Imagine that you are in chemistry lab and need to make 1.00 L of a solution with

Question

Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you You start to add HC1 to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH- Once you realize your error, you assess the situation. You have 85.0 mL of HC1 and 89.0 mL of NaOH left in their original containers. Part A Assuming the final solution will be diluted to 1.00 L how much more HCl should you add to achieve the desired pH?

Explanation / Answer

Part A
pH=log(H)
2=log H
H=1E-2=.01M

HCl net must be .01moles.

You have .009*7E-2 moles or .009*.063 moles

So additional moles must be .01-above.

addition volume HCL=additional mole/7E-2 in liters.

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