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What concentration is your potassium permanganate solution from above in percent?

What concentration is your potassium permanganate solution from above in percent?

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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It's your turn.. Exercise 2: You have been hired as lab manager for Dr. Pager's research lab. She has asked you to prepare 650 ml of a 2 M potassium permanganate (KMNO4) solution. How would you go about preparing this solution? Use the periodic table of elements provided in your manual. Conversions You may also have to convert from % solution to Molarity and vice versa, or use a solution of one concentration to make one of a different concentration. To convert from % solution to Molarity, multiply the % solution by 10 (this is to convert the percent solution, which is measured as grams/100milliliters, to grams/liter, then divide by the Molecular Weight of the solute. % solution * 10 Molecular Weight (g/mole) Molarity = Example: Your 2% maltose solution from the previous page would be, in Molarity: Molarity = 2% * 10 342.3 g/mole 0.0584 moles/liter Or, you can break it down into two separate steps and convert % (1/100) into 1/1000 (1/liter) first, 20g/liter 2g 100ml 1000ml 1 liter And then divide the resulting amount (should be in g/liter) by the Molecular Weight. 0.0584 moles/liter 20g/ 342.3 g/mole To convert from Molarity to % solution, multiply the Molarity by the Molecular Weight and divide by 10: % solution = Molarity (moles/liter) * Molecular Weight (g/mole) 10 Example: your 2 M sodium chloride solution from the previous example would be, in %: 2 moles/liter * 58.44g/mole = 11.69% % solution = 10 Of course, you know that you weighed out 29.22 g and dissolved it into 250 ml of water, so expressed as g/100 ml you do not need the Molecular Weight, just divide 29.22 by 2.5 and you have the g/100 ml (which is %). 15 Basic Laboratory Skills Boot Camp 1
Transcribed Image Text:It's your turn.. Exercise 2: You have been hired as lab manager for Dr. Pager's research lab. She has asked you to prepare 650 ml of a 2 M potassium permanganate (KMNO4) solution. How would you go about preparing this solution? Use the periodic table of elements provided in your manual. Conversions You may also have to convert from % solution to Molarity and vice versa, or use a solution of one concentration to make one of a different concentration. To convert from % solution to Molarity, multiply the % solution by 10 (this is to convert the percent solution, which is measured as grams/100milliliters, to grams/liter, then divide by the Molecular Weight of the solute. % solution * 10 Molecular Weight (g/mole) Molarity = Example: Your 2% maltose solution from the previous page would be, in Molarity: Molarity = 2% * 10 342.3 g/mole 0.0584 moles/liter Or, you can break it down into two separate steps and convert % (1/100) into 1/1000 (1/liter) first, 20g/liter 2g 100ml 1000ml 1 liter And then divide the resulting amount (should be in g/liter) by the Molecular Weight. 0.0584 moles/liter 20g/ 342.3 g/mole To convert from Molarity to % solution, multiply the Molarity by the Molecular Weight and divide by 10: % solution = Molarity (moles/liter) * Molecular Weight (g/mole) 10 Example: your 2 M sodium chloride solution from the previous example would be, in %: 2 moles/liter * 58.44g/mole = 11.69% % solution = 10 Of course, you know that you weighed out 29.22 g and dissolved it into 250 ml of water, so expressed as g/100 ml you do not need the Molecular Weight, just divide 29.22 by 2.5 and you have the g/100 ml (which is %). 15 Basic Laboratory Skills Boot Camp 1
It's your turn. Exercise 3. What concentration is your potassium permanganate solution from above in percent? Lastly, what if you already have 250 ml of a 2 M NaCl solution but you really need 400 ml of a 0.5 M NaCl solution? There is an equation for these kinds of calculations as well: C,*V, = C;*V2 Where C1: concentration of the original solution, V1: volume of the original solution and C2: concentration of the desired solution, V2: total volume of the desired solution Example: In the example above, C: concentration of the original solution: 2 moles/liter V: (volume of the original solution: 0.25 liter) C2: concentration of the desired solution: 0.5 moles/liter V2: total volume of the desired solution: 0.4 liter Hint: You seem to have all 4 entities given, so the problem is usually what are you looking for? If you think about it, yes, you have 0.25 liters of the original solution, but the question is, how much of it will you need to make the more dilute desired solution. So although you have a value for V1 (0.25 liters) you won't need all of it, and you need to rearrange the equation so that you can figure out how much of it you will need: you are looking for V1. How much of V is necessary to make our 400 ml a 0.5 M solution? And since the original solution is more concentrated, how much extra water do we have to add to bring the volume up to 400 ml? = 0.5 moles/liter * 0.4 liter 2 moles/liter VI C*V2 = 0.1 liter; We need 0.1 liter or 100 ml of the 2 M solution. If we then fill the total volume to 400 ml with water, we should have our 0.5 M solution. You can test your calculation: if we take 0.1 liter of a 2 M solution and dissolve it in a total of 0.4 liter, what is the resulting concentration? 0.1 liter * 2 moles/liter = ? 0.4 liter the answer should be 0.5M It's your turn.. Exercise 4: You are working as a Research Scientist I at Albany Molecular Research. For one of your bacterial growth media, you need to prepare 1.2 liters of a 20mM sucrose solution, but you currently only have 200 ml of a 1.5 M sucrose solution. What do you need to do?
Transcribed Image Text:It's your turn. Exercise 3. What concentration is your potassium permanganate solution from above in percent? Lastly, what if you already have 250 ml of a 2 M NaCl solution but you really need 400 ml of a 0.5 M NaCl solution? There is an equation for these kinds of calculations as well: C,*V, = C;*V2 Where C1: concentration of the original solution, V1: volume of the original solution and C2: concentration of the desired solution, V2: total volume of the desired solution Example: In the example above, C: concentration of the original solution: 2 moles/liter V: (volume of the original solution: 0.25 liter) C2: concentration of the desired solution: 0.5 moles/liter V2: total volume of the desired solution: 0.4 liter Hint: You seem to have all 4 entities given, so the problem is usually what are you looking for? If you think about it, yes, you have 0.25 liters of the original solution, but the question is, how much of it will you need to make the more dilute desired solution. So although you have a value for V1 (0.25 liters) you won't need all of it, and you need to rearrange the equation so that you can figure out how much of it you will need: you are looking for V1. How much of V is necessary to make our 400 ml a 0.5 M solution? And since the original solution is more concentrated, how much extra water do we have to add to bring the volume up to 400 ml? = 0.5 moles/liter * 0.4 liter 2 moles/liter VI C*V2 = 0.1 liter; We need 0.1 liter or 100 ml of the 2 M solution. If we then fill the total volume to 400 ml with water, we should have our 0.5 M solution. You can test your calculation: if we take 0.1 liter of a 2 M solution and dissolve it in a total of 0.4 liter, what is the resulting concentration? 0.1 liter * 2 moles/liter = ? 0.4 liter the answer should be 0.5M It's your turn.. Exercise 4: You are working as a Research Scientist I at Albany Molecular Research. For one of your bacterial growth media, you need to prepare 1.2 liters of a 20mM sucrose solution, but you currently only have 200 ml of a 1.5 M sucrose solution. What do you need to do?
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