A chemist needs to neutralize 349 L of HF solution that has a molarity of 3.6 M. She currently has an NaOH solution with a molarity of 5.4 M. How many liters of her NaOH solution would she need to neutralize the HF? The chemical equation for this reaction is HF + NaOH → NaF + H2O. I need the answer in 20 ish minutes! Please help!

Answers

Answer 1

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Explanation:A chemist needs to neutralize 349 L of HF solution that has a molarity of 3.6 M. She currently has an NaOH solution with a molarity of 5.4 M. How many liters of her NaOH solution would she need to neutralize the HF? The chemical equation for this reaction is HF + NaOH → NaF + H2O. I need the answer in 20 ish minutes! Please help!

Sure, I'd be happy to help! Based on the chemical equation you provided, one mole of HF reacts with one mole of NaOH to form one mole of NaF and one mole of water.

To calculate the number of moles of HF in 349 L of 3.6 M solution, we can use the formula:

moles of solute = molarity x volume in liters

So, moles of HF = 3.6 M x 349 L = 1256.4 moles of HF

Because the reaction is a 1:1 ratio between HF and NaOH, we would need the same number of moles of NaOH to neutralize the HF.

Therefore, we can find the number of liters of 5.4 M NaOH solution needed using the formula:

moles of NaOH = moles of HF

5.4 M x volume of NaOH solution in liters = 1256.4 moles of NaOH

volume of NaOH solution in liters = 1256.4 moles of NaOH / 5.4 M

volume of NaOH solution = 232.3 L

So, the chemist would need approximately 232.3 L of 5.4

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