How many milliliters of 0.132 M HClO₄solution are needed to neutralize 50.00 mL of 0.0789 M NaOH? A) 0.0120 B) 0.0335 C) 83.7 D) 29.9 E) 0.521

Question

Quizplus · Accepted Answer

To solve this problem, we can use the balanced chemical equation for the neutralization reaction between HClO and NaOH:

HClO + NaOH → NaClO + H2O

From this equation, we can see that the stoichiometric ratio of HClO to NaOH is 1:1. This means that for every 1 mole of NaOH, we need 1 mole of HClO to neutralize it.

First, we need to find the number of moles of NaOH in 50.00 mL of 0.0789 M NaOH:

moles NaOH = Molarity x Volume (in liters)
moles NaOH = 0.0789 M x 0.05000 L
moles NaOH = 0.003945

Since the stoichiometric ratio of HClO to NaOH is 1:1, we need 0.003945 moles of HClO to neutralize the NaOH.

Now we can use the concentration of the HClO solution to find the volume we need to add:

moles HClO = Molarity x Volume (in liters)
0.003945 = 0.132 M x Volume (in liters)
Volume (in liters) = 0.0299 L

Finally, we convert the volume from liters to milliliters:

Volume (in mL) = 0.0299 L x 1000 mL/L
Volume (in mL) = 29.9 mL

Therefore, the answer is D) 29.9.

How Many Milliliters of 0