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Answer:
1.64mL of 5.80M are added
Explanation:
First, we need to calculate total moles of acetic buffer. Then, with H-H equation, we need to find ratio of moles of acetate and acetic acid.
The moles of acetate increased are due the addition of moles of NaOH. Thus, we can find the volume of 5.80M NaOH that must be added:
Moles acetic acid and sodium acetate:
Acetic acid: 0.550L * (0.0215mol/L) = 0.011825 moles
Acetate: 0.550L * (0.0255mol/L) = 0.014025 moles
Total moles = 0.02585 moles = [Acetate] + [Acetic acid] (1)
H-H equation:
pH = pKa + log [Acetate] / [Acetic acid]
Where pH is 5.75;
pKa of acetic acid is 4.74;
And [ ] could be taken as moles of each species.
5.75 = 4.74 + log [Acetate] / [Acetic acid]
10.2329 = [Acetate] / [Acetic acid] (2)
Replacing (1) in (2):
10.2329 = 0.02585 - [Acetic acid] / [Acetic acid]
10.2329[Acetic acid] = 0.02585 - [Acetic acid]
11.2329[Acetic acid] = 0.02585
[Acetic acid] = 0.002301 moles.
Moles acetate:
[Acetate] = 0.02585 moles - 0.002301 moles = 0.023549 moles
Initial moles were 0.014025 moles, moles of acetate added (Due the addition of NaOH) are:
0.023549 moles - 0.014025 moles = 0.009524 moles of NaOH
Volume is:
0.009524 moles of NaOH * (1L / 5.80mol) = 1.64x10⁻³L = 1.64mL of 5.80M are added
A buffer solution is a solution consisting of a weak base and conjugate acid or vice versa. 1.64 mL of 5.80M NaOH must be added to increase pH.
What is volume?
Volume is the space or the area is occupied by a substance. It is calculated in milliliters, liters, etc.
Moles of acetic acid: [tex]0.550 \times 0.0215 = 0.011825 \;\rm moles[/tex]
And, moles of acetate: [tex]0.550 \times 0.0255 = 0.014025 \;\rm moles[/tex]
Now, the total moles = 0.02585 moles (equation 1)
Using the pH equation the ratio of moles of acetate and acetic acid is calculated as:
[tex]\begin{aligned} \rm pH& =\rm pKa + log \dfrac{[Acetate]}{[Acetic \;acid]}\\\\5.75 &= 4.74 +\rm log\dfrac {[Acetate]}{[Acetic \;acid]}\\\\10.2329 &= \rm \dfrac{[Acetate]}{[Acetic \;acid]} \rm .....(equation 2) \end{aligned}[/tex]
Now replacing the value of equation 1 in 2:
[tex]\begin{aligned}10.2329 &= 0.02585 - \rm \dfrac{[Acetic acid]}{[Acetic \;acid]}\\\\10.2329[\rm Acetic \; acid] &= 0.02585 - [\rm Acetic \; acid]\\\\&= 0.002301 \;\rm moles\end{aligned}[/tex]
Moles of acetate is calculated as:
0.02585 moles - 0.002301 moles = 0.023549 moles
The added moles of sodium hydroxide are: 0.023549 moles - 0.014025 moles = 0.009524 moles
Volume is calculated as:
[tex]0.009524\; \text{moles of NaOH}\times (1 \;\rm L / 5.80 \;\rm mol) = 1.64 \times 10 ^{-3}\;\rm L[/tex]
Therefore, 1.64 mL of 5.80 M sodium hydroxide should be added.
Learn more about buffer solutions here:
https://brainly.com/question/3310719
