Re: Chemistry Lab C
Posted: October 26th, 2018, 5:30 am
Dinoswarleafs wrote:Cool. Sorry about that :/Jacobi wrote:Volume of Object = 12.0 mL Density = m/V = 8.7 g/mL = 8700 kg/m^3
Give an element for n-type doping w/ Silicon
Arsenic?
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Re: Chemistry Lab C
Posted: October 26th, 2018, 7:26 am
Oops sorry. Havent done this before D:Jacobi wrote: Usually, the person who answered correctly asks the next question.
Re: Chemistry Lab C
Posted: October 28th, 2018, 8:32 am
What is the pH of a mixture of 
molar ammonium with 
molar ammonia in aqueous sol'n? Ammonium has a 
of 9.20.
Re: Chemistry Lab C
Posted: October 28th, 2018, 7:45 pm
Jacobi wrote:What is the pH of a mixture of
[img]https://cdn.discordapp.com/attachments/294282012146139147/506294811070824468/20181028_213345.jpg[/img]
Re: Chemistry Lab C
Posted: October 29th, 2018, 6:53 am
The image didn't load for me.Dinoswarleafs wrote:Jacobi wrote:What is the pH of a mixture ofYou made me realize on the UT inv yesterday I put the formula for ammonia as a base instead of ammonium dissociating. I was one off from placing. AAAAAAAAAAAAAAAAAAAAAAAAA[img]https://cdn.discordapp.com/attachments/294282012146139147/506294811070824468/20181028_213345.jpg[/img]
Re: Chemistry Lab C
Posted: November 5th, 2018, 5:17 pm
Jacobi wrote:What is the pH of a mixture of
6.2
Re: Chemistry Lab C
Posted: November 6th, 2018, 8:11 am
greenmilktea wrote:Jacobi wrote:What is the pH of a mixture ofA solution of a diprotic acid is standardized by titration with 0.20M NaOH. Calculate the molarity of the acidic solution if 30.24mL of the NaOH solution is required to completely neutralize 14.25mL of the acid solution.6.2
.212M
Re: Chemistry Lab C
Posted: December 18th, 2018, 11:08 pm
I guess I will bump with a question.
Which of the hydrohalic acids are the strongest? Justify your answer.
Which of the hydrohalic acids are the strongest? Justify your answer.
Re: Chemistry Lab C
Posted: January 20th, 2019, 10:03 pm
No one's answered, so I'll go--HI.whythelongface wrote:I guess I will bump with a question.
Which of the hydrohalic acids are the strongest? Justify your answer.
Rule of strengths: ARIO (atom holding the charge, resonance, inductive effects, orbital), in that order. Usually you only get to A with mineral acids, since the proton is often attached to different Hs.
Since F, Cl, Br, I are all in the same family, electronegativity is not the main factor. What matters is bond dissociation energy. The H-I bond is easier to break, so deprotonation is easier.
Also--the strength of an acid depends on the stability of its conjugate base. I- is the most stable since it's the largest. They all have a -1 charge. I- is the largest, so the negative charge is distributed over a larger space and leads to greater stability. My turn: HCl and HBr have the same acid strength in water, but they are clearly not the same strength. (They have different pKas). Why is this the case?
Re: Chemistry Lab C
Posted: January 28th, 2019, 2:19 pm
This is due to the leveling effect. In water, all the acid's strengths are leveled to H3O+, and since both completely dissociates, their strengths are leveled to that of hydronium ion. To see the difference in strength, one can use different solvent such as ammoniaprimitive_polonium wrote:No one's answered, so I'll go--HI.whythelongface wrote:I guess I will bump with a question.
Which of the hydrohalic acids are the strongest? Justify your answer.
Rule of strengths: ARIO (atom holding the charge, resonance, inductive effects, orbital), in that order. Usually you only get to A with mineral acids, since the proton is often attached to different Hs.
Since F, Cl, Br, I are all in the same family, electronegativity is not the main factor. What matters is bond dissociation energy. The H-I bond is easier to break, so deprotonation is easier.
Also--the strength of an acid depends on the stability of its conjugate base. I- is the most stable since it's the largest. They all have a -1 charge. I- is the largest, so the negative charge is distributed over a larger space and leads to greater stability. My turn: HCl and HBr have the same acid strength in water, but they are clearly not the same strength. (They have different pKas). Why is this the case?