Question
In: Chemistry
a) 125 mL of a 0.109 M phenylalanine (pKa1 = 1.83, pKa2 = 9.13) solution is...
a) 125 mL of a 0.109 M phenylalanine (pKa1 = 1.83, pKa2 = 9.13) solution is titrated with 0.223 M NaOH. What is the pH after 0 ml of NaOH have been added?
b) 125 mL of a 0.109 M phenylalanine (pKa1 = 1.83, pKa2 = 9.13) solution is titrated with 0.223 M NaOH. What is the pH after 25 ml of NaOH have been added?
c) 125 mL of a 0.109 M phenylalanine (pKa1 = 1.83, pKa2 = 9.13) solution is titrated with 0.223 M NaOH. What is the pH after 75 ml of NaOH have been added?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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A 20.00 mL solution of 0.200M diprotic acid (H2A, pKa1=3.500, pKa2=8.500) is titrated with 0.250M KOH....
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Apparently the answer is 2.79 but can someone explain this?
a. -0.029
b. 3.38
c. 2.79
d. 4.89
e. 2.37
Starting with 120 mL of a 0.45 M solution of phenylalanine, shown above at pH =...
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Calculate pH of 0.1 M potassium hydrogen oxalate. pKa1=1.25, pKa2=4.27. Calculate pH of solution prepared from...
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Calculate pH of solution prepared from 0.1 mole of formic acid
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What will be pH of a 100 mL buffer solution containing 0.064 M
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A sample of carbonic acid (0.125 L, 0.145 M, pKa1 = 6.35, pKa2 =
10.33) was titrated with 1.42 M NaOH. Calculate the pH at the
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1. Before the titration.
2. At the 1st midpoint.
3. At the 1st stoichiometric point.
4. At the 2nd midpoint.
5. At the 2nd stoichiometric point.
A sample of carbonic acid (0.125 L, 0.199 M, pKa1 = 6.35, pKa2 = 10.33) was...
A sample of carbonic acid (0.125 L, 0.199 M, pKa1 =
6.35, pKa2 = 10.33) was titrated with 1.75 M NaOH.
Calculate the pH at the following points:
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At the 1st midpoint.
At the 1st stoichiometric (equivalence) point.
At the 2nd midpoint.
At the 2nd stoichiometric (equivalence) point.
A sample of carbonic acid (0.125 L, 0.154 M, pKa1 = 6.35, pKa2 = 10.33) was...
A sample of carbonic acid (0.125 L, 0.154 M, pKa1 =
6.35, pKa2 = 10.33) was titrated with 1.53 M NaOH.
Calculate the pH at the first and at the second midpoints.
A sample of carbonic acid (0.125 L, 0.199 M, pKa1 = 6.35, pKa2 = 10.33) was...
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6.35, pKa2 = 10.33) was titrated with 1.75 M NaOH.
Calculate the pH at the following points:
Before the titration.
At the 1st midpoint.
375 mL of a .150 M aqueous solution of silver (1) nitrate is mixed with 125...
375 mL of a .150 M aqueous solution of silver (1) nitrate is
mixed with 125 mL of .125 M aqueous solution of sodium phosphate.
Calculate the mass of precipitate that forms and the final
concentration of each ion in the mixed solution. Volumes are
additive and the precipitation reaction goes to completion.
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