Acids and Bases
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Re: Acids and Bases
Phoebe 1H wrote:Also, what does amphiprotic mean?
it means that it is able to react as both an acid and a base since it can donate and accept a proton
Re: Acids and Bases
505968894 wrote:Is a negative pH possible?
even though the scale is usually 0-14, it is possible for pH to be negative.
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Re: Acids and Bases
505801516 wrote:505968894 wrote:Is a negative pH possible?
even though the scale is usually 0-14, it is possible for pH to be negative.
Considering the pH scale is a logarithmic scale, it's not possible for the value of a log to be negative. A zero on the pH scale is the log of 1, which means the concentration of H3O+ is 1.
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Re: Acids and Bases
"How do you know if a compound is acidic or basic?"
I don't know how to reply to comments directly but for this question, I am pretty sure you need to figure out the pH level for the compound and see if it is above or below 7. Above makes it basic and below makes it acidic!
I don't know how to reply to comments directly but for this question, I am pretty sure you need to figure out the pH level for the compound and see if it is above or below 7. Above makes it basic and below makes it acidic!
Re: Acids and Bases
Emily Lam 2H wrote:Does anyone know if we have to memorize strong acids and bases or will it be provided for us?
I believe we won't have to memorize them and we will be provided with them.
Re: Acids and Bases
505968894 wrote:Can you classify acids as strong or weak from their formulas alone?
You can't classify acids as strong or weak from their formulas alone. However, you can memorize the strong and weak acids provided to us then recognize them from the formulas provided by the question.
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Re: Acids and Bases
505968894 wrote:How can you tell if a compound is acidic or basic?
If a compound is acidic, it will usually have a hydrogen. If a compound is basic, it will usually have hydroxide. However, the best way to tell would be to calculate the pH!
Last edited by Julia Mizzi 2I on Sun Jan 22, 2023 10:11 pm, edited 1 time in total.
Re: Acids and Bases
Bella Valente 2K wrote:If a temperature is not given, can we assume we are solving at 25 degrees celcius?
Yes; 25 degrees Celsius is the standard.
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Re: Acids and Bases
505968894 wrote:Is a negative pH possible?
A negative pH is technically possible if the molarity of hydrogen ions is large enough, however, in most examples I believe we will only see pH values from 0-14 as that is the typical pH scale
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Re: Acids and Bases
Nicole Pablico wrote:How to determine the change in concentration when making the ICE table?
The change in concentration is usually represented by the variable x in the ICE tables. You would then subtract x from the reactants and add x to the products as products are being formed in the reactions.
Re: Acids and Bases
Is knowing if an acid/base is strong or weak relevant to solving any specific problems in 14B or is it just extra information?
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Re: Acids and Bases
405735471 wrote:Where do we find the answers to the recommended practice questions from the book?
It's in the "back matter" section of the book and then look under "odd number exercises" and scroll down to find the problem you're looking for
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Re: Acids and Bases
Levon_Avedian_2H wrote:How do acids and bases relate with pH levels and substance concentrations?
Acids have a pH level below 7, while bases have a pH level above 7. Also if a solution is diluted so the concentration is less, the pH will decrease as the concentration of hydrogen ions decreases
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Re: Acids and Bases
505968894 wrote:Is a negative pH possible?
A negative pH is possible! Although I believe it’s beyond the scope of this class?
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Re: Acids and Bases
Phoebe 1H wrote:Also, what does amphirotic mean?
Hello, so It is basically describing an element that can donate and accept a proton and in turn will be able to react as an acid and base. Typically an amphirotic substance typically contains a hydrogen atom
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Re: Acids and Bases
alyssa wrote:Is knowing if an acid/base is strong or weak relevant to solving any specific problems in 14B or is it just extra information?
I believe it matters in calculating concentrations after a reaction has completed since a strong base or acid will completely dissociate into its ionic components.
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Re: Acids and Bases
Hoang Nguyen 3H wrote:Emily Lam 2H wrote:Does anyone know if we have to memorize strong acids and bases or will it be provided for us?
There should be a list provided for us.
Although Professor Lavelle provided us with a list of strong/weak acids and bases, if I remember correctly, we are still required to be able to identify them on the midterm and final.
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Re: Acids and Bases
alyssa wrote:Is knowing if an acid/base is strong or weak relevant to solving any specific problems in 14B or is it just extra information?
Because weak acids and bases do not completely disassociate in a reaction while strong acids and bases completely disassociate, there are certain problems we can only solve with weak acids and bases. For example, we went over what percent ionization is and how to calculate it in weak acid and base reactions. This value essentially tells us the percentage that the reaction will create the ion(s).
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Re: Acids and Bases
Cara_Holden_3A wrote:In which situations does an acid or base completely dissociate?
My TA gave us a sports analogy that I thought would be good to share, here it is:
Acid = quarterback
Base = receiver
Strong acid: good QB with high pass rate & lets go of the ball (H+)
Strong base: good receiver that holds onto the ball until touchdown (reaction)
Weak acid: bad QB with low pass rate & holds onto the ball (H+)
Weak base: bad receiver that drops the ball before touchdown (reaction)
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Re: Acids and Bases
There is a section under 14A. There are various videos and links for acids and bases in 14B though.
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Re: Acids and Bases
How do you know if the change in ICE is a -x or +x if given molar concentrations for all three substances?
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Re: Acids and Bases
Cara_Holden_3A wrote:In which situations does an acid or base completely dissociate?
Strong acids and bases dissociate completely.
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Re: Acids and Bases
Cara_Holden_3A wrote:In which situations does an acid or base completely dissociate?
I believe strong acids and bases completely dissociate while weak bases don't completely dissociate 2
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Re: Acids and Bases
Ruby Stuart 1I wrote:How do you know if the change in ICE is a -x or +x if given molar concentrations for all three substances?
Typically, a - is used for the reactants and the + is used for the products of molar concentrations. Also, the coefficient of the change in ICE tables would be put in between the +/- and x of each substance.
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Re: Acids and Bases
Roni Nissim 1D wrote:What is the difference between K and Q reaction quotients. Does K only apply for reactions at equilibrium?
Q is a quantity that changes as a reaction system approaches equilibrium. K is the numerical value of Q at the "end" of the reaction, when equilibrium is reached.
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Re: Acids and Bases
Maya_Panozzo_2D wrote:In the equation where it says that pKw = pH + pOH = 14 at 25(degrees c) what does the p mean in the pKw section? And just to clarify the Kw refers to the equilibrium constant when water is involved right?
p just means to take the -log of whatever comes after it. pH would mean to take -log(H+ concentration) and the same with OH and Kw. you would be taking the -log of the Kw constant. Kw is the constant for H+ and OH+ concentrations being multiplied together.
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Re: Acids and Bases
Maya_Panozzo_2D wrote:In the equation where it says that pKw = pH + pOH = 14 at 25(degrees c) what does the p mean in the pKw section? And just to clarify the Kw refers to the equilibrium constant when water is involved right?
p means that you're basically taking the negative log of Kw. So -log[1.0 *10^-14]=14
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Re: Acids and Bases
505968894 wrote:Is a negative pH possible?
Yeah, I think in lecture Dr. Lavelle said it is possible when the concentration of H3O is greater than 1.0 M. However, in most biological situations, the pH range is 0 to 14.
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Re: Acids and Bases
Cara_Holden_3A wrote:In which situations does an acid or base completely dissociate?
When an acid or base is classified as strong, it will completely dissociate.
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Re: Acids and Bases
Nicole Pablico wrote:How to determine the change in concentration when making the ICE table?
So basically you add -x per mole from the initial concentrations given. For the starting condition of 0, you add x per mole. Not sure if that makes sense but its just a change of x per mole and the direction usually goes from higher concentrations to lower concentrations.
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Re: Acids and Bases
405735471 wrote:Where do we find the answers to the recommended practice questions from the book?
If you go to the Home page of BruinLearn for this class, the answers to the practice questions are at the link called "Chemical Principles, 7th Edition, Student Solutions Manual (Fundamentals, 1-7, 9)" Hope this helps!
Re: Acids and Bases
Do the weak acids not get accounted for when we calculate the K of the equation? Or does that just apply to solids?
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Re: Acids and Bases
amphiprotic means that a species can both donate or accept a proton. Water is an example, in autoprotolysis reactions.
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Re: Acids and Bases
Emily Lam 2H wrote:Does anyone know if we have to memorize strong acids and bases or will it be provided for us?
The list of strong/weak acids and bases can be found on the class website under learning outcomes titled "List of Acids and Bases."
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Re: Acids and Bases
705995679 wrote:Do the weak acids not get accounted for when we calculate the K of the equation? Or does that just apply to solids?
I believe that all aqueous solutions, including weak acids/ bases are accounted for when we calculate K because they contribute to the overall concentration at equilibrium (even if the concentration is small). Only solids and liquids are discounted from the equation.
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Re: Acids and Bases
Strong acids and bases ionize fully in an aqueous solution. Weak acids and bases also ionize, but only partially and the reaction is reversible.
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Re: Acids and Bases
405735471 wrote:Do we need to memorize certain acids or bases or will we be told whether or not it is a strong acid or base?
I think memorizing them will certainly make these problems easier to do. The professor recently emailed a list of all the strong acids and bases and here is a link to a quizlet to study them! https://quizlet.com/_cob0nb?x=1jqt&i=40ipnb
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Re: Acids and Bases
Does anyone know where to find the list of acids and bases we are responsible for memorizing? I'm at a loss.
EDIT: pardon me, missed the post directly above mine! Looks like there is a quizlet at https://quizlet.com/766418951/acids-and ... ds/?x=1jqt
EDIT: pardon me, missed the post directly above mine! Looks like there is a quizlet at https://quizlet.com/766418951/acids-and ... ds/?x=1jqt
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Re: Acids and Bases
Hi folks, I have a quick question regarding the ICE table / quadratic equation method. I must have forgotten to write it down, what is the maximum K value from which it is acceptable to assume x is near enough to round to zero?
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Re: Acids and Bases
Also, a secondary question also regarding the ICE table / quadratic equation process; I just wanted to double check, we ignore any negative values we get from solving the quadratic equation, correct?
Re: Acids and Bases
Can someone explain how to tell whether an approximation for concentration is valid or not? What are the parameters to check if it was okay to do?
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Re: Acids and Bases
Maya_Panozzo_2D wrote:Lavalle sent an email out recently saying that it will be provided to us and gave a list.
Should we memorize the list?
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Re: Acids and Bases
705995679 wrote:Do the weak acids not get accounted for when we calculate the K of the equation? Or does that just apply to solids?
Hi, I think that just applies to solids and liquids. I believe whether or not you take into account a weak acid or weak base depends on if you are trying to find Ka or Kb.
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Re: Acids and Bases
How do you know whether a compound is an acid or a base? Following that, how do you know whether it produces OH- or H3O?
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Re: Acids and Bases
405735471 wrote:Where do we find the answers to the recommended practice questions from the book?
The syllabus has all of the recommended practice problems for each section. You can find the syllabus on the class website.
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Re: Acids and Bases
Roni Nissim 1D wrote:Phoebe 1H wrote:Also, what does amphiprotic mean?
Amphiprotic is when a compound is able to accept a proton and donate a proton. Basically this compound can act as both an acid and a base.
An example is water. In the presence of an acid it accepts a proton. In the presence of a base it donates a proton
Re: Acids and Bases
Aanchal Kasargod 1H wrote:I just had a quick question about conjugate acids and bases. I just wanted to know how we know which compound is the conjugate acid/base in the chemical reaction and also how this concept may come up when solving problems?
The question might ask you to work backwards and give you the x value for the conjugate base/acid and you have to fill in the ICE chart to find the initial concentration. I think #5 for the HW teaches you how to work backwards in this kind of problem.
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Re: Acids and Bases
405735471 wrote:Do we need to memorize certain acids or bases or will we be told whether or not it is a strong acid or base?
We need to memorise. Here's a list: All group 1 and 2 hydroxides are strong bases, the others are weak.
HCl, HBr, HI, HClO4, HClO3, HNO3, H2SO4 are all strong acids, the others are weak
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Re: Acids and Bases
I was wondering on how we're supposed to know when to use either the Bronsted-Lowry Definition of an Acid/Base, and the Lewis Definition. Help would be greatly appreciated :)
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Re: Acids and Bases
Question:
HClO is a weak acid ( Ka=4.0×10−8 ) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.072 M in NaClO at 25 °C?
When I was doing this, I was confused about how to set up the equation and how they were interacting.
This is what I have so far:
I had the reaction as HClO (aq) + H20 (l) <--> ClO- + H30+ is this correct so far? (Ka)(Kb) = 1.0x10^-14
Kb = 1.0x10^-14 / 4.0×10−8
(can you do this only with water? is this only Kw?) do I need to do
Then I tried to set up an ICE table: make it pKa to pKb to Kb?
HClO ClO- H30+
I 0 .072 0 or .072
C x -x -x Where do I go from here? What is incorrect with what I am doing?
E. x. .072-x. .072-x (or -x?)
HClO is a weak acid ( Ka=4.0×10−8 ) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.072 M in NaClO at 25 °C?
When I was doing this, I was confused about how to set up the equation and how they were interacting.
This is what I have so far:
I had the reaction as HClO (aq) + H20 (l) <--> ClO- + H30+ is this correct so far? (Ka)(Kb) = 1.0x10^-14
Kb = 1.0x10^-14 / 4.0×10−8
(can you do this only with water? is this only Kw?) do I need to do
Then I tried to set up an ICE table: make it pKa to pKb to Kb?
HClO ClO- H30+
I 0 .072 0 or .072
C x -x -x Where do I go from here? What is incorrect with what I am doing?
E. x. .072-x. .072-x (or -x?)
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Re: Acids and Bases
Will the acid and base list that Professor Lavelle provided be the only possible strong/weak acids and bases that can come up on a test, or are they simply a list of the most popular ones?
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Re: Acids and Bases
405735471 wrote:Where do we find the answers to the recommended practice questions from the book?
You could find the recommended practice problems on page 3 of the syllabus.
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Re: Acids and Bases
Maya_Panozzo_2D wrote:In the equation where it says that pKw = pH + pOH = 14 at 25(degrees c) what does the p mean in the pKw section? And just to clarify the Kw refers to the equilibrium constant when water is involved right?
p in most situation is just another way to say -log. So, for example the pH, as we know is the -log (H+). This also goes for pOH and pKw.
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Re: Acids and Bases
alyssa wrote:Is knowing if an acid/base is strong or weak relevant to solving any specific problems in 14B or is it just extra information?
It is helpful depending on the question. If the reaction involves a strong base or acid, then we know that the entire compound will dissociate into salt. However, when dealing with a weak acid or base, then it does not completely dissociate and we would have to calculate exactly how much dissociated in order to proceed with the problem.
Re: Acids and Bases
405735471 wrote:Where do we find the answers to the recommended practice questions from the book?
They are on canvas under welcome and getting started and they are labeled "Chemical Principles, 7th Edition, Student Solutions Manual (Fundamentals, 1-7, 9)"
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Re: Acids and Bases
Nicole Pablico wrote:How to determine the change in concentration when making the ICE table?
It’s basically all about understanding the reaction equation provided. You make columns for each reactant and product, besides H2O and then if it is a reactant it is most likely a -x value and with a product it is a +x value, the number (if there is one) in front of the X is determined by the equation, for example if there are 2NH3 as the reactant, then the x value will be -2x. Then the x values are added to the initial concentrations if you know them and then are plugged into the equation.
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Re: Acids and Bases
When given a problem with Kb instead of Ka does this change the order in which you complete the problem or do all of the steps pretty much stay the same?
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Re: Acids and Bases
Maya_Panozzo_2D wrote:In the equation where it says that pKw = pH + pOH = 14 at 25(degrees c) what does the p mean in the pKw section? And just to clarify the Kw refers to the equilibrium constant when water is involved right?
Kw is the equilibrium constant for pure water and pKw comes from the equation pKw=-logKw, which helps calculate pH or pOH
Re: Acids and Bases
Abigail S 2C wrote:When given a problem with Kb instead of Ka does this change the order in which you complete the problem or do all of the steps pretty much stay the same?
All steps are pretty much the same except when you get to the final steps and have to calculate either pH or OH or anything else they ask
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Re: Acids and Bases
Can you use the blank equation HA + H20 <=> H3O+ + A- for any acid problem and A- + H2O <=> HA+ + OH- for any base problem?
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Re: Acids and Bases
Suraj Kulkarni 2B wrote:Does anyone have a list of the acids and bases we are supposed to know?
https://lavelle.chem.ucla.edu/wp-conten ... _Bases.pdf
Lots of people have been saying that you just really need to memorize strong acids and bases and then you'll be fine.
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Re: Acids and Bases
Damin Rawlins 3B wrote:I was wondering on how we're supposed to know when to use either the Bronsted-Lowry Definition of an Acid/Base, and the Lewis Definition. Help would be greatly appreciated :)
Both are just different types of definitions of how there can be an acid or base reaction. I think both definitions are more of a conceptual idea than something that you need to know for calculating purposes.
Re: Acids and Bases
Can someone explain 6D15 part b? I thought we can eliminate Cl- from the equation, but then if we consider it to be a strong acid, wouldn't the x value just be 0.055? However, that does not yield the correct answer.
Re: Acids and Bases
505968894 wrote:Is a negative pH possible?
I think technically you can calculate one, but pretty sure for our class we won't have a problem that will yield a neg pH.
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Re: Acids and Bases
In the textbook problem 6D.9, it asks us to use the percentage deprotonation (2.4%) of benzoic acid in a 0.110 M solution to find pH and Ka.
Does it matter if we put (1-0.024)(0.110) or just (0.110-0.00264). I know it is the same answer either way but I was wondering if we should follow the expression in the ice table which is 0.110-x or do it the way in the key on canvas (which is (1-0.024)(0.110))
Does it matter if we put (1-0.024)(0.110) or just (0.110-0.00264). I know it is the same answer either way but I was wondering if we should follow the expression in the ice table which is 0.110-x or do it the way in the key on canvas (which is (1-0.024)(0.110))
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Re: Acids and Bases
505968894 wrote:How can you tell if a compound is acidic or basic?
I think it might just be something you have to memorize. Dr. Lavelle gave us a list of common acids and bases and my TA told us to memorize them.
Re: Acids and Bases
Phoebe 1H wrote:Also, what does amphiprotic mean?
Amphiprotic is the ability to respond as both an acid and a base because it can both donate and take a proton.
Re: Acids and Bases
Maya_Panozzo_2D wrote:Are the pH and the pKa equal? Also, the pOH and pKb?
No, pH is equal to the sum of the pKa value and the log of the conjugate base concentration divided by the weak acid concentration.
Re: Acids and Bases
Cara_Holden_3A wrote:In which situations does an acid or base completely dissociate?
While weak acids and bases only partially dissociate, strong acids and bases entirely do so.
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Re: Acids and Bases
Emily Lam 2H wrote:Does anyone know if we have to memorize strong acids and bases or will it be provided for us?
I believe we have to memorize it! and there are a few mnemonics which could help you memorize the strong acids! For example, one of them is So (H2SO4) I (HI) Brought (HBr) No (HNO3) Clean (HCl) Clothes (HClO4).
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Re: Acids and Bases
Do we need to memorize only strong acids and bases or memorize both strong and weak acids and bases?
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Re: Acids and Bases
Jake1K wrote:What is an acid and a Base? How can you tell the difference? Have a nice day.
The pH of an acid will be less than 7 while the pH of a base will be greater than 7.
The pH of an acid is calculating by finding -log of the hydronium ion concentration in the solution. The pH of a base can be found by first calculating the pOH (-log of hydroxide ion concentration in solution). After finding the pOH, the pH an be calculated by solving 14 - pOH.
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Re: Acids and Bases
Do we need to memorize the list of acids and bases that the professor provided to us?
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Re: Acids and Bases
Keanu Ngo 3B wrote:How can you tell if a salt is acidic or basic?
One can tell if a salt is acidic when a strong acid reacts with a weak base. A salt is basic when a strong base reacts with a weak acid. When a strong base interacts with a strong acid, the salt is neutral.
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Re: Acids and Bases
I appreciate all the help, and thanks for answering my question about the principle.
Re: Acids and Bases
Maya_Panozzo_2D wrote: Lavalle sent an email out recently saying that it will be provided to us and gave a list.
He sent an email with the list but it seemed as though the list wouldn't be provided to us and we would have to memorize them. Did he specifically clarify this?
Re: Acids and Bases
505968894 wrote:How can you tell if a compound is acidic or basic?
The Lewis theory states that acids accept elections and bases donate electrons.
Re: Acids and Bases
Do we have to memorize the chemical reaction for a certain element (for example: NH4Cl)?
Re: Acids and Bases
Phoebe 1H wrote:Also, what does amphiprotic mean?
Amphiprotic just means that the molecule is able to both donate and accept a proton. Therefore it is able to react as both an ACID and a BASE
Re: Acids and Bases
906023369 wrote:Do we only approximate when the value is less than 10^-3?
That's the rule of thumb that Lavelle gave in class. However, there were some problems on the Week 2 achieve homework where I applied that rule and It didn't work for me. What I've been doing now to make sure that I get the question correct is to approximate regardless of the 10^-n value and to check the percentage ionization. If it is below 5% you should be good to approximate, if it is above, stick with the quadratic formula.
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Re: Acids and Bases
You can determine if a compound is acidic or basic by looking at the cation and anion of the compound and seeing what they will form with water (strong/weak acid or strong/weak base). For example, if NaCN is placed in water, NaOH and HCN will form. NaOH is a strong acid while HCN is a weak base, indicating that NaCN is basic (rather than acidic or neutral).
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Re: Acids and Bases
Keanu Ngo 3B wrote:How can you tell if a salt is acidic or basic?
You can determine if a compound is acidic or basic by looking at the cation and anion of the compound and seeing what they will form with water (strong/weak acid or strong/weak base). For example, if NaCN is placed in water, NaOH and HCN will form. NaOH is a strong acid while HCN is a weak base, indicating that NaCN is basic (rather than acidic or neutral).
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Re: Acids and Bases
906023369 wrote:Do we have to memorize what a monoprotic acid is for the test?
I believe that you should memorize what it is because there is a chance that a problem may not state a specific acid in which case you will have to just use the equation HA + H20 ⇌ A- + H3O+
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Re: Acids and Bases
Maya_Panozzo_2D wrote:Can you use the blank equation HA + H20 <=> H3O+ + A- for any acid problem and A- + H2O <=> HA+ + OH- for any base problem?
You can only use those equations if the base or acid is monoprotic.
Re: Acids and Bases
When we are given a situation where we have to find pOH using pOH + pH = 14 to calculate one of them and the temperature is not at 25c, how do we solve it?
Re: Acids and Bases
If the acid or base is not monoprotic, will we be given the dissociation equation?
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Re: Acids and Bases
When are we allowed to make the approximation that the initial concentration(s) of reactants don't change that much?
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Re: Acids and Bases
906023369 wrote:Do we have to memorize what a monoprotic acid is for the test?
I believe so. Although a monoprotic acid is just one that donates only one proton meaning it can only dissociate once. Although you need to know what this is most acids are monoprotic and only dissociate once.
Re: Acids and Bases
Can someone explain what a protonation state is and how to find it? Will this be something to look out for on the midterm
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