CHM2046L UF Spring Exam
Study Guide – Practice
Questions with Verified
Answers. GRADED A+. Latest
2026/2027 Update.
beer-lambert law - Answer✔✔-A = εdc
A = absorbance
ε = molar absorptivity (L mol-1 cm-1)
d = distance the light travels through the solution (the cuvette) in cm
c = concentration of the solution (mol/L)
Beer's Law calibration curve:
Use the following data to generate a calibration curve of Absorbance vs
Concentration at λmax = 420.6 nm.
,concentration 1: 6e-5 M; absorbance 1: 1.330
concentration 2: 2e-5 M; absorbance 1: 0.451
concentration 1: 1e-5 M; absorbance 1: 0.239
concentration 1: 2e-6 M; absorbance 1: 0.042
Record the equation and analyze your data:
- do all of the data points fall on the trendline? Is your R2 value greater than
0.990?
- what does y represent?
- what does x represent?
- why should the y-intercept of the linear trendline be very close to 0? -
Answer✔✔-equation: y=22066x + 0.008
yes, all points fall on the trendline or are very close. R2 = 0.9998
y = absorbance
x = solute concentration (mol/L)
a y-intercept of 0 indicates 0 absorbance at 0 M concentration of colored solute
,Serial Dilution:
- Perform calculations to determine the amount of 6.00x10-5 M stock solution
needed to prepare 20.00 mL of 2.00x10-5 M dye solution.
- Perform calculations to determine the amount of 2.00x10-5 M stock solution
needed to prepare 20.00 mL of 1.00x10-5 M dye solution.
- Perform calculations to determine the amount of 1.00x10-5 M stock solution
needed to prepare 20.00 mL of 2.00x10-6 M dye solution. - Answer✔✔-x =
6.67 ml
x = 10 ml
x = 4 ml
using this Beer's Law calibration curve equation, y=22066x + 0.008, at λmax =
420.6 nm, determine the concentrations for each of the absorbances values
below:
absorbance 1: 2.224
absorbance 2: 1.558
if absorbance 1 is from a 1e-3 M stock solution and absorbance 2 is from a 1e-4
M stock solution, do all of these data points follow Beer's Law? (did the
concentrations you obtained using the equation match the concentrations of
the stock solutions?). If not, why? (***hint: look at the excel graph you
, generated and determine the maximum absorbance at λmax = 420.6 nm that
falls on/very close to the trendline) - Answer✔✔-for absorbance 1:
x = 1e-4 M
for absorbance 2:
x = 7.02e-5 M
No. These concentrations obtained from the absorbances, y = 2.224 and y =
1.558, do not follow Beer's Law. The concentrations calculated do not match
the stock solution concentrations, 1e-3 M and 1e-4 M. The maximum
absorbance value that follows Beer's Law is 1.330 at λmax = 420.6 nm because
1.330 falls on the trendline. The absorbances, y = 2.224 and y = 1.558, do not
follow the trendline because their absorbances surpass the maximum
absorbance at λmax = 420.6 nm.
consider that you have a 100 mM stock solution and you need to prepare 10 ml
of a 30 mM solution.
How many ml of the stock solution do you need?
How many ml of deionized water do you need?
enter each of your answers to 2 sig figs - Answer✔✔-3.0 ml stock
7.0 ml DI water
Study Guide – Practice
Questions with Verified
Answers. GRADED A+. Latest
2026/2027 Update.
beer-lambert law - Answer✔✔-A = εdc
A = absorbance
ε = molar absorptivity (L mol-1 cm-1)
d = distance the light travels through the solution (the cuvette) in cm
c = concentration of the solution (mol/L)
Beer's Law calibration curve:
Use the following data to generate a calibration curve of Absorbance vs
Concentration at λmax = 420.6 nm.
,concentration 1: 6e-5 M; absorbance 1: 1.330
concentration 2: 2e-5 M; absorbance 1: 0.451
concentration 1: 1e-5 M; absorbance 1: 0.239
concentration 1: 2e-6 M; absorbance 1: 0.042
Record the equation and analyze your data:
- do all of the data points fall on the trendline? Is your R2 value greater than
0.990?
- what does y represent?
- what does x represent?
- why should the y-intercept of the linear trendline be very close to 0? -
Answer✔✔-equation: y=22066x + 0.008
yes, all points fall on the trendline or are very close. R2 = 0.9998
y = absorbance
x = solute concentration (mol/L)
a y-intercept of 0 indicates 0 absorbance at 0 M concentration of colored solute
,Serial Dilution:
- Perform calculations to determine the amount of 6.00x10-5 M stock solution
needed to prepare 20.00 mL of 2.00x10-5 M dye solution.
- Perform calculations to determine the amount of 2.00x10-5 M stock solution
needed to prepare 20.00 mL of 1.00x10-5 M dye solution.
- Perform calculations to determine the amount of 1.00x10-5 M stock solution
needed to prepare 20.00 mL of 2.00x10-6 M dye solution. - Answer✔✔-x =
6.67 ml
x = 10 ml
x = 4 ml
using this Beer's Law calibration curve equation, y=22066x + 0.008, at λmax =
420.6 nm, determine the concentrations for each of the absorbances values
below:
absorbance 1: 2.224
absorbance 2: 1.558
if absorbance 1 is from a 1e-3 M stock solution and absorbance 2 is from a 1e-4
M stock solution, do all of these data points follow Beer's Law? (did the
concentrations you obtained using the equation match the concentrations of
the stock solutions?). If not, why? (***hint: look at the excel graph you
, generated and determine the maximum absorbance at λmax = 420.6 nm that
falls on/very close to the trendline) - Answer✔✔-for absorbance 1:
x = 1e-4 M
for absorbance 2:
x = 7.02e-5 M
No. These concentrations obtained from the absorbances, y = 2.224 and y =
1.558, do not follow Beer's Law. The concentrations calculated do not match
the stock solution concentrations, 1e-3 M and 1e-4 M. The maximum
absorbance value that follows Beer's Law is 1.330 at λmax = 420.6 nm because
1.330 falls on the trendline. The absorbances, y = 2.224 and y = 1.558, do not
follow the trendline because their absorbances surpass the maximum
absorbance at λmax = 420.6 nm.
consider that you have a 100 mM stock solution and you need to prepare 10 ml
of a 30 mM solution.
How many ml of the stock solution do you need?
How many ml of deionized water do you need?
enter each of your answers to 2 sig figs - Answer✔✔-3.0 ml stock
7.0 ml DI water
