This is perfect working!Kearnzo said:n(H+ in HCl)= 0.02 x 0.08 = 1.6x10^-3
n(OH- in NaOH)= 0.03 x 0.05 = 1.5x10^-3
That is right
But 0.0016 - 0.0015 is 0.0001
This is number of moles of H+ ions left in the solutions
Ph = -log10[H+]
c = n/v
volume is 20mls +30 mls = 0.05 L
therefore [H+] is 0.0001/0.05 = 0.002
Ph = -log10[0.002] is equal to 2.69... = 2.7
hahahahaHAHAHAHA lol i did the exact same thing except i didnt even try calculations only looked at that question with 10 mins to go and i was like fuck it theyre both strong acids so they must neutralise to form neutral salts.....how unscientific of me xD@who said:damn. i put d. 7 . lol i tried the calculations and came out with a weird answer so i just said since they are both strong acid / base then it must neutralise . fark me
Im not sure becuase i havent looked at the working but amaybe they think ur double counting the volume. I really dont care i know i got it wrong and that answer looks right cause all the rest are whole numbers there to throw stupid people like me off that like nice answers.iEdd said:lol, funny how the people who put C are now trying to argue that acids cannot be diluted and defy the laws of chemistry. You do realise that if the answer is C, the volumes are completely ignored, and adding any amount more water to the solution will not change the pH (by your logic)?
The teacher that thinks it is C either made a mistake, as we all do, or is a moron and should be fired.
pH = -log[concentration of H+] You do this, you get B.
pH = -log[absolute number of H+] - do this, which is incorrect, you get C. And as I said, if you ignore volumes and don't work with concentrations, then you are effectively arguing that there is no such thing as diluting or concentrating a substance and the world as we know it is fucked as simple concepts are apparently too hard.
your teachers credability goes out the window.Aaron.Judd said:
I find it quite funny that people are using comments like these as definite proof and reasoning for an answer ==Aaron.Judd said: