Ion Concentration in Solutions From Molarity, Chemistry Practice Problems
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- Опубліковано 11 вер 2024
- This chemistry video tutorial explains how to calculate the ion concentration in solutions from molarity. This video contains plenty of examples and practice problems.
Stoichiometry Practice Test: • How To Solve Stoichiom...
Solute, Solvent, & Solution:
• Solute, Solvent, & Sol...
Strong & Weak Electrolytes:
• Identifying Strong Ele...
Molarity Practice Problems:
• Molarity Practice Prob...
Ion Concentration In Solutions:
• Ion Concentration in S...
Dilution Problems:
• Dilution Problems, Che...
___________________________________
Types of Chemical Reactions:
• Types of Chemical Reac...
Solubility Rules:
• Solubility Rules
Predicting The Products of Reactions:
• Predicting The Product...
Activity Series of Metals:
• Activity Series of Met...
Will This Reaction Occur?
• Chemistry - Will The R...
Predicting Products of SR Reactions:
• Predicting Products of...
___________________________________
Double Replacement Reactions:
• Introduction to Double...
Net Ionic Equations:
• Precipitation Reaction...
Writing Chemical Equations From Words:
• How To Write Chemical ...
Solution Stoichiometry:
• Solution Stoichiometry...
Molarity & Dilution Problems:
• Molarity Dilution Prob...
Acid Base Neutralization Reactions:
• Acid Base Neutralizati...
____________________________________
Acid Base Titration Problems:
• Acid Base Titration Pr...
Mixture Problems:
• Mixture Problems
Calculating Oxidation Numbers:
• How To Calculate Oxida...
Oxidation and Reduction Reactions:
• Oxidation and Reductio...
Balancing Redox Reactions:
• Half Reaction Method, ...
Ideal Gas Law Problems:
• Ideal Gas Law Practice...
___________________________________
Final Exams and Video Playlists:
www.video-tuto...
Full-Length Videos and Worksheets:
/ collections
Stoichiometry Formula Sheet:
bit.ly/3Z7uMw8
Stoichiometry Formula Sheet: bit.ly/3Z7uMw8
Final Exams and Video Playlists: www.video-tutor.net/
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professor literally did not discuss this at all in class and yet the homework with this on it is due tomorrow. thank you.
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Thank you so so much for simplifying those problems
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For example 4, it's easier if you look for the molar mass first
then you look for the mass conc by dividing the gram by liter(obviously you convert if it's in ML)
the 3rd step is to look for the molarity by dividing the result of your mass conc by the result of your molar mass(it has to be 284/142)
you'll get 2 and you can multiply it by 2 then you'll get 4. Happy to help.
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Me
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i think there is an error in 5:10 shouldn't it be .2 litres not .25 litres
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Professor Organic Chemistry Tutor, thank you for a powerful video /lecture on Ion Concentration in Solutions from Molarity in AP/General Chemistry. Some of the examples are easy to understand, however, harder problems are problematic from start to finish. Professor Organic Chemistry Tutor, thanks to the viewers for finding and correcting the error(s) in this video.
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On some occasions, you divided the solute mole into solvent litres/volume in order to find the Molarity, in another question you divided the solute mole into whole solution volume to find the molarity or concentration. What's the reason or factor for this?
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At 1:48, you said that we need to divide 2mol by 1 mole. So as at 3:10, why you did not multiply it with 2 and divided with 3? Because this isn’t the ration of moles between 2al and 3SO4 ?
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For the last question. If it was the entire equation I would have to calculate molarity for, would I include the water?
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Excuse me! Concentration and molarity are two different terms. Concentration is the ratio of the mass of solute per liter solution and its unit is kg per meter cube.
On the other hand, molarity is the ratio of the mole number of solute per liter solution and its unit is mole/Liter.
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in 7:13 why isnt the volume of 800 mL in L
For the last question why didn't we multiply the Na by 2 when we got 4M
It is Na2 shouldn't we multiply it be 2 ? Na2= 4×2=8? Could you explain it to me please
Bro 4M came bc we multiplied 2 by 2. The molarity of the solution in that case is 2 and in sodium sulphate , sodium has a subscript of 2 so we multiply the subscript by molarity (which equals to 2) and hence 2*2 equals 4
Kindly upload some videos on formality
Wow I never knew it could be so simple
Does ion concentration change when there is Ka involved?
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Please Help. When CuSo4 is the n 4 or 1? When we calculate the CN from CM
Can you please do a video on unit cells?
For question 5, why do you multiply the molar mass by 2 moles na, that step for me seemed like it came out of knowhere
Yes thats what i wz thinking too plus why do you write the whole name of the compound when it just cancels out?
excuse me, in the second example why didn't you convert ml to liter and you keep it ?
Iam lost 😔😔😔. and if i convert ml to liter, will my solution be right
Thank you, helpful :)
@ 5:01 why did you divide mols of sodium phosphate by 0.25L when you only have O.2L of solution?!?!?!?!?
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How can I find the Molarity of the compound NaNO3 when the molarity of Na+ ion is given? Is it just the reverse?
All you need to do is just multiply it by 1 mole of the compound by the amount of Na+ ions given. So : 1mol NaNO3 / 3 mol Na+. This will give you the molar concentration of the solute, or NaNO3.
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0:18 point what? point two-five no this guy who trying to teach me something just said "point twenty-five" in the first 20 seconds of a educational video...
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can someone explain the cross method that he does with the three at 4:30
It’s an easy way to know the amount of atoms in a compound it’s like an easier way of figuring out the bond
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5:01
You should have taken 20 not 25
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Don't you have to convert moles of na to ions of Na by dividing my avogadros number?
that's for the last one
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does the M stand for moles or concentration
im pretty sure its concentration
Capital M stands for moles/liter (moles per liter)
Now solve problem 4 with the only given information being 1.6M (as my professor wants). There isn’t a single Khan tutorial that gives as little information as my professor. Solving the easiest problems is not helpful.
Lmao u r complaining about ur professor in most of the comments ...is he that horrible in teaching XD
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