Imagine that you are in chemistry lab and need to make 1.00 LL of a solution...

Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pHpH of 2.60.

You have in front of you

100 mLmL of 6.00×10−2mol L−16.00×10−2mol L−1 HClHCl,
100 mLmL of 5.00×10−2mol L−15.00×10−2mol L−1 NaOHNaOH, and
plenty of distilled water.

You start to add HClHCl 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 NaOHNaOH. Once you realize your error, you assess the situation. You have 83.0 mLmL of HClHCl and 90.0 mLmL of NaOHNaOH left in their original containers.

Assuming the final solution will be diluted to 1.00 LL , how much more HClHCl should you add to achieve the desired pH?

Solutions

Expert Solution

queen_honey_blossom answered 10 months ago

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