How to solve percent concentration problems even if you're 🤷🏻‍♀️ - Dr K

[@SyedNaqvi-u7r]

The first two minutes of this video teaches me more than what my professor taught me in one hour, and that isn't even an exageration. I love the work you're doing, thank you for putting in so much effort into your videos. I love how everything is color coded, it really helps me understand the math more and where you're getting the numbers from. Thank you so much!!!

[@ChemSimplified]

Thanks so much for taking the time to leave your comments. The specific feedback is very constructive and now I know to keep the color coding in future videos! Please share the video with your friends who may find it helpful. Let's help reduce the struggles in Chemistry! 😁

[@lheenmallari5718]

Can you make it more simple?

[@jamalbartholomewiii7133]

Thank goodness, I finally get the concept our chem teacher said to us.

[@ChemSimplified]

That's awesome! Congrats on your understanding! 🎉

[@midnightshatinggabi]

life could've been so easy like this but my teacher likes it so complicated im gonna cry out for this

[@ChemSimplified]

You're fine now that you've found simpler explanation. 😊

[@rickycrumel]

Nice video but the words are too small. Thank you.

[@ChemSimplified]

Thanks for the feedback.

[@stellamendoza4587]

Thank you!!!!! This made sense it was short nd cut to the chase!😊

[@ChemSimplified]

Thanks! Could you do me a favor and help share it with your friends who need this? It'll mean a lot. 😊

[@aegonplayz7356]

I finally got it TYSM

[@ChemSimplified]

Congrats!!!

[@muhammada.muhammad6287]

good job

[@baraa3822]

Thank you greatly for these easy, straightforward videos. By any chance do you have any videos relating to molar concentration not percentage? Or is it the same process but without the percentage?

[@ChemSimplified]

Glad you find the videos helps. I do have quite a few videos on molar concentration. I refer to them as molarity. Here are a few to get you started: kzbin.info/www/bejne/rIisenx-r79opZY kzbin.info/www/bejne/bKS9eGNtbb6ebs0 kzbin.info/www/bejne/lWeQq36GjL6rhsk Do you need dilution videos?

[@ChemSimplified]

Molar concentration and percentage are similar in that their numerator is solute and the denominator is solution. However for molar concentration the top part is mols and the bottom part is L, and it does not have multiply 100. For that rrason, I'd say it's rather different than the percent concentrations. Hope the videos above will give you a good start on molar concentrations!

[@baraa3822]

@@ChemSimplified thank u so much ur amazing

[@ChemSimplified]

You're most welcome! I'm happy to be able to help. All the best in your Chemistry. You got it! 💪🏼😊

[@omaryousef7806]

thank you so much

[@ChemSimplified]

You're most welcome.

[@ayissa48]

Thank you so very much!!!!

[@ChemSimplified]

You're absolutely welcome!

[@BreadPitt24]

Danke ^-^

[@ChemSimplified]

du bist sehr willkommen

[@adnanheiza442]

How to prepare 50wt% of A with B?

[@ChemSimplified]

If you look at the formula for %wt, it's mass of solute/mass of solution x 100%. In this case, assuming you're preparing a total of 100g solution, how much A will you need? And how much B would that be?

[@rbd6661]

you failed to demonstrate the numerator version of an equation. call conversions was done with denominators.

[@ArpitDixit-ez3bk]

God great thanks

[@ChemSimplified]

Glad you find the video helpful. Thanks for leaving a comment!

[@ArpitDixit-ez3bk]

@@ChemSimplified thanks can you upload more on formulas and numerical of chemistry please it's a request

[@nokia_eq23]

Is it the same if you're using a stock solution? Bc in my book it sys that 6ml of stock solution (glucose) in 4ml of water has a concentration % of 12

[@nurmuhammad4540]

so for the last question, the amount of solvent is 350-3.5=346.5 ml or 353.5 total volume?

[@ChemSimplified]

For that question, you can't figure out the volume of solvent. This is because the information we obtained for the solute (NaCl) is mass (in grams), and you can't subtract mass from volume.

[@nurmuhammad4540]

@@ChemSimplified Then, to make a 10 wt% (NaCl) 35 ml solution, I need to add 3.5 g solute to the 35 ml solvent, right? and in this case, water is the solvent. isn't 1ml water = 1 g?

[@ChemSimplified]

@@nurmuhammad4540 Hi Nur, if it's 10% (m/v), then the way you will prepare it is to measure out 3.5g of solute. Then, you'll add sufficient solvent so that the overall solution reaches 35mL. Since the solute takes up volume, the volume of solvent is definitely less than 35mL.

[@nurmuhammad4540]

@@ChemSimplified Thank you so much.

[@ChemSimplified]

@@nurmuhammad4540 No problem! Glad I could help.

[@elvi3372]

Is %(m/m)the same as %(w/w)

[@ChemSimplified]

Yes