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Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]
Correct answer is '0.001'. Can you explain this answer?
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Verified Answer
Suppose you have extracted RNA, following which you performed spectrop...
Molarity = Number of moles of solute per litre of solution.
Here, concentration is 10 mg/ml or 10 g L-1
This means that 10 g RNA per litre Number of moles = given weight/molecular weight = 10 10000 = 10-3
There are 10-3 moles per litre.
Here, concentration is 10 mg/ml or 10 g L-1
This means that 10 g RNA per litre Number of moles = given weight/molecular weight = 10 10000 = 10-3
There are 10-3 moles per litre.
Most Upvoted Answer
Suppose you have extracted RNA, following which you performed spectrop...
Explanation:
To determine the molarity of the RNA solution, we need to consider the molecular weight of RNA and the concentration of the solution.
Molecular weight of RNA:
It is given that each RNA has an average weight of 10 kDa (kilodaltons). To convert this into grams, we need to multiply it by the molecular weight conversion factor:
1 kDa = 1 x 10^3 g/mol
So, the molecular weight of RNA is:
10 kDa = 10 x 10^3 g/mol = 10,000 g/mol
Concentration of the RNA solution:
The spectrophotometry measurement showed a concentration of 10 mg/ml.
To convert this concentration into moles per liter (Molarity), we need to divide the concentration by the molecular weight of RNA.
Calculating the molarity:
Step 1: Convert the concentration from mg/ml to g/L:
10 mg/ml = 10 x 10^-3 g/ml
As there are 1000 ml in 1 L, the concentration in g/L will be:
10 x 10^-3 g/ml x 1000 ml/L = 10 g/L
Step 2: Calculate the number of moles of RNA in 1 liter of the solution:
Number of moles = Concentration (in g/L) / Molecular weight (in g/mol)
Number of moles = 10 g/L / 10,000 g/mol = 0.001 mol/L
Step 3: Convert moles per liter to Molarity:
Molarity (M) = Number of moles / Volume (in L)
As we want the molarity in 1 L, the volume is 1 L:
Molarity (M) = 0.001 mol/L / 1 L = 0.001 M
Therefore, the molarity of the RNA solution is 0.001 M.
To determine the molarity of the RNA solution, we need to consider the molecular weight of RNA and the concentration of the solution.
Molecular weight of RNA:
It is given that each RNA has an average weight of 10 kDa (kilodaltons). To convert this into grams, we need to multiply it by the molecular weight conversion factor:
1 kDa = 1 x 10^3 g/mol
So, the molecular weight of RNA is:
10 kDa = 10 x 10^3 g/mol = 10,000 g/mol
Concentration of the RNA solution:
The spectrophotometry measurement showed a concentration of 10 mg/ml.
To convert this concentration into moles per liter (Molarity), we need to divide the concentration by the molecular weight of RNA.
Calculating the molarity:
Step 1: Convert the concentration from mg/ml to g/L:
10 mg/ml = 10 x 10^-3 g/ml
As there are 1000 ml in 1 L, the concentration in g/L will be:
10 x 10^-3 g/ml x 1000 ml/L = 10 g/L
Step 2: Calculate the number of moles of RNA in 1 liter of the solution:
Number of moles = Concentration (in g/L) / Molecular weight (in g/mol)
Number of moles = 10 g/L / 10,000 g/mol = 0.001 mol/L
Step 3: Convert moles per liter to Molarity:
Molarity (M) = Number of moles / Volume (in L)
As we want the molarity in 1 L, the volume is 1 L:
Molarity (M) = 0.001 mol/L / 1 L = 0.001 M
Therefore, the molarity of the RNA solution is 0.001 M.
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Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer?
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Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer?.
Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer?.
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Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer?, a detailed solution for Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? has been provided alongside types of Suppose you have extracted RNA, following which you performed spectrophotometry to determine the concentration and machine showed you a concentration of 10 mg/ml. The molarity of this solution will be ________ (M). (Provided each RNA has on an average weight 10 kDa). [Answer upto three place of decimal]Correct answer is '0.001'. Can you explain this answer? theory, EduRev gives you an
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