Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: steph_r on August 19, 2008, 03:40:24 AM
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Hi everyone,
I was having a look at this question in my chem book and found it a little confusing..
Question: Explain why the pH of a 1.0M solution of Hydrochloric acid is greater than the pH of a 1.0M solution of sulfuric acid
My attempt: I would have thought that HCl acid is a stronger acid and therefore, would have a smaller pH (more acidic) than sulfuric acid ???..
Help woudl be greatly appreciated ..
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hey steph_r!
nono, why do you think HCl is a stronger acid? This question can actually be done intuitively, since the concentration of the acids are the same. Otherwise, you can calculate the concentration of H+ ions, thus the pH.
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Yes, i see where you're coming from, but how would you actually explain it? How do you explain that HCl has a greater pH than sulfuric acid?
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Yes, i see where you're coming from, but how would you actually explain it? How do you explain that HCl has a greater pH than sulfuric acid?
A strong acid ionises more fully. So Ka value would be higher as more H30+ is produced. Look at the Ka tables for acids if you don't want to use formulas to work it out.
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hey
can you show that 1.0M of HCl is less acidic than 1.0M of H2SO4? Therefore concluding, HCl has higher pH since it is less acidic.
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hello all!!!
HCl ---> H++ Cl-
1,0 1,0M
but
H2SO4 ------> 2H++ SO42-
1,0 2.0M
then pH[HCl] > pH[H2SO4]
note
HSO4- -------> H+ + SO42- not all 100%
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Yuki just answered the question perfectly. All I can add is that the reason why H2SO4 can almost ionize both of its protons is because of the stability of the HSO4- and the SO4 2- ion due to resonance.
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Yuki just answered the question perfectly. All I can add is that the reason why H2SO4 can almost ionize both of its protons is because of the stability of the HSO4- and the SO4 2- ion due to resonance.
H2SO4 ionizes its second proton in about 70 %.