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    Slide 5 Table 4-1, p.72

    Slide 6

    Mass and Weight

    Mass (m): invariantmeasure of amount ofmatter

    Weight

    g: acceleration due togravity

    p.73

    mgw =

    mgw =

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    Slide 7

    Calculating moles from massFactor Label Method Review

    Mass of TRIS that will reactwith 35 mL of 0.1 M HCl.

    Moles of HCl in 35 mL

    mol HCl = VHCl x MHCl=

    Moles of TRIS

    Mass of TRIS

    mol TRIS x molar mass TRIS

    molHCl

    molTRISmolHClnTRIS

    1

    1# =

    molTRIS

    gTRISmolTRISmTRIS

    1

    14.121# =

    Use the factor label method : Prelab of Experiment 3

    Slide 8

    The Mole

    Mole (mol): SI unit for the amount of achemical species

    1 mole = 6.022 x 1023 particles

    Molar mass: mass (in g) of one mole

    Calculating molar masses using EXCEL(Chapter 3, p 60-67).

    Importing data from Web Pages

    Dealing with Character Strings (FINDfunction, MID function)

    Using VLOOKUP to locate Data in aWorksheet

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    Slide 9

    Solutions and their Concentrations

    Analytical molarity Equilibrium molarity

    Percent concentration

    Parts per Million/Billion

    P-Functions or p-value

    Slide 10

    Solutions and their Concentrations Analytical molarity

    Total number of moles of a solute in 1L of the

    solution (according to recipe).

    Example: NaCl, Na2SO4

    Equilibrium molarity

    Molar concentration of a given species insolution

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    Slide 11

    Percent Concentrations

    %100,

    ,)/(/

    %100)/(

    %100)/(

    =

    =

    =

    mLsolutionvolume

    gsoluteweightvwpercentvolumeweight

    solutionvolume

    solutevolumeVVpercentVolume

    solutionweight

    soluteweightwwpercentweight

    Slide 12 Fig 4-1, p.82

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    Slide 13

    Density and Specific Gravity of Solutions

    Density of a substance is its mass per unitvolume

    Specific gravity: ratio of mass of substance tothe mass of equal volume of water at 4C.

    When using the metric system density andspecific gravity can be used interchangeably,

    because the density of water is approximately1.00 g/mL

    Slide 14

    From % w/w to mol/L solution

    36.5 % HCl

    FW = 36.46

    Specific gravity = 1.18

    ML

    ml

    mL

    g

    gSgHCL

    molHClgHCl

    Ls

    molcHCl 8.11

    1

    1000

    00.1

    18.1

    ln100

    1

    46.36

    15.36

    ln==

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    Slide 15 Table 4-3, p.82

    Slide 16

    Back to Concentrations: Parts Per Million,

    Parts per Billion For very dilute solutions, it is convenient to express

    concentrations in ppm or ppb

    An approximation that is commonly used is that thedensity of dilute solution approaches the density ofwater (1.00 g/ml)

    ppbsolutionmasssolutemassc

    ppmsolutionmass

    solutemassc

    ppb

    ppm

    9

    6

    10

    10

    =

    =

    Units in numerator and denominator must be consistent!

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    Slide 17

    Back to Concentrations:p-functions or p-values

    The p-value is the negative log (base 10) of themolar concentration

    P-values are convenient to use when changesoccur over several orders of magnitude

    [H+], pH

    [Ba2+], pBa

    [Cl-], pCl

    [Cl-]=2.45 x 10-5M

    pCl=4.6108= 4.61?

    Slide 18 Fig 4-2, p.84

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    Slide 19

    Stoichiometric Calculations

    Problem 4-36

    What mass of MgNH4PO4 precipitated when 200.00 mL of a

    1.000% (w/v) solution of Mg Cl2 were treated with 40.0 mL of0.1753 M Na3PO4 and an excess of NH4

    +? What was themolarity of the excess reagent (Na3PO4 or MgCl2) after the

    precipitation was complete?

    Steps

    Write chemical equation and balance it

    Calculate moles of reagents mixed

    Determine the limiting reagent

    Calculate mass of precipitate

    Calculate moles of unreacted reagent

    Calculate concentration of unreacted reagent

    Slide 20

    Stoichiometry

    Problem 4-6:

    How many K ions are contained in 6.76 mol ofK3PO4?

    1.22 x 1025 K+.

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    Slide 21

    Dilution Factors

    Problem 4-30 Describe the preparation of 1.50 mL of 0.215 M NaOHfrom the concentrated commercial reagent [50% NaOH(w/w)]. Specific gravity = 1.525

    50 % NaOH (w/w) = 19.06 M

    Volume NaOH 50% (w/w) required = 16.9 mL