Top Score GC question

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TXpredent

Always confused
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What volume of HCl was added if 20 mL of 1 M NaOH is titrated with 1 M HCl to produce a pH = 2?

I know since the concentrations of the strong acid and strong base are the same, they will cancel each other out with a 1:1 ratio. So I know it's got to be just over 20 mL but how much HCl will give me a pH of 2?

I figured it would've been 1 x 10^-2 moles of HCl which with 1 M solution would be 1 x 10^-2 L which is 10 mL so 30 mL of HCl was titrated but the answer is 20.4. Their solution is really confusing and I can't figure out what's going on in it. Any ideas on how to do this problem?
 
if its 1M NaOH and 1M HCL both around 20 mL, how is the pH 2? - shouldn't it be around 7 (the equivalence point) b/c you're titrating a strong base with a strong acid?
 
Since the pH is 2 we know [H+] = 1e^-2. Set up as follows and solve for x.
1e^-2= x / 40 + x.....where 40 is the total volume (solved via MV=MV) and the x on the denominator is minute so can be ignored here. x = .4. Add that to the 20 that you added for neutralization. Bam!

ok, that makes much more sense, i was kinda close lol! I didn't understand Top Score's explanation but this makes much more sense. How did you know 'x' in the denominator was going to be minute? Also, what does 'x' represent here? The [H+] ions needed in a 40 mL solution to get a total concentration of 1 x 10^-2?
 
I believe that X represents the number of moles of H+ ions needed since molarity which can also be viewed as concentration is equal to the number of ( moles / liters ).
 
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