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what is the molarity of an hcl solution if it takes 25.00 ml of a 0.750 m naoh solution to neutralize 10.00 ml of the hcl solution?

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Bharathparasad577idn

1.875M is the molarity of an HCl solution if it takes 25.00 ml of a 0.750 m NaOH solution to neutralize 10.00 ml of the HCl solution

The Balanced reaction for the equation is given by:

HCl+NaOH⇌H₂O+NaCl

It is given that the molarity of NaOH is 0.750M, the volume of HCl is 25ml, the volume of HCl to be neutralized is 10ml.

Then,

By titration:

We know that,

Molarity = n/V

n = Molarity x V

0.025 L of 0.750 mol/L of NaOH= No of moles of NaOH

No of moles NaOH = 0.025 x 0.750

No of moles of NaOH = 0.01875 mol

Then it can be written that,

0.01875 mol NaOH ⋅ 1 mol HCl/1 mol NaOH =

0.01875 mol HCl

Now,

0.01875 mol HCl / 0.010 L =1.875M HCl

Therefore, the molarity is 1.875M

To know more about acid-base titration, click below:

https://brainly.com/question/23687757

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