The goal of the experiment was to be able to determine the effect that temperature has on solubility by using a salt in water and doing acid-base titrations at varying temperatures. The experiment will also be done to examine the relationship of solubility.
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i have no idea what the mark scheme is trying to say
Well the pH is going to rise because either H+ conc is decreasing and OH- conc is increasing but I dont understand what's happening.
Hi fellow redditors, Im really struggling with this problem at the moment: A solution of .0479M HCl is used to titrate 26M of an ammonia solution of unknown concentration. The equivalence point is reached at 16mL of HCl added. KW=1.01E-14 I need to find the original pH of the ammonia solution.
I’ve been working on chemistry all day, and I never completely got the concept of ICE tables down. I managed to calculate the unknown concentration of ammonia to be .0289M. Where do I go from here to get the pH of the solution? I know all of the information is here, I just need a little extra help on this, if anyone is willing!
Edit: forgot part of the question
So i was given the titration curve of three diprotic acids. The further right we go, pka1 increases and pka2 decreases. The titration curves also appear less and less diprotic; the first equivalence point pretty much disappears. The titration curve of succinic acid looks monoprotic. Why is this happening?
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If weak acids like acetic acid, CH3COOH ionize only a few percent in aqueous solution, why is it possible to fully neutralize a weak acid by reacting it with the stoichiometric equivalent of sodium hydroxide solution, NaOH?
Hi everyone!
Do you recommend any videos or study material that I can use to thoroughly cover acids/bases, titration, and buffer?
Thank you!
I'm in bed mulling this over so sorry if things are not correct. In a buret is a weak acid CH3COOH. The base is NaOH. I begin with 25mL of 0.1222M of NaOH in the beaker. I did 3 trials and I can only remember two of the 3 one was 18.00mL, the other was 18.06 mL. I used the M1V1 = M2V2 to calculate molarity of acetic acid. It's a 1:1 mole ratio. I got that from the balanced equation. So it takes one mole of OH- to neutralize one mole of H+ Acetic acid is diprotic. Ok my first question is what is being titrated. In this lab. The base or the acid? I'm adding acid to the base so I think it's acid? Not really sure. The second question is I need to calculate for precision and accuracy. I was told the acedic acid is 1 liter and at 5% w/w am I using the equation grams of solute over grams of solution? I'm may have to add on questions to this because I'm having a heck of a time trying to retain this information. Edit was the equation
Hi everyone, I’ve been trying to think through the cause of the initial uptick in pH in a weak acid-strong base titration for a couple of days, but unfortunately, I can’t seem to find a clear answer as to what’s happening. Here’s my thoughts and reasoning:
At the start of a titration of a weak acid with a strong base, there is a small uptick in pH before a buffer solution is formed, which causes pH change to plateau. The only way I can make sense of the initial uptick is that the existing H+ ions that are already dissociated from HA get mopped up as the titrant is introduced, therefore reducing the concentration of H+ (and increasing pH). pH change then plateaus as the initial H+ have been removed and the weak acid compensates for this by dissociating further (of which the H+ are immediately consumed by the base, and a buffer is created with the change in HA : A- ratio). But as there is no significant change in H+ concentration at this point, the buffer remains in place until HA is totally consumed.
To me, the above makes sense. But I’ve also heard that strong bases will rip a H+ directly from the weak acid. If this is true, wouldn’t the pH immediately jump up to 14, rather than creating a buffer, as there would be no freely dissociated H+ (and thus a H+ concentration of 0)?
Any feedback to point me in the right direction would be really appreciated for either of the above points.
Cheers
There are no plateaus in this graph, nor is there a sudden jump. I'm so confused. Please help!
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Hey Reddit! I am currently working on a lab report but I do not understand the following questions listed below. Hopefully I can get some help with those questions.
We have performed an acid-base titration using NaOH [0.1 M] and an unknown weak acid (HA). The acid is diluted (1:10, as written below). After the titration we calculated the diluted [acid] (by v * c = v * c) to be 0.101 M. Here are the questions asked regarding the lab:
1: What is the molar mass of the unknown acid HA when 59.5g of the acid was added to 1 liter of water before dilution (25.0mL pipetted into an Erlenmeyer flask and diluted with water to 250mL).
2: What is the unknown acid HA? (The molar masses calculated in problem 1) and with a pKa of ca 4.7?
Thanks in advance!
