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By what factor must the mass increase to reduce the sampling standard deviation by a factor of 2?

Short Answer

Expert verified

The mass needs to be increased four times to reduce the sampling standard deviation by a factor of 2.

Step by step solution

01

Assumption

Let,

Ks= Sampling constant

m = mass of particle

R= relative standard deviation

σ = Standard deviation

m1 = mass of particlefor 1st case

R1= relative standard deviationfor 1st case

σ1 = Standard deviationfor 1st case

m2 = mass of particle for 2nd case

R2= relative standard deviationfor 2nd case

σ2 = Standard deviationfor 2nd case

As per the given information

σn2=σn12

02

Determine relative standard deviation

Ks=mR2m=KsR2m1=KsR12m1=Ksσn1n2m2=KsR22m2=Ksσn2n2

m2=Ksσn12n2Asσn2=σn12nm2=Ks14σn1n2m2=4Ksσn1n2m2=4m1Asm1=Ksσn1n2

Therefore, the mass needs to be increased four times to reduce the sampling standard deviation by a factor of 2

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Most popular questions from this chapter

:(a) Describe the steps in QuEChERS and explain their purpose.

(b) Why is an internal standard used in QuEChERS?

(c) What is displayed in the total ion chromatogram in Figure 28-22?

(d) What is displayed in the extracted ion chromatogram in Figure 28-22? What is the difference between an extracted ion chromatogram and a selected ion chromatogram? Which would have greater signal-to-noise ratio?

(e) What mass spectrometric method could be used to obtain even greater signal-to-noise ratio from the same QuEChERS extract?

How many 2.8-g samples must be analyzed to give 95% confidence that the mean is known to within ±4%?

What mass of sample in Figure 28-3 is expected to give a sampling standard deviation of \( \pm 6\% \)?

From their standard reduction potentials, which of the following metals would you expect to dissolve in \({\rm{HCl}}\)by the reaction\({\rm{M}} + n{{\rm{H}}^ + } \to {{\rm{M}}^{n + }} + \frac{n}{2}{{\rm{H}}_2}:{\rm{Zn}},{\rm{Fe}},{\rm{Co}},{\rm{Al}},{\rm{Hg}},{\rm{Cu}},{\rm{Pt}}\),\({\bf{Au}}\)?

(When the potential predicts that the element will not dissolve, it probably will not. If it is expected to dissolve, it may dissolve if some other process does not interfere. Predictions based on standard reduction potentials at \({\bf{2}}{{\bf{5}}^{^{\bf{o}}}}C\) are only tentative, because the potentials and activities in hot, concentrated solutions vary widely from those in the table of standard potentials.)

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