According to Beer’s law, which of the following is true? If the absorbing species is the same, the absorbance will be the same regardless of the concentration. The greater the concentration of an absorbing species, the lower the absorbance. A solution with a concentration of 0.100 M will have a lower absorbance that one with 0.0500 M of the same absorbing species. None of the above is true.

According to Beer’s law, which of the following is true? If the absorbing species is the same, the absorbance will be the same regardless of the concentration. The greater the concentration of an absorbing species, the lower the absorbance. A solution with a concentration of 0.100 M will have a lower absorbance that one with 0.0500 M of the same absorbing species. None of the above is true.

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 59A: Explain the meaning of the relative sizes of the two shaded areas to the right of the dark vertical...

See similar textbooks

Related questions

Q: Number of Added Drops pH of Non-Buffer Solution (Water) pH of Buffer Solution 0 7.00 7.00 1…

A: As we add the drops of base solution to water, the pH of the water increases.

Q: The buffer from the above question was made by mixing 150.0 mL of 0.10 M HC7H502 with 100.0 mL of…

A: To calculate the pH of the solution formed by mixing HC7H5O2 (benzoic acid) and NaC7H5O2 (sodium…

Q: Use the HH equation to solve for the ratio of conjugate base to weak acid at pH=1. The pKa of acetic…

A: Since you have posted a question with multiple sub- parts, we will solve first three sub- parts for…

Q: This question is about a buffer solution made by mixing together solutions containing ethanoic acid…

A: Since you have posted a question with multiple independent parts, we will solve first part for you.…

Q: If two water samples were collected as follows: Sample #1 with a pH = 8.8 and the concentration of…

A: The alkalinity of water is responsible due to the presence of a concentration of ions like…

Q: and after blowing air into it for Q1. The pH of unbuffered water before blowing exhaled air into…

A: A buffer is a solution which resists any change in pH by adding a small amount of acid or base. It…

Q: Volume NaOH (added). pH of analyte 0.00 mL _1.00 10.00 mL 1.23 20.00 mL _1.54 30.00 mL _2.20…

A: Graph can be used to represent the relation between two variables over two axis, X and Y axis.…

Q: A 0.4-L unbuffered solution needs the pH adjusted from 10.0 to 3.0. How many microliters of a 5…

Q: The student added universal indicator to the alkali solution at the start of the experiment. The…

A: The Concept used here is from the ACID and BASE of chemistry. According to question. When a student…

Q: 1. Which of the following is/are true when NH4Br is dissolved in water? 1. Both NH4* and Br" are…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Question

According to Beer’s law, which of the following is true?

		If the absorbing species is the same, the absorbance will be the same regardless of the concentration.
		The greater the concentration of an absorbing species, the lower the absorbance.
		A solution with a concentration of 0.100 M will have a lower absorbance that one with 0.0500 M of the same absorbing species.
		None of the above is true.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Indicator Colour pH approximation orange IV orange Indicator Colour pH approximation thymol blue red Indicator Colour pH approximation alizarin yellow R red
Which of the following is/are true when NH Br is dissolved in water? 1. Both NH4 and Br are hydrolysable ions resulting in a neutral solution. II. The salt will completely dissociate into NH4+ and Br ions in the solution. III. The Br ion is considered as the hydrolysable ion and thus an acidic solution will form. IV. The most probable pH of the solution is acidic due to the hydrolysis of the NH4+ ion. A. I and II B. II and III C. II and IV D. I and IV
How does the concentration of a solution affect its appearance? Does changing the concentration change the color, or the intensity of the color?
2. Given the H3PO4 - NaH₂PO4 buffer system, which of the following is false when KOH is added into the said solution? O The concentration of the H3PO4 will decrease upon addition of KOH. O The concentration of the H₂PO4 will decrease upon addition of KOH. O The concentration of the H₂PO4 will increase upon addition of KOH. O The [H₂PO4 ]/[H3PO4] will decrease due to the neutralization of the added KOH.
What is the ionic strength of the following solutions? 0.100M NaH2PO4 in 0.100M NaNO3 2. 0.100M Na2HPO4 in 0.100M NaNO3 3. 0.100M Na3PO4 in 0.100M NaNO3
In the laboratory, a general chemistry student measured the pH of a 0.474 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.077. Use the information she obtained to determine the Ka for this acid. Ka(experiment)
This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added. b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?
1. How many moles of Ca2+ and OH- ions are produced for every one mole of Ca(OH)2 that dissolves in solution? Ca(OH)2(s)↔ Ca2+(aq) + 2OH-(aq) 2. A student determined that 20.0 mL of a saturated calcium hydroxide solution required 5.23 mL of a 0.108 M HCl solution to reach the equivalence point. Calculate the number of moles of Ca(OH)2 titrated and the molar concentration of the saturated Ca(OH)2 solution. Ca(OH)2(aq)+ 2HCl (aq)→ CaCl2(aq) + 2H2O(l) 3. Calculate the Ksp of Ca(OH)2
Calculate pH of a weak base/conjugate acid buffer solution. A 0.186-M aqueous solution of C6H5NH2 (aniline) has a pH of 9.07. Calculate the pH of a buffer solution that is 0.186 M in C6H5NH2 and 0.292 M in C6H5NH3. pH =
Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Name Formula Kb 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, 4.38 x 10-4 C₂H5NH₂ 5.6 x 10-4 Ethylamine Aniline CHẠNH, 3.8 x 10-10 Pyridine CsHsN 1.7 x 10-⁹ 2. Compute for pKb Conjugate Acid NH4+ CH;NH * C₂H5NH3+ CH,NH,* CH,NH*
A solution is tested with the four indicator solutions shown in the attached colour chart. The following results are obtained: Thymol blue turns yellow. Methyl orange turns yellow. Methyl red turns orange. • Bromothymol blue turns yellow. What is the estimated pH of the solution? Thymol blue red 1,2 - 2,8 yellow 8.0-9,6 blue Methyl orange red 3,0 - 4,6 yellow Methyl red red 4,2 - 6,3 yellow Bromothymol blue yellow 6,0 - 7,8 blue 2 3 4 10 11 12 pH A. 4.3 В. 8.0 C. 5.3 D. 2.8
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMO(aq) → H(aq) + MO (aq) yellow red If methyl orange is added to distilled water, the solution turns yellow. If a drop or two of 6 M HCI is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH the color reverts to yellow.