Professor Organic Chemistry Tutor, thank you for a solid/clear explanation of How to Convert PPM to Molarity in AP/General Chemistry. The definition of Molarity and PPM (parts per million) increases my understanding of conversions in this video. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
so if i get this right, you can basically say ppm = mg/L ?? because in general you don't have the density of a solution and furthermore, usually the density doesn't change a lot (e.g. in you example the result is 0.022, and without considering the density the result is 0.021, which is an error of 5%).
To convert parts per million (ppm) to parts per billion (ppb), you need to multiply the ppm value by 1000. This is because there are 1000 parts per billion in one part per million. Here's the formula for the conversion: ppb = ppm * 1000 For example, if you have a concentration of 5 ppm, you can convert it to ppb as follows: ppb = 5 ppm * 1000 = 5000 ppb So, 5 ppm is equivalent to 5000 ppb.
Hi he Organic Chemistry Tutor, can you answer a question for me? I've been reviewing this topic and it has made me super confused. I have 2 scenarios I hope you can clear up for me. I hope my wording is understandable. First, some definitions: A. *SolVENT*: the liquid that the (usually solid) substance is dissolved in, like water, oil or alcohol. B. *SoLUTE*: the substance needing dissolving or diluting C. *SoLUTION*: the final thing with both a solvent and a solute. Question 1: What is the definition of CONCENTRATION, amount of solute per solVENT or per final solution? My issue: Scenario 1: Imagine I have 1 liter of water (solvent) and I have to use all of it. If I add 10g of salt, what is the concentration? Note, when you add the salt, the volume will increase and no longer be 1 liter. This scenario is used in cooking, say I have a liter of soup and I want to add salt for flavour. I can have a recipe/ratio that says "Add 10g of salt for every 1 liter of soup". How would I summarise this statement? The concentration of salt for this recipe is ___?" Scenario 2: Imagine I dissolve 10g of salt in some water, then ADD ENOUGH WATER TO FORM EXACTLY 1 LITER, what is the concentration? I haven't done wet lab stuff for a while now so I am confused, please forgive any errors below: I have definitely done both scenarios before, but cannot think of when I would do what. For scenario 2, from memory, the instructions in my handbooks would read " Make a solution of X in Y. What is the molarity of the SOLUTION?" and the way we would do this is, say, 1 in 10 would be X in (10-X) of Y, eg, 1g of salt in (10-1=) 9g of water = 10 gram overall, with the salt being 1/10 per gram of saline. This is used in serial dilutions, so that you might then have make 1 in 10, 2 in 10, 3 in 10 or 1 in 10, 1 in 100, 1 in 1000 etc. So, now I am confused.When do you use which method, and, if a question is worded like "What is the concentration if you add 10g of salt to 1 liter of water?", what is the answer? Is it 10g of salt per Liter [of water] or is it 10g of salt per unknown liters of solution, since you don't know the new volume?
Like the other reply says you don't add the volume of the salt solid. There is enough space in the water that when you add salt, water volume doesn't change. You use the Molarity equation there. You only consider changes in volume if you're adding liquid to liquids like the serial dilution you mention. In that case you use M1V1 = M2V2 and so on.
@@ridwan6695 The volume of the overall solution is raised when you add anything to it. The added substance displaces some of the solvent, so the overall volume goes up. Put some water in a measuring jug and add something to it, say a rock or something, and watch the water level rise.
Thats million in scientific form. Parts per million, to the power 6 indicates there's 6 zeros. Same with billion , it has 9 zeros, so parts per billion is 10^9. I hope this makes it clear for you. Xoxo
A city’s water supply is fluoridated by adding NaF. The desired concentration of F- is 1.6 ppm. How many mg of NaF should be added per gallon of treated water if the water supply already is 0.2 ppm in F-? Please help
Concentration - Free Formula Sheet: bit.ly/3YfzBTf
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Professor Organic Chemistry Tutor, thank you for a solid/clear explanation of How to Convert PPM to Molarity in AP/General Chemistry. The definition of Molarity and PPM (parts per million) increases my understanding of conversions in this video. This is an error free video/lecture on TH-cam TV with the Organic Chemistry Tutor.
I will never stop watching these videos.
Thank you orgo tutor. Once again you're making my chem courses a lot easier.
My mom says that I can watch one more video before my bedtime.
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Nice! The legend of chemistry coming back at it again with the clutch!
You are a Blessing from God❣️
Better than my lecturer by ppb, thanks so muchhh
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Huge thanks
Thank you so much! This video finally made me understand PPM
so if i get this right, you can basically say ppm = mg/L ?? because in general you don't have the density of a solution and furthermore, usually the density doesn't change a lot (e.g. in you example the result is 0.022, and without considering the density the result is 0.021, which is an error of 5%).
Thank you sir. I always watch your videos since High School
best teacher ❤ iam teacher at chemistry department at uni. regard
How do you upload so many videos so consistently tho I have huge respect for you :")
thank you for the explanation
so clear, thanks man
To convert parts per million (ppm) to parts per billion (ppb), you need to multiply the ppm value by 1000. This is because there are 1000 parts per billion in one part per million.
Here's the formula for the conversion:
ppb = ppm * 1000
For example, if you have a concentration of 5 ppm, you can convert it to ppb as follows:
ppb = 5 ppm * 1000 = 5000 ppb
So, 5 ppm is equivalent to 5000 ppb.
any video how to convert g/mol to ppm ?
Hi he Organic Chemistry Tutor, can you answer a question for me?
I've been reviewing this topic and it has made me super confused. I have 2 scenarios I hope you can clear up for me. I hope my wording is understandable.
First, some definitions:
A. *SolVENT*: the liquid that the (usually solid) substance is dissolved in, like water, oil or alcohol.
B. *SoLUTE*: the substance needing dissolving or diluting
C. *SoLUTION*: the final thing with both a solvent and a solute.
Question 1:
What is the definition of CONCENTRATION, amount of solute per solVENT or per final solution?
My issue:
Scenario 1:
Imagine I have 1 liter of water (solvent) and I have to use all of it. If I add 10g of salt, what is the concentration? Note, when you add the salt, the volume will increase and no longer be 1 liter.
This scenario is used in cooking, say I have a liter of soup and I want to add salt for flavour. I can have a recipe/ratio that says "Add 10g of salt for every 1 liter of soup". How would I summarise this statement? The concentration of salt for this recipe is ___?"
Scenario 2:
Imagine I dissolve 10g of salt in some water, then ADD ENOUGH WATER TO FORM EXACTLY 1 LITER, what is the concentration?
I haven't done wet lab stuff for a while now so I am confused, please forgive any errors below: I have definitely done both scenarios before, but cannot think of when I would do what. For scenario 2, from memory, the instructions in my handbooks would read " Make a solution of X in Y. What is the molarity of the SOLUTION?" and the way we would do this is, say, 1 in 10 would be X in (10-X) of Y, eg, 1g of salt in (10-1=) 9g of water = 10 gram overall, with the salt being 1/10 per gram of saline. This is used in serial dilutions, so that you might then have make 1 in 10, 2 in 10, 3 in 10 or 1 in 10, 1 in 100, 1 in 1000 etc.
So, now I am confused.When do you use which method, and, if a question is worded like "What is the concentration if you add 10g of salt to 1 liter of water?", what is the answer? Is it 10g of salt per Liter [of water] or is it 10g of salt per unknown liters of solution, since you don't know the new volume?
The volume of water is not increased when salt is added into it
Like the other reply says you don't add the volume of the salt solid. There is enough space in the water that when you add salt, water volume doesn't change. You use the Molarity equation there. You only consider changes in volume if you're adding liquid to liquids like the serial dilution you mention. In that case you use M1V1 = M2V2 and so on.
@@ridwan6695 The volume of the overall solution is raised when you add anything to it. The added substance displaces some of the solvent, so the overall volume goes up. Put some water in a measuring jug and add something to it, say a rock or something, and watch the water level rise.
Thanks for your help sir.
Love from india
Does this hold true for gases?
Why do some express 1ppm as 1mg/L? not considering the density
Its usually because the solution is water so its density is 1kg/L and you can write ppm as mg/kg
Thankyou so much 😊
6:04 Molarity -> PPM
Thank youuuuu
Wow thank you
What if you’re not given the density of the solution
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Check Tyler Dewitt
Very nice
million is smaller than a billion right? so when you convert from million to billion you should devide it by 1000
Thanks
This video was confusing what about (w/v) he completely skipped that.
Now, if I know the density of the solution and molar mass of the solute, I can change the ppm to molarity and change the molarity to ppm freely.
Can someone please explain where 10^6 comes from???
Thats million in scientific form. Parts per million, to the power 6 indicates there's 6 zeros. Same with billion , it has 9 zeros, so parts per billion is 10^9. I hope this makes it clear for you. Xoxo
how 1ppm = 1000ppb is that not 1ppb = 1000ppm or im the one who confused
How to convert ppm to molality plz see us quickly
A city’s water supply is fluoridated by adding NaF. The desired concentration of F- is 1.6 ppm. How many mg of NaF should be added per gallon of treated water if the water supply already is 0.2 ppm in F-? Please help
nice
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