In a lab simulation, I used 0.1M NaOH solution in a burette and placed 10ml of u

Question

In a lab simulation, I used 0.1M NaOH solution in a burette and placed 10ml of unknown molarity in a flask. I used an indicator to help me find an equivalence point in the HCl. It turned pink after delivering 11.20ml of 0.1M NaOH into the HCl. I need to find the molarity of the HCl used in the experiment.

I have posed this question already on this site and another and received two different answers, so I am posing it again to hopefully see the layout of the calculations.

Volume of NaOH solution in the burette at the start (mL): 50ml 38.80ml 11.20ml 10ml Volume of NaOH solution in the burette at the end (mL): Volume of NaOH solution delivered to the flask (mL): d Volume of HCl solution in the flask (mL)

Explanation / Answer

Neutralisation reaction between NaOH and HCl is written as,

NaOH (aq.) + HCl (aq.) -------------> NaCl (aq.) + H2O (l)

Neutralisation formula is,

M1V1 / n1 = M2V2 / n2

0.1 * 11.20 / 1 = M2 * 10 / 1

M2 = Molarity of HCl solution = 0.112 M

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