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![Page 1: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/1.jpg)
Principles of Analytical Chemistry (F13I11)
Recommended textbook:“Fundamentals of Analytical Chemistry”Skoog, West and Holler, 7th Ed., 1996
(Saunders College Publishing)
![Page 2: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/2.jpg)
Applications of Analytical Chemistry
Industrial Processes: analysis for quality control, and “reverse engineering”
(i.e. finding out what your competitors are doing).
Environmental Analysis: familiar to those who attended the second year
“Environmental Chemistry” modules. A very wide range of problems and
types of analyte
Regulatory Agencies: dealing with many problems from first two.
Academic and Industrial Synthetic Chemistry: of great interest to many of my
colleagues. I will not be dealing with this type of problem.
![Page 3: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/3.jpg)
The General Analytical Problem
Select sample
Extract analyte(s) from matrix
Detect, identify andquantify analytes
Determine reliability andsignificance of results
Separate analytes
![Page 4: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/4.jpg)
Errors in Chemical Analysis
Impossible to eliminate errors.How reliable are our data?Data of unknown quality are useless!
•Carry out replicate measurements•Analyse accurately known standards•Perform statistical tests on data
![Page 5: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/5.jpg)
Mean Defined as follows:
xx
N
i
N
= i = 1
Where xi = individual values of x and N = number of replicate measurements
Median
The middle result when data are arranged in order of size (for even numbers the mean of middle two). Median can be preferred whenthere is an “outlier” - one reading very different from rest. Median less affected by outlier than is mean.
![Page 6: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/6.jpg)
Illustration of “Mean” and “Median”
Results of 6 determinations of the Fe(III) content of a solution, known to contain 20 ppm:
Note: The mean value is 19.78 ppm (i.e. 19.8ppm) - the median value is 19.7 ppm
![Page 7: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/7.jpg)
Precision
Relates to reproducibility of results..How similar are values obtained in exactly the same way?
Useful for measuring this:Deviation from the mean:
d x xi i
![Page 8: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/8.jpg)
Accuracy
Measurement of agreement between experimental mean andtrue value (which may not be known!).Measures of accuracy:
Absolute error: E = xi - xt (where xt = true or accepted value)
Relative error: Er
xi xtxt
100%
(latter is more useful in practice)
![Page 9: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/9.jpg)
Illustrating the difference between “accuracy” and “precision”
Low accuracy, low precision Low accuracy, high precision
High accuracy, low precision High accuracy, high precision
![Page 10: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/10.jpg)
Some analytical data illustrating “accuracy” and “precision”
HHSNH3+Cl-NH
N
OH
O
Benzyl isothioureahydrochloride
Nicotinic acid
Analyst 4: imprecise, inaccurateAnalyst 3: precise, inaccurateAnalyst 2: imprecise, accurateAnalyst 1: precise, accurate
![Page 11: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/11.jpg)
Types of Error in Experimental Data
Three types:(1) Random (indeterminate) Error
Data scattered approx. symmetrically about a mean value.Affects precision - dealt with statistically (see later).
(2) Systematic (determinate) ErrorSeveral possible sources - later. Readings all too high or too low. Affects accuracy.
(3) Gross ErrorsUsually obvious - give “outlier” readings.Detectable by carrying out sufficient replicatemeasurements.
![Page 12: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/12.jpg)
Sources of Systematic Error1. Instrument Error
Need frequent calibration - both for apparatus such asvolumetric flasks, burettes etc., but also for electronicdevices such as spectrometers.
2. Method ErrorDue to inadequacies in physical or chemical behaviourof reagents or reactions (e.g. slow or incomplete reactions)Example from earlier overhead - nicotinic acid does notreact completely under normal Kjeldahl conditions for nitrogen determination.
3. Personal Errore.g. insensitivity to colour changes; tendency to estimatescale readings to improve precision; preconceived idea of“true” value.
![Page 13: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/13.jpg)
Systematic errors can be constant (e.g. error in burette reading -less important for larger values of reading) orproportional (e.g. presence of given proportion ofinterfering impurity in sample; equally significantfor all values of measurement)
Minimise instrument errors by careful recalibration and goodmaintenance of equipment.
Minimise personal errors by care and self-discipline
Method errors - most difficult. “True” value may not be known.Three approaches to minimise:•analysis of certified standards•use 2 or more independent methods•analysis of blanks
![Page 14: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/14.jpg)
Statistical Treatment of Random Errors
There are always a large number of small, random errorsin making any measurement.
These can be small changes in temperature or pressure; random responses of electronic detectors (“noise”) etc.
Suppose there are 4 small random errors possible.Assume all are equally likely, and that each causes an errorof U in the reading.Possible combinations of errors are shown on the next slide:
![Page 15: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/15.jpg)
Combination of Random Errors
Total Error No. Relative Frequency
+U+U+U+U +4U 1 1/16 = 0.0625
-U+U+U+U +2U 4 4/16 = 0.250+U-U+U+U+U+U-U+U+U+U+U-U
-U-U+U+U 0 6 6/16 = 0.375-U+U-U+U-U+U+U-U+U-U-U+U+U-U+U-U+U+U-U-U
+U-U-U-U -2U 4 4/16 = 0.250-U+U-U-U-U-U+U-U-U-U-U+U
-U-U-U-U -4U 1 1/16 = 0.01625
The next overhead shows this in graphical form
![Page 16: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/16.jpg)
Frequency Distribution forMeasurements Containing Random Errors
4 random uncertainties 10 random uncertainties
A very large number ofrandom uncertainties
This is aGaussian or
normal errorcurve.
Symmetrical aboutthe mean.
![Page 17: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/17.jpg)
Replicate Data on the Calibration of a 10ml Pipette
No. Vol, ml. No. Vol, ml. No. Vol, ml
1 9.988 18 9.975 35 9.9762 9.973 19 9.980 36 9.9903 9.986 20 9.994 37 9.9884 9.980 21 9.992 38 9.9715 9.975 22 9.984 39 9.9866 9.982 23 9.981 40 9.9787 9.986 24 9.987 41 9.9868 9.982 25 9.978 42 9.9829 9.981 26 9.983 43 9.97710 9.990 27 9.982 44 9.97711 9.980 28 9.991 45 9.98612 9.989 29 9.981 46 9.97813 9.978 30 9.969 47 9.98314 9.971 31 9.985 48 9.98015 9.982 32 9.977 49 9.98316 9.983 33 9.976 50 9.97917 9.988 34 9.983
Mean volume 9.982 ml Median volume 9.982 mlSpread 0.025 ml Standard deviation 0.0056 ml
![Page 18: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/18.jpg)
Calibration data in graphical form
A = histogram of experimental results
B = Gaussian curve with the same mean value, the same precision (see later)and the same area under the curve as for the histogram.
![Page 19: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/19.jpg)
SAMPLE = finite number of observations
POPULATION = total (infinite) number of observations
Properties of Gaussian curve defined in terms of population.Then see where modifications needed for small samples of data
Main properties of Gaussian curve:
Population mean () : defined as earlier (N ). In absence of systematic error, is the true value (maximum on Gaussian curve).
Remember, sample mean ( x ) defined for small values of N.
(Sample mean population mean when N 20)
Population Standard Deviation () - defined on next overhead
![Page 20: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/20.jpg)
: measure of precision of a population of data,given by:
( )x
N
ii
N2
1
Where = population mean; N is very large.
The equation for a Gaussian curve is defined in terms of and , as follows:
ye x
( ) /
2 22
2
![Page 21: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/21.jpg)
Two Gaussian curves with two different
standard deviations, A and B (=2A)
General Gaussian curve plotted inunits of z, where
z = (x - )/i.e. deviation from the mean of adatum in units of standard deviation. Plot can be used for data with given value of mean,and any standard deviation.
![Page 22: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/22.jpg)
Area under a Gaussian Curve
From equation above, and illustrated by the previous curves, 68.3% of the data lie within of the mean (), i.e. 68.3% of
the area under the curve lies between of .
Similarly, 95.5% of the area lies between , and 99.7% between .
There are 68.3 chances in 100 that for a single datum the random error in the measurement will not exceed .
The chances are 95.5 in 100 that the error will not exceed .
![Page 23: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/23.jpg)
Sample Standard Deviation, s
The equation for must be modified for small samples of data, i.e. small N
sx x
N
ii
N
( )2
1
1
Two differences cf. to equation for :
1. Use sample mean instead of population mean.
2. Use degrees of freedom, N - 1, instead of N.Reason is that in working out the mean, the sum of the differences from the mean must be zero. If N - 1 values areknown, the last value is defined. Thus only N - 1 degreesof freedom. For large values of N, used in calculating, N and N - 1 are effectively equal.
![Page 24: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/24.jpg)
Alternative Expression for s(suitable for calculators)
sx
x
NN
ii
N ii
N
( )( )
2
1
1
2
1
Note: NEVER round off figures before the end of the calculation
![Page 25: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/25.jpg)
Reproducibility of a method for determining the % of selenium in foods. 9 measurements were made on a single batch of brown rice.
Sample Selenium content (g/g) (xI) xi2
1 0.07 0.00492 0.07 0.00493 0.08 0.00644 0.07 0.00495 0.07 0.00496 0.08 0.00647 0.08 0.00648 0.09 0.00819 0.08 0.0064
xi = 0.69 xi2= 0.0533
Mean = xi/N= 0.077g/g (xi)2/N = 0.4761/9 = 0.0529
Standard Deviation of a Sample
s
0 0533 0 0529
9 10 00707106 0 007
. .. .
Coefficient of variance = 9.2% Concentration = 0.077 ± 0.007 g/g
Standard deviation:
![Page 26: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/26.jpg)
Standard Error of a Mean
The standard deviation relates to the probable error in a single measurement.If we take a series of N measurements, the probable error of the mean is less thanthe probable error of any one measurement.
The standard error of the mean, is defined as follows:
s sNm
![Page 27: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/27.jpg)
Pooled Data
To achieve a value of s which is a good approximation to , i.e. N 20,it is sometimes necessary to pool data from a number of sets of measurements(all taken in the same way).
Suppose that there are t small sets of data, comprising N1, N2,….Nt measurements.
The equation for the resultant sample standard deviation is:
sx x x x x x
N N N tpooled
i i ii
N
i
N
i
N
( ) ( ) ( ) ....
......
12
22
32
111
1 2 3
321
(Note: one degree of freedom is lost for each set of data)
![Page 28: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/28.jpg)
Analysis of 6 bottles of wine for residual sugar.
Bottle Sugar % (w/v) No. of obs. Deviations from mean1 0.94 3 0.05, 0.10, 0.082 1.08 4 0.06, 0.05, 0.09, 0.063 1.20 5 0.05, 0.12, 0.07, 0.00, 0.084 0.67 4 0.05, 0.10, 0.06, 0.095 0.83 3 0.07, 0.09, 0.106 0.76 4 0.06, 0.12, 0.04, 0.03
s
sn
1
2 2 20 05 010 0 08
2
0 0189
20 0972 0 097
( . ) ( . ) ( . ) .. .
and similarly for all .
Set n sn
1 0.0189 0.0972 0.0178 0.0773 0.0282 0.0844 0.0242 0.0905 0.0230 0.1076 0.0205 0.083
Total 0.1326
( )x xi 2
spooled
01326
23 60 088%
..
Pooled Standard Deviation
![Page 29: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/29.jpg)
Two alternative methods for measuring the precision of a set of results:
VARIANCE: This is the square of the standard deviation:
sx x
N
ii
N
2
2 2
1
1
( )
COEFFICIENT OF VARIANCE (CV)(or RELATIVE STANDARD DEVIATION):Divide the standard deviation by the mean value and express as a percentage:
CVs
x ( ) 100%
![Page 30: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/30.jpg)
Use of Statistics in Data Evaluation
![Page 31: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/31.jpg)
How can we relate the observed mean value ( x ) to the true mean ()?
The latter can never be known exactly.
The range of uncertainty depends how closely s corresponds to.
We can calculate the limits (above and below) around x that must lie,
with a given degree of probability.
![Page 32: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/32.jpg)
Define some terms:
CONFIDENCE LIMITS interval around the mean that probably contains .
CONFIDENCE INTERVALthe magnitude of the confidence limits
CONFIDENCE LEVELfixes the level of probability that the mean is within the confidence limits
Examples later. First assume that the known s is a goodapproximation to.
![Page 33: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/33.jpg)
Percentages of area under Gaussian curves between certain limits of z (= x - )
50% of area lies between 0.6780% “ 1.2990% “ 1.6495% “ 1.9699% “ 2.58
What this means, for example, is that 80 times out of 100 the true mean will liebetween 1.29 of any measurement we make.
Thus, at a confidence level of 80%, the confidence limits are 1.29
For a single measurement: CL for = x z (values of z on next overhead)
For the sample mean of N measurements ( x ), the equivalent expression is:
CL for x zN
![Page 34: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/34.jpg)
Values of z for determining Confidence Limits
Confidence level, % z
50 0.6768 1.080 1.2990 1.6495 1.9696 2.0099 2.5899.7 3.0099.9 3.29
Note: these figures assume that an excellent approximationto the real standard deviation is known.
![Page 35: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/35.jpg)
Atomic absorption analysis for copper concentration in aircraft engine oil gave a value
of 8.53 g Cu/ml. Pooled results of many analyses showed s = 0.32 g Cu/ml.Calculate 90% and 99% confidence limits if the above result were based on (a) 1, (b) 4, (c) 16 measurements.
90% 853164 0 32
1853 052
85 05
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
(a)
99% 8 532 58 0 32
18 53 0 83
8 5 0 8
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
(b)
90% 853164 0 32
4853 0 26
85 0 3
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
99% 8532 58 0 32
4853 0 41
85 0 4
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
(c)
90% 8 53164 0 32
168 53 013
8 5 01
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
99% 8 532 58 0 32
168 53 0 21
8 5 0 2
CL g / ml
i.e. g / ml
.( . )( . )
. .
. .
Confidence Limits when is known
![Page 36: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/36.jpg)
If we have no information on , and only have a value for s - the confidence interval is larger,i.e. there is a greater uncertainty.
Instead of z, it is necessary to use the parameter t, defined as follows:
t = (x - )/s
i.e. just like z, but using s instead of .
By analogy we have: CL for
(where = sample mean for measurements)
x tsN
x N
The calculated values of t are given on the next overhead
![Page 37: Principles of Analytical Chemistry (F13I11) Recommended textbook: “Fundamentals of Analytical Chemistry” Skoog, West and Holler, 7th Ed., 1996 (Saunders.](https://reader033.fdocuments.in/reader033/viewer/2022061609/56649e555503460f94b4c575/html5/thumbnails/37.jpg)
Values of t for various levels of probability
Degrees of freedom 80% 90% 95% 99%(N-1)1 3.08 6.31 12.7 63.72 1.89 2.92 4.30 9.923 1.64 2.35 3.18 5.844 1.53 2.13 2.78 4.605 1.48 2.02 2.57 4.036 1.44 1.94 2.45 3.717 1.42 1.90 2.36 3.508 1.40 1.86 2.31 3.369 1.38 1.83 2.26 3.2519 1.33 1.73 2.10 2.8859 1.30 1.67 2.00 2.66 1.29 1.64 1.96 2.58
Note: (1) As (N-1) , so t z(2) For all values of (N-1) < , t > z, I.e. greater uncertainty
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Analysis of an insecticide gave the following values for % of the chemical lindane: 7.47, 6.98, 7.27. Calculate the CL for the mean value at the 90% confidence level.
xi% xi2
7.47 55.80096.98 48.72047.27 52.8529
xi = 21.72 xi2 = 157.3742
xx
Ni
2172
37 24
..
sx
x
NN
ii
22
2
1
157 3742 21723
20 246 0 25%
( ). ( . )
. .
90% CL
x tsN
7 242 92 0 25
37 24 0 42%
.( . )( . )
. .
If repeated analyses showed that s = 0.28%: 90% CL
x zN
7 24164 0 28
37 24 0 27%
.( . )( . )
. .
Confidence Limits where is not known
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Testing a Hypothesis
Carry out measurements on an accurately known standard.
Experimental value is different from the true value.
Is the difference due to a systematic error (bias) in the method - or simply to random error?
Assume that there is no bias(NULL HYPOTHESIS),and calculate the probabilitythat the experimental erroris due to random errors.
Figure shows (A) the curve for
the true value (A = t) and
(B) the experimental curve (B)
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Bias = B- A = B - xt.
Test for bias by comparing with the
difference caused by random error
x xt
Remember confidence limit for (assumed to be xt, i.e. assume no bias)
is given by:
CL for
at desired confidence level, random
errors can lead to:
if , then at the desired
confidence level bias (systematic error)
is likely (and vice versa).
xts
N
x xts
N
x xts
N
t
t
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A standard material known to contain 38.9% Hg was analysed byatomic absorption spectroscopy. The results were 38.9%, 37.4%and 37.1%. At the 95% confidence level,is there any evidence for a systematic error in the method?
x x x
x x
s
t
i i
37 8% 11%
113 4 4208 30
4208 30 113 4 3
20 943%
2
2
. .
. .
. ( . ).
Assume null hypothesis (no bias). Only reject this if
x x ts Nt
But t (from Table) = 4.30, s (calc. above) = 0.943% and N = 3
ts N
x x ts Nt
4 30 0 943 3 2 342%. . .
Therefore the null hypothesis is maintained, and there is no evidence for systematic error at the 95% confidence level.
Detection of Systematic Error (Bias)
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Are two sets of measurements significantly different?
Suppose two samples are analysed under identical conditions.
Sample 1 from replicate analyses
Sample 2 from replicate analyses
x N
x N1 1
2 2
Are these significantly different?
Using definition of pooled standard deviation, the equation on the last overhead can be re-arranged:
x x tsN N
N Npooled1 21 2
1 2
Only if the difference between the two samples is greater than the term onthe right-hand side can we assume a real difference between the samples.
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Test for significant difference between two sets of data
Two different methods for the analysis of boron in plant samples gave the following results (g/g):(spectrophotometry)(fluorimetry)
Each based on 5 replicate measurements.At the 99% confidence level, are the mean values significantlydifferent?Calculate spooled = 0.267. There are 8 degrees of freedom,
therefore (Table) t = 3.36 (99% level).Level for rejecting null hypothesis is
ts N N N N1 2 1 2 3 36 0 267 10 25 - i.e. ( . )( . )i.e. ± 0.5674, or ±0.57 g/g.
But g / gx x1 2 28 0 26 25 175 . . . i.e. x x ts N N N Npooled1 2 1 2 1 2
Therefore, at this confidence level, there is a significant difference, and there must be a systematic error in at least one of the methods of analysis.
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A set of results may contain an outlying result - out of line with the others. Should it be retained or rejected? There is no universal criterion for deciding this. One rule that can give guidance is the Q test.
Qexp xq xn /w
where xq = questionable result xn = nearest neighbour w = spread of entire set
Consider a set of results
The parameter Qexp is defined as follows:
Detection of Gross Errors
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Qexp is then compared to a set of values Qcrit:
Rejection of outlier recommended if Qexp > Qcrit for the desired confidence level.
Note:1. The higher the confidence level, the less likely is rejection to be recommended.
2. Rejection of outliers can have a marked effect on mean and standard deviation, esp. when there are only a few data points. Always try to obtain more data.3. If outliers are to be retained, it is often better to report the median value rather than the mean.
Qcrit (reject if Qexpt > Qcrit)
No. of observations 90% 95% 99% confidencelevel
3 0.941 0.970 0.9944 0.765 0.829 0.9265 0.642 0.710 0.8216 0.560 0.625 0.7407 0.507 0.568 0.6808 0.468 0.526 0.6349 0.437 0.493 0.59810 0.412 0.466 0.568
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The following values were obtained for the concentration of nitrite ions in a sample of river water: 0.403, 0.410, 0.401, 0.380 mg/l.Should the last reading be rejected?
Qexp . . ( . . ) . 0 380 0 401 0 410 0 380 0 7
But Qcrit = 0.829 (at 95% level) for 4 values
Therefore, Qexp < Qcrit, and we cannot reject the suspect value.
Suppose 3 further measurements taken, giving total values of:
0.403, 0.410, 0.401, 0.380, 0.400, 0.413, 0.411 mg/l. Should
0.380 still be retained?
Qexp . . ( . . ) . 0 380 0 400 0 413 0 380 0 606But Qcrit = 0.568 (at 95% level) for 7 values
Therefore, Qexp > Qcrit, and rejection of 0.380 is recommended.
But note that 5 times in 100 it will be wrong to reject this suspect value!Also note that if 0.380 is retained, s = 0.011 mg/l, but if it is rejected,s = 0.0056 mg/l, i.e. precision appears to be twice as good, just by rejecting one value.
Q Test for Rejection of Outliers
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Obtaining a representative sample
Homogeneous gaseous or liquid sampleNo problem – any sample representative.
Solid sample - no gross heterogeneityTake a number of small samples at random from throughout the bulk - this will give a suitable representative sample.
Solid sample - obvious heterogeneityTake small samples from each homogeneous region and mix these in the same proportions as between each region and the whole.
If it is suspected, but not certain, that a bulk material is heterogeneous, then it is necessary to grind the sample to a fine powder, and mix this very thoroughly before taking random samples from the bulk.
For a very large sample - a train-load of metal ore, or soil in a field - it is always necessary to take a large number of random samples from throughout the whole.
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Sample Preparation and Extraction
May be many analytes present - separation - see later.
May be small amounts of analyte(s) in bulk material. Need to concentrate these before analysis.e.g. heavy metals inanimal tissue, additives in polymers, herbicide residues in flour etc. etc.
May be helpful to concentrate complex mixtures selectively.
Most general type of pre-treatment: EXTRACTION.
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Classical extraction method is: SOXHLET EXTRACTION
(named after developer). Apparatus
Sample in porous thimble. Exhaustive reflux for up to 1 - 2 days. Solution of analyte(s) in volatile solvent (e.g. CH2Cl2, CHCl3 etc.) Evaporate to dryness or suitable concentration, for separation/analysis.