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A couple of chemistry acid/base questions! Urgent! Help please!
Asked by: ashleighmarie
from GREENSBORO, NC
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My teacher didn't really explain these well. Any help appreciated. This is due tonight so please help me!
1. What is the value of the equilibrium constant (three sig figs) for the reaction of hydrofluoric acid and ammonia?
K =
Fill in the following reaction table with millimoles (to the nearest 0.01 mmol) for the reaction occurring when 44.7 mL of 0.222-M ammonia are mixed with 27.6 mL of 0.292-M hydrofluoric acid.
HF + NH3 ↔ F1- + NH41+
initial
delta
final
What is the final concentration of ammonium ion to three significant figures?
[NH41+] =
How many mmols (three sig figs) of the limiting reactant are actually present at equilibrium? Note that this value is not based on the final amount in the reaction table because the table assumes complete reaction (not an equilibrium) of the limiting reactant.
Link to acid/base table: http://www.webassign.net/wertz...
2. Consider the titration of 35.0 mL of 0.165-M of KX with 0.078-M HCl. The pKa of HX = 5.21. Give all pH values to 0.01 pH units.
a) What is the pH of the original solution before addition of any acid?
b) How many mL of acid are required to reach the equivalence point?
c) What is the pH at the equivalence point?
d) What is the pH of the solution after the addition of 37.0 mL of acid?
e) What is the pH of the solution after the addition of 88.8 mL of acid?
1. What is the value of the equilibrium constant (three sig figs) for the reaction of hydrofluoric acid and ammonia?
K =
Fill in the following reaction table with millimoles (to the nearest 0.01 mmol) for the reaction occurring when 44.7 mL of 0.222-M ammonia are mixed with 27.6 mL of 0.292-M hydrofluoric acid.
HF + NH3 ↔ F1- + NH41+
initial
delta
final
What is the final concentration of ammonium ion to three significant figures?
[NH41+] =
How many mmols (three sig figs) of the limiting reactant are actually present at equilibrium? Note that this value is not based on the final amount in the reaction table because the table assumes complete reaction (not an equilibrium) of the limiting reactant.
Link to acid/base table: http://www.webassign.net/wertz...
2. Consider the titration of 35.0 mL of 0.165-M of KX with 0.078-M HCl. The pKa of HX = 5.21. Give all pH values to 0.01 pH units.
a) What is the pH of the original solution before addition of any acid?
b) How many mL of acid are required to reach the equivalence point?
c) What is the pH at the equivalence point?
d) What is the pH of the solution after the addition of 37.0 mL of acid?
e) What is the pH of the solution after the addition of 88.8 mL of acid?
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I know this is not the answer you are hoping/looking for, but if you do not understand or your teacher did not explain it correctly, I suggest you talk to your teacher or ask for additional help. If someone on Askpedia is currently doing your acid/base questions, what will you get out of it? Probably some answers but still, you will not know how to do it or what your teacher is looking for.
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Answer Date: 12:01pm 11/08/07
