Acid Base Neutralization Reactions & Net Ionic Equations - Chemistry
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- Опубліковано 19 сер 2017
- This chemistry video tutorial explains how to predict the products of acid base neutralization reactions. It explains how to balance the chemical equation, write the total ionic equation, identify the spectator ions and write the net ionic equations. It discusses what to do when strong acids and weak acids are present. Weak acids should not be separated into ions in the ionic equation due to partial ionization. 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...
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TIMESTAMPS 🍋
0:00 H2SO4 + NaOH
4:53 HC2H3O2 + KOH
9:54 HNO3 + Mg(OH)2
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STEPS: 👣
1. Write the products (acid + base = salt + water)
2. Balance the equation, if needed
3. Decide if the salt is soluble or not. If it's soluble, it's in aq state
4. Are the initial acids and bases strong or weak? If they are strong they will dissociate in ions, if not, they won't
5. Write the net ionic equation. Everything that is in the aq state and is strong, will dissociate into ions, write the rest as they were
6. Cancel out ions that are the same on both sides
7. If you have a number that is repeating on every part of the equation, divide the equation by that number
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Alkali metals are always soluble
You make something so complicated in class into something so simple online. Thank you so much for doing what you do
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I know this video is old but it still helps me and other people to this day, thank you for the amazing explanations
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Thanks this video was very good, and easy to understand.
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Thank you so much! This video was super helpful! You provided many easy-to-follow examples, and now I am very confident in predicting acid-base equations!
thanks man you are the best really helped a lot i have a test tomorrow and thanks so much wish you the best
Professor Organic Chemistry Tutor, thank you for a solid analysis of Acid Base Neuralization Reactions and Net Ionic Equations in AP/General Chemistry. Writing the total ionic equations, balancing the chemical equations, identify the spectator ions and writing the net ionic equations are excellent from start to finish. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
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got gcse mocks coming up, i love how you explain the steps for each equation and why you do certain things.
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1:01 really amazing teaching. When you started drawing that line I instantly knew what to do..thank you
Under 2 hours, I learned how to balance equations, learned solubility rules, create net ionic equations and other chemical equation related topic because of this guy, than my 4 class sessions (6 hours) with our teacher
Late reply, but yes. It is crazy how condensing information into comprehensible videos is so efficient. Professors overcomplicate things sometimes.
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thank you for explaining Na2 (subscript) I couldn't understand where the Na2 (subscript) came from.
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But what if the equation works out that your products are HOH and a non-soluble compound? I have a chem lab that is asking for the ionic and net-ionic equations on a problem like that but wouldn’t the ionic and net-ionic reactions be the same since every ion became part of a non-aqueous compound? I’m so confused 😅
I like this guy
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So how come acetic acid won't dissociate on the left side with Hydrogen, but will with K+ on the right? o_O I am confusion- around minute 9- thanks in advance if someone answers
CalYsta Y The K is a group one alkali metal so it is completely soluble. The one with the hydrogen is a weak base, meaning when put in water it stays mostly as an acid ad not ions. That’s why we can’t show it as disassociating but we can show it’s salt as it’s ions
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Are we supposed to be able to tell these are aqueous from the beginning or would it be specified in the beginning of a problem?
5:25 Shouldn't the arrow be double-sided since hydrogen acetate is a weak acid?
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Yo
do we need to separate weak base into ions for ionic equation?
Hi, why do you only break up substances in the aqueous phase ? And not liquid or solid ?
i think bc it dissociates in an aqueous solution or smtg
U saved me and all of us lol
But how do you know how many ions are in each component. How do i know what it plus and minus and by how much :( i don’t get this
What is the cross cross method?
this guy's back must hurt from consistently carrying us D;
in 3:45 why did we add the 1 in front of H2 and Na2SO4?
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how can we tell if it's a strong or a weak acid/base?
U just have to get good bruv
Memorize
For the first problem, couldn't you have done [H2SO4 + NaOH --> H2O + NaHSO4] than ionize the equation to [H(+) + HSO4(-) + Na(+) + OH(-) ---> H2O + Na(+) + HSO4(-), than cancel the spectators to get the same answer? Just curious. lol literally got to the 8minute mark and here you are answering my question. So, since it was a strong base that completely ionized HSO4(-) to SO4(2-). Would the approach I went about work for all SB and SA reactions?
Holy shit thank you so much
I don't understand with the sulfuric acid ionising partially in water
under basic conditions u leave it as is, but sometimes u have to dissociate it
What is the reaction when hcl+naoh
anda how you do that same thing but in a problem they are giving you the products and no the reactors
i think u have to dissociate it first before u can do anything else
i dont know the phases except the solubility chart can you help like when does it have (g)
halogens in column VIIA are gases meaning they are diatomic elements, you'll see those in Single Replacement or Combination, Depositions. H2O MAY also be a gas H2O (g) when a reaction produces steam when you add heat to it. The symbol used for heat us a triangle in a chemical reaction involving heat. But thats the only time H2O can be a gas. When their is no heat and just neutralization or ionizations its a liquid (l)
how did you know the charge of c2h3o2
*Im not understanding how you are supposed to "Know" how to get the answers you got. You literally just looked at it and then "so we have this, we get this" How do we know that???*
Professional Biologist, you have to learn the solubility rules.
This should be viewed as a series with many prior videos alongside a good bit of 1st-3rd chapter of a basic inorganic chemistry book. Flashcards for the polyatomic ions really helped.
This was 5 years ago and guess what we can both agree you never used this ever again in your life after that exam you had isn’t it crazy ?
How is the net ionic equation H+. + OH-? isn't a net ionic equation the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction.
so basically if its not in the strong acids/bases chart then its a weak acid/base?
Anonymous yes if its not strong then its weak
But you say strong or weak alkali not base
Good video but
acetic acid formula is CH3COO but you wrote HC2H3O2 so plzz make me understand
they are the same thing. CH3COO is just written in a way that is more similar to what it looks like structurally.
It can be written as C2H3O2 as well. It’s preference. Good luck.
it's the same thing there's just two different ways to write it lol, if u count the amount of each element they're the same
Chemistry is fun guys💗
@Dr.K
for the first strong acid strong base reaction, why don't you write out the ions for water?
Because water is not soluble in water; it is a liquid.
can the acetate be broken down into smaller compounds?
No, never break down Miscellaneous Ions. Think of it as a "whole number", breaking it down would only make it more challenging for you and you waste time
Y did you split H2SO4 and NAOH dont they stay as it cuz they are strong acids ?
no nigga
You split if they are strong
Why do we write KC2H3O2 as K+C2H3O2?
it gets dissociated :)
What about a reaction like Na2CrO4 + HCl?
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If the equation in a question does not specify an ion's phase/state, how would I determine the reactant and product's phase/state?
I'm not sure but maybe te solubility rules?
What happened to the third H for the Neutralisation of H2SO4+NaOH?
Bratisma •999 it was written as OH
Unicorn Spirts: Oh, Right!Thank you!
Also, my teacher did the same example with the net ionic equation of H3O + OH -> 2H2O
Rather than just 1 H2O
H2+OH=H2O but H3O+OH= 2H2O
you must be an angel @_@
do combustion reactions have net ionic equations?
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Why does SO4 have a -2 charge? I thought it would be -4 because S has +4 and O has -2 x 4? Please help ik I’m wrong I just don’t know why. 1:20
Creeperroese SO4 is a polyatomic ion, meaning they have different charges and don’t follow the normal rules
@@challyzilla9483 ik about polyatomic ions and their charges but any idea why they dont follow normal rules?
@@challyzilla9483 hi
Hii
sulfate is a polyatomic ion :)
A teacher took off points for writing the ones in, why??
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@@PHILLYMEDIC69 tf
Where did you write the ones ?
You have to explain more
am i dumb? i swear im just not getting it. how do you know the charge of each? how does the criss cross method work?
You look at the periodic table. Elements in the 1st vertical row will have a +1 charge, 2nd row a +2 charge, row 13 a +3 charge and so on
for transitional metals, it is hard to tell because they have many, but there are some that in nature tend to have/are more abundant than others such as Fe. It tends to be Fe 2+ ion that stick together to another element. if it were Fe 3+, the question would be say it or your professor would mention it. BUT there are some common elements like group I A and II A that will always have the same charge. Those you must memorize it. it is like a person's name. They will always be called by their first name. They will have nicknames, but only few people say it because they are close to that person, not any random person would know if they could call them by their nickname.
when do you learn in high school? which grade?
bruh we are doing this in middle school :((((
Grade 11 or 10
im doing this in general chem in college
wait how did he produce water by H2 and OH? Shouldn't he have produced H3O and not H2O?
Oliver Abbott look up balancing vids, because the H2 in the reactant side has the 2 because of sulphate that has a charge of two, while when he combined OH with a charge of -1 with H, cross cross the charges and they will cancel out giving us h2o, and that’s why by then end we balance so the product side fits the reactant , I know terrible explaining I’m sorry but watching a balancing video will help
🎉