In Part 1 of this experiment, you will standardize the NaOH solution by using it

Question

In Part 1 of this experiment, you will standardize the NaOH solution by using it in a titration with HCI of known concentration. Suppose that you transfer 10.00 mL of 0.1106 M HCI into an Erlenmeyer flask via volumetric pipet. You then add 25 mL of deionized water to the flask to dilute the acid solution. How many moles of HCl are present in the Erlenmeyer flask at the beginning of your titration? Suppose you titrate this HCI solution with NaOH of unknown concentration. At the beginning of the titration, your initial volume reading from the buret (Vi) is 0.52 mL. At the endpoint, when the solution in the Erlenmeyer flask just turns pink, the final buret reading (Vf) is 14.16 mL. What was the total volume (in mL) of NaOH solution added to reach the endpoint?

Explanation / Answer

moles of NaOH used = moles of HCl = 1.106 millimoles.

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