Assume you titrate 25.00 mL of your freshly made ~1.0 M NaOH solution with 1.000 M HCl using phenolphthalein as the indicator. If 24.02 mL of HCl was required to reach a pale pink endpoint, what is the molarity of your solution? Assume the unit is M and your answer must contain 4 significant figures

answer

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Elin HesselLv2

10 Oct 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

A chemist had a bottle of HCl (aq) of unknown concentration. Sheperformed a titration experiment in order to determine itsconcentration. She pipeted 15.00 mL of the HCl solution into anErlenmeyer flask. She then added about 20 mL of deionized water and3 drops of phenolphthalein indicator dye to the flask. She titratedthis mixture with 0.07269 M NaOH (aq), and obtained a permanent,pale pink endpoint after the addition of 24.33 mL of NaOH (aq).Given that the density of the HCl solution was 1.095 g/mL,determine the concentration of the original HCl acid solution inunits of:

A. Molarity

B.Percent by mass

Thanks!!