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vera_ewing
 one year ago
A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH was added?
A. 5.1
B. 7.2
C. 3.4
D. 8.6
vera_ewing
 one year ago
A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH was added? A. 5.1 B. 7.2 C. 3.4 D. 8.6

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taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Do you have a guess of which one it is?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1I'm thinking so I don't think I messed up on my math would you like to know what I did?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Ok so we have 15ml of 0.1M NaOH. We can find the moles of NaOH by multiplying the volume in liters (0.015L) by the molarity of 0.1

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1So that means I have 0.0015moles of NaOH

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Then we can set up the ice table HA+NaOH > NaA+ H2O with the initial moles for NaOH as the 0.0015moles

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1I am really bad at explaining this I followed what they did in this link http://chemwiki.ucdavis.edu/Analytical_Chemistry/Quantitative_Analysis/Titration/Titration_Of_A_Weak_Acid_With_A_Strong_Base

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0Okay, hold on let me read it.

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Let me try this again and I'll let you know

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Now I'm getting an answer no where near anything my answer was just over one which does not make sense one bit!

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2I don't think you need to do any math for the question since all the possible options are so far apart. Picture a titration curve dw:1437179500727:dw Initially, and for most of the curve, the slope is small, so we don't expect use changes in pH. If you used 1/3 of the moles that got you to 8.6 (which is a difference of about 5 from 3.2). so, 1/3 of 5 is 1.7, so 3.2 + 1.7\(\approx\)5 so I think 5.1 is reasonable

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2sorry my graph is terrible and unrepresentative of whats going on lol

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1that makes sense just to clarify though the 1/3 you get from the fact that it's 5mL out of the 15mL?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Sounds good it makes a lot more sense than the number I got and not having to do all that math is even better lol

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2the math is often needed but it doesnt always have to be the first way to approach a problem.

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Good to know!
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