Can you help me out? I need help with c and d. 4. A light pink, 0.050 M stock solution of cobalt (II)chloride (COCL) is analyzed by Spectrophotometry.The cuvettes are 1.0 cm wide. The data from thespectrograph is plotted here.Absorption Spectrum of CoCl,(aq)0.50.45-0.4(a) Analyze the graph above.8 0.350.3E 025E 0.20.150.10.05Estimate the wavelength you would use to(i)study the concentration of thissolution 550nmWhat is the absorbance at this wavelength?.45(ii)200300400500600700800Wavelength (nm)(b) From your various estimates and the giveninformation, calculate the molar absorptivity (ɛ) of Co2+ ions in solution.Beer-Lambert Law:.45=E x ICm x 0.0S0M E= cm-(c) Suppose this 0.05 M stock solution was left on the counter, open, overnight before generating the resultsabove. How would this affect any results from some other experiment, where this stock solution was used asmpoa standard to find an unknown Co²* concentration?sthe rightlvest leanebeand coSubstance Bsolles.(d) Solutions of transition metals are colorful when ions in solution have unpaired d-electrons. Justify that whencobalt loses two valence electrons to form Co²" ions, that this condition has been met.Wol)

The Solution of CoCl2 is stored at 4 to -20°C for the stability of the concentration. As the…

Answered: (c) Suppose this 0.05 M stock solution…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Can you help me out? I need help with c and d.

4. A light pink, 0.050 M stock solution of cobalt (II)
chloride (COCL) is analyzed by Spectrophotometry.
The cuvettes are 1.0 cm wide. The data from the
spectrograph is plotted here.
Absorption Spectrum of CoCl,(aq)
0.5
0.45-
0.4
(a) Analyze the graph above.
8 0.35
0.3
E 025
E 0.2
0.15
0.1
0.05
Estimate the wavelength you would use to
(i)
study the concentration of this
solution 550nm
What is the absorbance at this wavelength?
.45
(ii)
200
300
400
500
600
700
800
Wavelength (nm)
(b) From your various estimates and the given
information, calculate the molar absorptivity (ɛ) of Co2+ ions in solution.
Beer-Lambert Law:
.45=E x ICm x 0.0S0M E= cm-
(c) Suppose this 0.05 M stock solution was left on the counter, open, overnight before generating the results
above. How would this affect any results from some other experiment, where this stock solution was used as
mpoa standard to find an unknown Co²* concentration?
sthe right
lvest leane
beand co
Substance B
sol
les.
(d) Solutions of transition metals are colorful when ions in solution have unpaired d-electrons. Justify that when
cobalt loses two valence electrons to form Co²" ions, that this condition has been met.
Wol)

Expert Solution

Step 1:(C)

The Solution of CoCl₂ is stored at $4 t o - 20 ° C$ for the stability of the concentration.

As the solution is lefty over night the strength of the solution decreases as the dissolution of CoCl₂ solution is an endothermic reaction.

${[C o {(H_{2} O)}_{6}]}^{2 +}_{(a q)} + 2 C {l^{-}}_{(a q)} ⇌ C o C {l_{4}}^{2 -}_{(a q)} + 6 H_{2} O$

As it is an endothermic reaction the concentration of CoCl₂ is stable at very low temperatures. As it is left over open, the solution absorbs the heat and equilibrium is shifted forward. As a result of equilibrium shift the concentration of the solution decreases.

As the concentration of CoCl₂ decreases if it is used as a standard solution then the strength of unknown solution is estimated lower than the actual concentration.

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