A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?
Solution Preview
You need the buffers mathematical equation, and to be able to identify each speices.
Ka = [H+] x (A-/HA)
Ka is the Ka of the acid HA
[H+] is your pH term (your answer in most cases)
A- is the conjugate species of the acid HA
HA is the acid that we have the Ka value for...
Setting up the BUFFER equation...
Ka = [H+] x 0.250/0.100
From this we can find the pH before the ...
Solution Summary
The solution explains the steps necessary to find the pH of a buffer solution after some HCl is added in almost 300 words.
Find the solutions without using the Henderson-Hasselbalch equation. Please show all calculations.
Question #1
A student dissolves 0.25 moles of the acid HA in water and dilutes the solution to the final volume of 500 mL. The student then gives a small portion of the solution to her professor. The professor uses a pH meter
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HEPES has MW 238.3 and pK = 7.48
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11. The Ka of HBrO is 2.5 x 10-9
When eql volumes of 0.1 M HbrO and 0.1 M NaBrO are mixed the pH of the solution will be
A. Between 0 and 1
B. Between 4 and 5
C. Approximately = 7
D. Between 8 and 9
E. Between 9 and 10
Justify your answer with a calculation
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I've attached the whole page from the exam for the information it provides. I've boxed my previous answers in case they are needed to figure out the four questions.
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