Sulfuric acid is a highly corrosive substance that should be handled with extreme caution. It is important to always wear proper protective gear when working with sulfuric acid to avoid any potential injuries or accidents. Remember, safety should always be the number one priority when dealing with hazardous chemicals like sulfuric acid.
 
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Please help..?
Calcium ion solution is titrated with ethylenediaminetetraacetic acid (EDTA) solution in a complexation titration.
Qualitatively explain the effect of the concentration of the analyte solution on the shape and the shape of the titration curve.
Qualitatively explain the effect of the concentration of the titrant solution on the shape and the shape of the titration curve.

 ''When the concentration of the analyte solution is low, the titration curve may exhibit a gradual increase in the titrant volume added before reaching the equivalence point. This is because a low concentration of the analyte solution requires less titrant to reach the equivalence point, resulting in a gentle slope on the titration curve. As the concentration of the analyte solution increases, the steepness of the titration curve around the equivalence point also increases since more titrant is needed to fully neutralize the higher concentration of the analyte.'' Is this correct? I have to explain how the titration curve moves, Idk how. Please help:/ Thank you!

so I've been banging my head against this problem for a while now and I'm pretty sure I'm doing something wrong. this is the unbalanced reaction:
(may be important the mention: this is happening in acidic conditions.)

CuS(s) + HNO₃    Cu(NO₃)₂ + H₂O + NO(g) + S(s)

the first thing that I got stuck on was finding the oxidation states for the atoms in Cu(NO₃)₂. after doing some googling I found out that NO₃ should have a minus sign on it((NO₃)^-) which made some sense after drawing the lewis stracture for it.
after doing that I noticed that S and N changed their oxidation number(S was -2 and became 0, N was +5 and became +2).

However when writing the half reactions for oxidation and reduction, I got stuck. this was my process:

oxidation half reaction(unbalanced):

CuS(s)+ HNO₃  S(s)+ Cu((NO₃)^-)₂

Cu and S quantities were already balanced, and the same goes for oxygen quantities. which only leaves balancing Hydrogen and nitrogen quantities like so:

CuS(s)+ 2HNO₃  S(s)+ Cu((NO₃)^-)₂ + 2H⁺

the weird thing is that after doing that the charges are balanced too, which makes no sense because that should mean there was no transfer of electrons and hence no oxidation.

as for reduction, I tried balancing this:
HNO₃  NO(g)

however, the weird thing is that H₂O is not present in either, and I have no idea how to include it.

summery of all of my questions:
1. Is the lack of a minus sign on (NO₃)₂ really a mistake or am I missing something? If it is intentional, how do I find the oxidation numbers for the atoms in Cu(NO₃)₂?
2. is my oxidation half-reaction correct? if not, what am I missing?
3. how do I involve H₂O in my half reactions?

I honestly tried to solve this for a long time and I'm not asking people to do it for me, I'm just really, really, bad at chemistry and I'm kinda stuck.

H is the packaging height. This information should gives your column. Probably the 20 cm.

With the passage of time and the progress of the reaction, does the value of the potential of the element (Ecell) increase or decrease? When will the specific electrolytic cell stop working? Explain qualitatively.
(Given: Faraday constant, NA (Avogadro), R constant)


''With time, the concentration of the electrolyte solution change. Hence, their electrode potentials change. When the electrode potentials of the two half − cells become equal, the cell stops working.'' Is this correct? Any thoughts? Should I also use an equation? I'm not sure what else to add. Thank you for any help