Question
In: Chemistry
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
queen_honey_blossom answered 1 year agoRelated Solutions
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
a solution with a pH of 2.60.
You have in front of you
100 mL of 7.00×10−2 M HCl,
100 mL of 5.00×10−2 M NaOH,
and plenty of distilled water.
You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
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7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of
distilled water. You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
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distilled water. You start to add HCl to a beaker of water when
someone asks you a question. When you return to your dilution, you
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Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
a solution with a pH of 2.50.
You have in front of you
100 mL of 7.00×10−2M HCl,
100 mL of 5.00×10−2M NaOH, and
plenty of distilled water.
You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00 Lof a solution with...
Imagine that you are in chemistry lab and need to make 1.00 Lof
a solution with a pH of 2.80.
You have in front of you
100 mL of 7.00×10−2M HCl,
100 mL of 5.00×10−2M NaOH, and
plenty of distilled water.
You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
a solution with a pH of 2.50. You have in front of you
100 mL of 6.00×10−2 M HCl,
100 mL of 5.00×10−2 M NaOH,
and plenty of distilled water.
You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of
a solution with a pH of 2.60.
You have in front of you
100 mL of 7.00×10−2M HCl,
100 mL of 5.00×10−2M NaOH, and
plenty of distilled water.
You start to add HCl 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...
Imagine that you are in chemistry lab and need to make 1.00L of a solution with...
Imagine that you are in chemistry lab and need to make 1.00L of
a solution with a pH of 2.40.
You have in front of you
100 mL of 6.00
ORGANIC CHEMISTRY (TLC lab) if you used a solution of 90% ethyl acetate / 10% hexane...
ORGANIC CHEMISTRY (TLC lab)
if you used a solution of 90% ethyl acetate / 10% hexane instead
of 10% ethyl acetate / 90% hexane to elute your TLC plates, what
would you expect to see?
Would the Rf valaues increase of decrease for each compound?
Explain in detail.
Rf values
Naphthalene = 0.44
9-fluorene 0.56
Benzophenone = 0.39
Fluorene = 0.88
4-nitroaniline = 0.28
4- methoxyacetophenone = 0.24
1. You make a solution of 0.464 moles HClO2 and 0.464 moles ClO2- dissolved in 1.00...
1. You make a solution of 0.464 moles HClO2 and 0.464 moles
ClO2- dissolved in 1.00 L. What is the minimum number of moles of
KOH would need to be added in order to 'overwhelm' this buffer?
2. You make a solution of 0.316 moles
HClO2 and 0.464
moles ClO2-
dissolved in 1.00 L. What is the minimum number of moles of
KOH would need to be added in order to 'overwhelm' this
buffer?
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