Post by: spectroscopy on September 17, 2013, 07:16:47 pm
in an experiment 20.00mL of hydrochloric acid was standardised by titration with a solution of 0.104M sodium carbonate
the average titre of socium carbonate was 11.6ml
find the concentration of this solution of hydrochloric acid
Post by: RKTR on September 17, 2013, 07:59:53 pm
2HCl(aq) + Na2CO3(aq) --> 2NaCl(aq) + H2O(l) + CO2(g)
from the equation,we can see that 2 mol of HCl reacts with 1 mol of Na2CO3
ratio 2 : 1
find n of Na2CO3 n=cv n=0.104 x ( 11.6/1000) = 1.21 x 10^-3 mol
n of HCl = 2 x n of Na2CO3 = 2(1.21 x 10^-3) mol
= 2.42 x 10^-3 mol
n=cv 2.42 x 10^-3 = c ( 20.00/1000)
c=0.121 M
Post by: RazzMeTazz on January 22, 2014, 10:30:05 pm
Thankyou! :)
Post by: brightsky on January 22, 2014, 10:56:32 pm
Post by: RazzMeTazz on January 23, 2014, 12:48:15 am
1 mol of sodium atoms = 6.02 * 10^(23) sodium atoms. it follows that 1.0 * 10^(20) sodium atoms = (1.0 *10^(20))/(6.02 * 10^(23)) mol of sodium atoms.
Thankyou so much! :)
Post by: RazzMeTazz on February 02, 2014, 10:24:05 am
We are doing a prac sac in chemistry and our teacher said that we would be expected to know general theory about doing practical reports and answering questions about it :)
Has anyone does this type of thing in chemistry before?
What would it require us to know?
Just stuff like what the limitations are and what was the variable?
Thanks!
Post by: alchemy on February 02, 2014, 10:36:14 am
Hi,
We are doing a prac sac in chemistry and our teacher said that we would be expected to know general theory about doing practical reports and answering questions about it :)
Has anyone does this type of thing in chemistry before?
What would it require us to know?
Just stuff like what the limitations are and what was the variable?
Thanks!
Have a look at this for an example, it might help: http://www.vcehelp.com.au/preparing-artificial-fragrances-and-flavours-vce-chemistry-prac-report-1691/
I've been told that criteria for Prac reports vary from school to school. So it's best if you ask your teacher for more details regarding this.
Post by: RazzMeTazz on February 04, 2014, 08:23:07 pm
Did he propose that they were moving in random circular orbits around the nucleus?
Did he say that electrons belonged to random circular orbits?
Thanks!
Post by: bucklr on February 04, 2014, 09:15:38 pm
Hi, I was wondering what did Rutherford's model of the atom say about electrons?Your right. His model disproved J.J Thompson's plumb pudding model where electrons where arranged in non-random rings.
Did he propose that they were moving in random circular orbits around the nucleus?
Did he say that electrons belonged to random circular orbits?
Thanks!
Rutherford's model says that electrons move randomly, and that the an atom's mass is concentrated in the centre of the atom - the nucleus. Electrons were suggested by him to move randomly in rings of different energy levels.
Post by: RazzMeTazz on February 04, 2014, 10:48:26 pm
Your right. His model disproved J.J Thompson's plumb pudding model where electrons where arranged in non-random rings.
Rutherford's model says that electrons move randomly, and that the an atom's mass is concentrated in the centre of the atom - the nucleus. Electrons where suggested by him to move randomly in rings of different energy levels.
Thankyou so much! :D
Post by: MNM101 on February 07, 2014, 09:46:04 pm
Post by: grannysmith on February 07, 2014, 10:22:01 pm
Hi I'm stuck on a chem unit 1 and 2 question also. We were learning about shells and there subs he'll and within the sub jells contains s,p,d,f but I'm really confused about all this plus the orbitals so if anyone can help me out that'd be greatSchrodinger's model says that there are different energy levels (shells if you like) in which electrons can occupy. Whereas Bohr's model says that electrons of the same shell are of equal energy levels, Schrodinger's states that within these shells exist subshells. Electrons of different sub shells have varying energy levels, and these are termed s, p, d and f.
The s sub shell contains 1 orbital; p contains 3; d contains 5 and f contains 7.
An orbital can only hold a maximum of 2 electrons. Thus, the s sub shell has a maximum of 2 electrons; p has a max of 6 etc..
When electrons are given enough energy (e.g. heat), they can jump to higher energy levels (they can go from, say, 1s to 2p). However, electrons always want to be at their lowest energy state, their 'ground state'. That is, as close to the nucleus as possible. When they go from a higher energy level to a lower energy level, the energy must be emitted somehow. Usually, this is given of as a photon, which is essentially a packet of light.
Guys, correct me if I'm wrong. I've only learnt this ever so recently :p
Post by: RazzMeTazz on February 18, 2014, 10:21:37 pm
Why does the core charge of an atom increase across a period, and stay the same as you go down a group?
THanks
Post by: alchemy on February 18, 2014, 11:23:37 pm
Hey,
Why does the core charge of an atom increase across a period, and stay the same as you go down a group?
Thanks
Yes. The core charge is basically the number of valence electrons, meaning they increase as you go across a period, and stay the same as you go down a group.
Post by: RazzMeTazz on March 06, 2014, 10:39:17 am
Does it cause other substances to gain electrons? Or does it gain electrons itself?
thanks!
Post by: jgoudie on March 06, 2014, 05:06:23 pm
In an oxidation reaction electrons are lost by the reductant causing the oxidant to under go reduction and gain electrons.
Electrons are transferred from the reductant to the oxidant.
If you read through it slowly it makes sense.
I know if something is reduced, it has gained electrons but what does a reducing agent do?
Does it cause other substances to gain electrons? Or does it gain electrons itself?
thanks!
Post by: RazzMeTazz on March 06, 2014, 05:34:37 pm
The reducing agent is called the reductant, it loses electrons in an oxidation reaction.
In an oxidation reaction electrons are lost by the reductant causing the oxidant to under go reduction and gain electrons.
Electrons are transferred from the reductant to the oxidant.
If you read through it slowly it makes sense.
Thanks so much! :)
Post by: Tyleralp1 on March 06, 2014, 07:00:17 pm
"Nitrogen in the air may react with Magnesium. Explain how this may effect results"
Could someone please provide a nice answer to this, or at least point me in the right direction by listing a few pointers of what to mention.
Thanks! :)
Post by: jgoudie on March 06, 2014, 11:04:45 pm
If Magnesium reaction with nitrogen, it forms Mg3N2, think about the charges involved in the ionic bonding.
Now being that nitrogen is less heavy that oxygen and that the ratio is in Mg3N2 is more favourable to magnesium, if any magnesium forms Magnesium nitride instead of magnesium oxide, you will get less mass in your end product.
This will mean you will end up calculating less oxygen is formed than if the atmosphere was pure oxygen, this less mass will lead you to calculate a greater ratio of Magnesium to Oxygen. So you might end up with Mg2O or Mg3O or Mg3O2 or something like that.
Hope that makes some sense.
Here is a question we have to complete as part of a prac report on Determining the Empirical Formula of Magnesium Oxide...
"Nitrogen in the air may react with Magnesium. Explain how this may effect results"
Could someone please provide a nice answer to this, or at least point me in the right direction by listing a few pointers of what to mention.
Thanks! :)
Post by: Tyleralp1 on March 06, 2014, 11:23:36 pm
Also another question:
Differentiate Relative Atomic Mass, Relative Molecular Mass, Molar Mass as well as amu, grams, grams/mol.
Post by: RazzMeTazz on March 09, 2014, 11:01:16 pm
? I thought Avogadro came up with the mole unit..
Post by: grannysmith on March 10, 2014, 11:43:36 am
What is the difference in the definition between a 'mole' and 'Avogadro's constant'Same thing
? I thought Avogadro came up with the mole unit..
Post by: alchemy on March 10, 2014, 12:41:28 pm
What is the difference in the definition between a 'mole' and 'Avogadro's constant'
? I thought Avogadro came up with the mole unit..
One mole contains the same number of elementary particles (atoms) that is expressed by the number that's 'Avagadro's Constant'. So yes, "a" (one) mole is the same as Avagadro's constant, as the mole is a SI unit which measures the number of particles in a particular substance. However, 2 moles means the number (Avagadro's constant) must be doubled if you want to find the number of particles. 3 moles of a substance would contain 3 times as many particles as 1 mole, and so on...
Post by: RazzMeTazz on March 20, 2014, 07:19:18 pm
An oxide of Copper is heated in a stream of hydrogen until only the copper remains according ti the equation:
CuxO(s) + H2(g) --> XCu(s) + H2O(l)
the data for the experiment are given in the table below. Calculate the empirical formula of the oxide of copper.
Item and mass:
Crucible - 27.002g
Crucible plus contents before heating - 27.128g
Crucible plus contents after heating - 27.114g
Post by: darka221 on March 20, 2014, 07:40:09 pm
Post by: rhinwarr on March 20, 2014, 08:37:40 pm
Post by: IndefatigableLover on March 20, 2014, 09:46:43 pm
I'm kind of stuck with this question..Alright so if we want to find the mass of CuxO then we subtract the mass of crucible with contents before heating with crucible to find that out (27.128 - 27.002 = 0.126g)
An oxide of Copper is heated in a stream of hydrogen until only the copper remains according ti the equation:
CuxO(s) + H2(g) --> XCu(s) + H2O(l)
the data for the experiment are given in the table below. Calculate the empirical formula of the oxide of copper.
Item and mass:
Crucible - 27.002g
Crucible plus contents before heating - 27.128g
Crucible plus contents after heating - 27.114g
To find the mass of copper then we subtract the other one with the mass of the crucible for the weight of Copper (27.114 - 27.002 = 0.112g).
As a result we have the masses of CuxO and Cu so now we can find the weight of oxygen (0.126-0.112=0.014g)
Now to find the empirical formula then we must find the number of moles for Copper in CuxO and the number of moles of Oxygen in CuxO. In this case we'll be dividing the masses of Copper and Oxygen by their molar mass.
(http://latex.codecogs.com/gif.latex?\therefore&space;Moles&space;\&space;of&space;\&space;Copper&space;=\frac{0.012}{63.5}&space;\\\\&space;\therefore&space;Moles&space;\&space;of&space;\&space;Oxygen&space;=&space;\frac{0.014}{16})
Now the next step in finding the empirical formula is t divide all the amounts by the smallest number of moles. In this case we will be dividing the moles of oxygen against copper to determine our empirical formula (since it's the least).
Keeping our fractions before and dividing, you should get an answer of 256/127 which roughly translates to 2.
Therefore for every one oxygen, there are 2 copper atoms.
So then x=2.
(You can kind of see the answer since the charge of oxygen is -2 so we can assume that the charge of Copper must be equal with it).
Post by: RazzMeTazz on March 23, 2014, 08:30:16 pm
Alright so if we want to find the mass of CuxO then we subtract the mass of crucible with contents before heating with crucible to find that out (27.128 - 27.002 = 0.126g)
To find the mass of copper then we subtract the other one with the mass of the crucible for the weight of Copper (27.114 - 27.002 = 0.112g).
As a result we have the masses of CuxO and Cu so now we can find the weight of oxygen (0.126-0.112=0.014g)
Now to find the empirical formula then we must find the number of moles for Copper in CuxO and the number of moles of Oxygen in CuxO. In this case we'll be dividing the masses of Copper and Oxygen by their molar mass.
(http://latex.codecogs.com/gif.latex?\therefore&space;Moles&space;\&space;of&space;\&space;Copper&space;=\frac{0.012}{63.5}&space;\\\\&space;\therefore&space;Moles&space;\&space;of&space;\&space;Oxygen&space;=&space;\frac{0.014}{16})
Now the next step in finding the empirical formula is t divide all the amounts by the smallest number of moles. In this case we will be dividing the moles of oxygen against copper to determine our empirical formula (since it's the least).
Keeping our fractions before and dividing, you should get an answer of 256/127 which roughly translates to 2.
Therefore for every one oxygen, there are 2 copper atoms.
So then x=2.
(You can kind of see the answer since the charge of oxygen is -2 so we can assume that the charge of Copper must be equal with it).
thanks!! so much!! :D great explanation!
Post by: RazzMeTazz on March 23, 2014, 08:32:46 pm
Naturally occuring bromine consists of two isotopes, 79Br and 81Br. However the mass spectrum of bromine molecules, Br2 shows three peaks at relative masses 158, 160 and 162. Give an explanation for this observation
Post by: rhinwarr on March 23, 2014, 08:44:34 pm
79Br-79Br
79Br-81Br
81Br-81Br
Post by: alchemy on March 24, 2014, 08:53:24 pm
Hi guys! Does anybody have worksheets on the mole and mole calculations or know of any good online quizzes, resources etc?? i have a test coming up and I'm looking for some extra revision.Hey jess, you could try this for practice questions: http://www.sciencegeek.net/Chemistry/taters/directory.shtml. They're all relatively easy btw.
And click on the learning outcome links on this page for theory behind it all: http://www.chemguideforcie.co.uk/sect1menu.html#top
Post by: IndefatigableLover on March 24, 2014, 09:15:33 pm
Hey jess, you could try this for practice questions: http://www.sciencegeek.net/Chemistry/taters/directory.shtml. They're all relatively easy btw.ChemGuide is literally something you can't live without when it comes to VCE Chemistry LOL
And click on the learning outcome links on this page for theory behind it all: http://www.chemguideforcie.co.uk/sect1menu.html#top[/b]
It's like your second textbook (only that it's free ;))
Post by: jessica666 on March 24, 2014, 10:17:33 pm
Hey jess, you could try this for practice questions: http://www.sciencegeek.net/Chemistry/taters/directory.shtml. They're all relatively easy btw.
And click on the learning outcome links on this page for theory behind it all: http://www.chemguideforcie.co.uk/sect1menu.html#top
thanks so much!
Post by: jessica666 on March 24, 2014, 10:18:22 pm
ChemGuide is literally something you can't live without when it comes to VCE Chemistry LOL
It's like your second textbook (only that it's free ;))
thanks heaps! didn't know about that! :)
Post by: MNM101 on April 21, 2014, 12:21:18 pm
Post by: IndefatigableLover on April 21, 2014, 12:29:04 pm
Just wondering if an element has low melting temperature does that mean they have a weak force of attraction between the particles that make up the substance?Generally associated with low melting temperatures are gases which have a weak force of attraction between the particles that make up the substance. It goes the opposite way as well where if the force of attraction between particles that make up the substance is strong then it's more likely to be a solid. So in short yes you are right MNM101 :)
Post by: MNM101 on April 21, 2014, 12:30:37 pm
Generally associated with low melting temperatures are gases which have a weak force of attraction between the particles that make up the substance. It goes the opposite way as well where if the force of attraction between particles that make up the substance is strong then it's more likely to be a solid. So in short yes you are right MNM101 :)
Thanks!!
Post by: rhinwarr on April 21, 2014, 12:36:00 pm
Post by: jessica666 on May 12, 2014, 05:43:09 pm
Post by: Einstein on May 12, 2014, 06:28:00 pm
Post by: alchemy on May 12, 2014, 09:38:50 pm
What's the difference between covalent network lattices and covalent layer lattices??
Covalent network lattices consist entirely of very strong carbon-carbon covalent bonds all linked to one another in three dimensions. Hence, a material that consists of a covalent network lattice structure (e.g. diamond) has a very high melting point and doesn't conduct electricity because there are no free moving electrons. It is insoluble in water and organic solvents because no attractions can possibly occur between carbon atoms of the covalent network lattice and solvent molecules.
Covalent layer lattices consist of sheets (layers) of carbon atoms bound together as well, but there is a gap between each of the layers. This characteristic makes a material, such as graphite, have a soft/greasy feel. Graphite has one delocalised electron per carbon atom, allowing it to conduct electricity in 2-dimentions (within sheets, BUT not between them). It has a high melting point as a large amount of energy is required to break the strong covalent bonds between carbon atoms. Another interesting fact about covalent layer lattices is that they have a lower density in comparison to covalent network lattices because of the space in between the sheets.
whats everyone upto in 1/2 chem? we're upto organic chem, nearly done
Almost finished organic chem. Really looking forward to getting Unit 1 over and done with!
Post by: ronniecoollike on May 13, 2014, 05:40:36 pm
Post by: Einstein on May 13, 2014, 08:17:17 pm
I think ionic compounds when put in water dissolve as the electrons break the rigid structure - electrolytes, something along those lines.
Post by: katie101 on June 02, 2014, 07:22:18 am
I was just wondering what your thoughts were on picking up unit 2 chem without doing unit 1?
Post by: IndefatigableLover on June 02, 2014, 05:51:41 pm
Hi GuysKind of depends on what your school has done on for Unit 1 of Chemistry.... for instance if you were at my school then I'd say you'd be okay because we've done all the 'non-calculation stuff' (E.g Organic Chemistry etc.) but haven't touch on the idea of moles which most schools have done (in saying that, majority of people in our cohort do know quite a bit about Chemistry so it's not really that bad).
I was just wondering what your thoughts were on picking up unit 2 chem without doing unit 1?
Have a look at this and check over Unit 1 & Unit 2 and that's pretty much what you 'should' have covered or will cover in Year 11 Chemistry (what you personally learn will be dependant on your school though).
Post by: Einstein on June 04, 2014, 04:43:29 pm
Im really shattered now, the fact that i got that score (my standards are higher), but it is 1/2 after all. Is it worth going over the things i got wrong, i know that i lost a few marks for not knowing ions, but other then that id suspect things to be stupid mistakes. I only studied the week before really briefly and on the day of the exam for 1 and a half hours.
Thanks
Post by: alchemy on June 05, 2014, 08:59:10 pm
just got my exam score back and got low 80s, despite scoring mid 90s all year in SACs. Though i do have a excuse, i had a 3/4 sac on the day of the exam, but i dont know if that would be good enough to compensate for my score.
Im really shattered now, the fact that i got that score (my standards are higher), but it is 1/2 after all. Is it worth going over the things i got wrong, i know that i lost a few marks for not knowing ions, but other then that id suspect things to be stupid mistakes. I only studied the week before really briefly and on the day of the exam for 1 and a half hours.
Thanks
Wait, this is a questions thread right? What's your question?
Post by: IndefatigableLover on June 05, 2014, 09:23:53 pm
Wait, this is a questions thread right? What's your question?
just got my exam score back and got low 80s, despite scoring mid 90s all year in SACs. Though i do have a excuse, i had a 3/4 sac on the day of the exam, but i dont know if that would be good enough to compensate for my score.;)
Im really shattered now, the fact that i got that score (my standards are higher), but it is 1/2 after all. Is it worth going over the things i got wrong, i know that i lost a few marks for not knowing ions, but other then that id suspect things to be stupid mistakes. I only studied the week before really briefly and on the day of the exam for 1 and a half hours.
Thanks
But seriously to answer your question, I think you should be content with your score. You know where you went wrong so check if it's a necessary part of the VCE course (which memorising ions is) so you will need to know your ions properly.
Post by: alchemy on June 06, 2014, 08:57:58 pm
The number of people complaining here about the relatively high scores they get is too damn high! :P
Post by: RazzMeTazz on June 19, 2014, 08:18:19 pm
Post by: jgoudie on June 20, 2014, 08:21:09 am
Another good example is oil and water. Put a cup of each on the stove and see which one gets hotter quicker. (oil wins every time)
Waters SHC is 4.18, most other things are around 2 and below.
(yeah i know there are currents and all that jazz in play as well, but you get the idea)
Does water have a higher heat capacity than most other common molecular substances?
Post by: RazzMeTazz on June 23, 2014, 05:49:38 pm
But why is water not a polyatomic ion?
The molecule itself has 10 protons and 8 electrons,
Shouldn't it be positively charged then?
Post by: RazzMeTazz on June 23, 2014, 07:33:35 pm
Post by: IndefatigableLover on June 23, 2014, 07:36:33 pm
This might sound silly,Well Hydrogen has one proton and one electron and then Oxygen has 8 Protons and Electrons so in the end the molecule itself has 10 Protons and 10 Electrons making it neutrally charged (I think you're forgetting about the lone pairs)?
But why is water not a polyatomic ion?
The molecule itself has 10 protons and 8 electrons,
Shouldn't it be positively charged then?
Can the hydrogen atom in a hydroxyl group form hydrogen bonds with other molecules in which hydrogen is attached to a N,O or F?I'm pretty sure that it can!
Post by: RazzMeTazz on June 23, 2014, 07:54:09 pm
Well Hydrogen has one proton and one electron and then Oxygen has 8 Protons and Electrons so in the end the molecule itself has 10 Protons and 10 Electrons making it neutrally charged (I think you're forgetting about the lone pairs)?
I'm pretty sure that it can!
Oh thanks so much! :)
That makes sense now!
Post by: RazzMeTazz on July 09, 2014, 10:26:48 am
Post by: alchemy on July 09, 2014, 10:28:53 am
When writing precipitation reactions and a particular compound is slightly insoluble, what do you consider it to be when writing states, soluble or insoluble?
Slightly insoluble still means it's insoluble.
Post by: Yacoubb on July 12, 2014, 03:23:59 pm
Can the hydrogen atom in a hydroxyl group form hydrogen bonds with other molecules in which hydrogen is attached to a N,O or F?
The hydrogen atom on a hydroxyl (-OH) and carboxyl (-COOH) group is capable a forming a hydrogen bond with F, O or N. :)
Post by: MNM101 on July 23, 2014, 09:04:49 pm
Post by: jgoudie on July 23, 2014, 09:27:27 pm
m=n.Mr
n=c.V
If you think about whatever the question is asking and transpose these equations you should be able to come up with something.
Alternatively post the full question on here.
How would u calculate the volume in mL and mass of KMnO4 dissolved in a solution(500mL) flask. It says that 0.5 g of KMnO4 is supposed to be dissolved but that's where it's confusing me a bit.
Post by: MNM101 on July 23, 2014, 09:43:38 pm
Post by: jgoudie on July 23, 2014, 09:49:58 pm
What would make more sense is if they wanted you to find the concentration. This can be found in gram/ml or mol/L. For each of these just do what the units tell you.
grams/ml -> divide mass by volume (ml)
mol/L -> divide mol by volume (L)
It's a practical experiment where I had to dissolve 0.5g of KMnO4 in 500mL water in a 500mL flask. The question is then asking what the volume of the solution is in mL and what the mass of KMn04 is( dissolved in the solution)
Post by: MNM101 on July 30, 2014, 09:17:41 pm
Post by: jgoudie on July 30, 2014, 09:35:55 pm
Hi, I'm trying to write the observations&discussion for a supersaturation experiment. The substance we tested was sodium thiosulfate. I'm just having a hard time trying to write down the discussion section, I always have problems with this section as I barely write any prac reports, so can anyone help, thanks in advance.
Post by: MNM101 on July 30, 2014, 10:00:04 pm
Here is a video on super saturation. Most pracs will pretty much deal how supersaturation is formed, what must happen to trigger crystallisation and what type of reaction (exothermic) it is. You might also need to explain where it is used in real life, i.e. heat packs and what not.
Thank you that was so helpful!
Post by: MNM101 on July 31, 2014, 06:45:55 pm
Post by: jgoudie on August 01, 2014, 07:33:50 am
Find the concentration in the first 500ml. (n=m/Mr, then c=n/V)
The next step is the dilution.
so C1V1 = C2V2
C1 = concentration found in part a
V1 = volume of this, (your 50ml you have left)
V2 = the volume you are diluting to (450ml + 50ml = 500ml)
For this question it's asking to calculate the volume of solution in mL, mass if the substance dissolved in g/mL and the concentration in mol/L of 0.5g of KMnO4 which has been dissolved in a 500mL flask and then had 450mL tipped out of it, and then had 450mL of water added to that remaining solution (50mL) , it a dilution process but the question is asking for the concentration so I'm not sure what to do. Do I use c1v1=c2v2 or just c=n/V or c=m/V? Also can you show the working out? Thanks a lot
Post by: dankfrank420 on August 06, 2014, 07:59:10 pm
Post by: RazzMeTazz on August 09, 2014, 10:49:52 pm
Because when you have lets say for example, PO43- as the Bronsted-Lowry base and HNO3 as Bronsted-Lowry acid, you form NO3- and HPO42-.
And hence the products of this acid-base reaction are not a salt and water?
Post by: MNM101 on September 23, 2014, 03:28:44 pm
Post by: RazzMeTazz on September 25, 2014, 02:40:35 pm
Post by: zsteve on October 15, 2014, 07:32:26 pm
Also, take graphite and diamond, allotropes of carbon
@MNM101:
HCl can be assumed to ionize virtually completely in water. The fact that your pH is reading 8 is weird - no matter what the conc of HCl, it should be less than 7. Ignoring the inconsistency (check the indicator again, make sure there are no contaminants!), the pH tells you the concentration of
To compare the actual strengths of acids, you need to compare two samples at the same concentration, i.e. 0.1M HCl and 0.1M CH3COOH.
In Units 1/2 (which is the extent of my present knowledge), you can calculate the pH of both acids/bases theoretically, however, this assumes that it ionises completely. CH3COOH, as we know, does not, so we cannot accurately calculate its pH theoretically with our Units 1/2 knowledge.
However, assuming that you actually do this in a lab, you would find that HCl has a lower pH than CH3COOH at the same conc, meaning that HCl is a stronger acid.