1.If a solution absorbed violet light, what color would the solution appear to be?
________________
Calculate the concentration of a solution prepared by adding 15.00 mL of
2.00×10^−3 M KMnO4
from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation mark with distilled water.
______________ M
Draw a color wheel. Draw three lines as diameter lines equidistant around the wheel, label the intersection of the circle with the lines as Red, Orange, yellow, green blue violet. The color absorbed is opposite to the color of the object.
2.
2.00E-3 M x (15.00/50,00) = ?
1. To determine the color of a solution that absorbs violet light, we need to understand the concept of absorption spectra. Absorption spectra refer to the wavelengths of light that a substance can absorb. Different molecules absorb different wavelengths, resulting in the appearance of different colors.
Violet light has a wavelength of approximately 400-450 nanometers. Therefore, if a solution absorbs violet light, it means that the molecules in the solution are absorbing light in this range and preventing it from reaching our eyes. As a result, the solution would appear to be a color other than violet.
Without knowing the specific molecule or solution in question, it is difficult to determine the exact color the solution would appear to be. However, we can make a general inference that if violet light is absorbed, the solution would likely appear to be a color that is complementary to violet, such as yellow or orange. Keep in mind that the appearance of a solution can also be influenced by factors such as concentration and impurities.
2. To calculate the concentration of the solution prepared by adding 15.00 mL of 2.00×10^−3 M KMnO4 into a 50.00 mL volumetric flask that is then filled to the 50.00 mL mark with distilled water, we can use the following formula:
C1V1 = C2V2
Where:
C1 = Initial concentration
V1 = Initial volume
C2 = Final concentration
V2 = Final volume
In this case:
C1 = 2.00×10^−3 M
V1 = 15.00 mL
C2 = ?
V2 = 50.00 mL
Plugging these values into the formula:
(2.00×10^−3 M) * (15.00 mL) = C2 * (50.00 mL)
Simplifying the equation:
2.00×10^−3 * 15.00 = C2 * 50.00
0.0300 = 50.00 C2
To isolate C2, we divide both sides of the equation by 50.00:
0.0300 / 50.00 = C2
C2 = 0.0006 M
Therefore, the concentration of the solution prepared is 0.0006 M.