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SOVA2 [1]
2 years ago
12

Question 2/4

Chemistry
1 answer:
notka56 [123]2 years ago
4 0

Answer:

I think false

Explanation:

sue me if I am wrong I don't care and how do you get 6 points up there

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it's answer 2

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Calculate the pH of a buffer solution prepared by mixing 60.0 mL of 1.00 M lactic acid and 25.0 mL of 1.00 M sodium lactate.
marshall27 [118]
This problem could be solved easily using the Henderson-Hasselbach equation used for preparing buffer solutions. The equation is written below:

pH = pKa + log[(salt/acid]

Where salt represents the molarity of salt (sodium lactate), while acid is the molarity of acid (lactic acid). 

Moles of salt = 1 mol/L * 25 mL * 1 L/1000 mL = 0.025 moles salt
Moles of acid = 1 mol/L* 60 mL * 1 L/1000 mL = 0.06 moles acid
Total Volume = (25 mL + 60 mL)*(1 L/1000 mL) = 0.085 L

Molarity of salt = 0.025 mol/0.085 L = 0.29412 M
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Thus,
pH = 3.86 + log(0.29412/0.70588)
pH = 3.48
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3 years ago
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I tried sorry if it’s not worded perfect :)
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Who knows how to do this please help
Fofino [41]

Answer: You forgot to zero the balance

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