Friday
November 21, 2014

Homework Help: Chemistry

Posted by Jake on Monday, March 16, 2009 at 12:26am.

Pre-Lab Questions

Data:

[mass of copper wire]
0.738 g

[standard solutions]
solution 1: 0.738 g of copper wire dissolved in 50.00 mL solution
solution 2: 1:2 dilution of solution 1
solution 3: 1:4 dilution of solution 1

[absorbance data at lambda(max)]
solution 1: 0.740
solution 2: 0.365
solution 3: 0.195

[least squares analysis of these data pieces]
slope: 49.458
y-intercept: 0.0075

A brass sample of mass 0.643 g was dissolved to make 50.00 mL of solution, which was found to have an absorbance of 0.589 at lambda(max).


Questions:

1) Calculate the concentrations of the three standard solutions (in g/mL).

solution 1: 0.738 g / 50.00 mL = 0.0148 g/mL
solution 2: 0.0148 g/mL / 2 = 0.740 g/mL
solution 3: 0.740 g/mL / 2 = 0.370 g/mL

2) If the concentrations are in units of g/mL, what are the units for the slope?

If absorbance (A) is graphed against concentration (C) then, using the least squares method, the best-fit straight line through the data will be:

A = mC + b

m (slope) = delta y / delta x = delta A / delta C

A is dimensionless. C has units of g/mL. Therefore, the slope for the data presented above is 49.458 (g/mL)^(-1).

3) What are the units for the y-intercept?

The y-intercept (b) is found when concentration is 0. This yield only a numerical value for A without any units.

Therefore, the y-intercept for the data presented above is already correct as 0.0075.

4) Calculate the percent copper in the brass sample.

This is where I'm stuck. I have no idea how to use the absorbances of the various solutions to find the percent copper in the brass sample.

The only step I'm fairly certain about is:

% copper in brass = (mass of copper in brass sample) / (mass of brass sample) *100%
% copper in brass = (mass of copper in brass sample) / (0.643 g) *100%


Any feedback regarding my work for the first 3 questions and any help on the 4th question is greatly appreciated. Thanks in advance.

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