1) Write the NET IONIC equation for each of the titration reactions: a)) HCl tit

ID: 791621 • Letter: 1

Question

1) Write the NET IONIC equation for each of the titration reactions:

a)) HCl titration

b)) CH3COOH titration:

2) A researcher takes a10 mL sample of HCl from a bottle and titrates it with NaOH. It was

found that 22.4 mL of 0.25 M NaOH were required to reach the equivalence point. What

is the concentration of the HCl in original bottle?

3) Would the calculation in question # 2 be different if the original acid was CH3COOH?

Why or why not?

Please Show steps for all solutions and reasoning. Thanks.

1. NET EQUATIONS

HCl + NaOH= NaCl +H2O

CH3COOH +NaOH= CH3COONa + H2O

2 .M1V1=M2V2 FOR HCl M1=??? V1=10ML

NaOH M2=0.25M V2=22.4ML

M1=(0.25*22.4)/10

=0.56 M

ORIGINAL CONCENTARTION OF HCl is 0.56M

3.NO BECAUSE IT FOLLOWS THE EQUATION M1V1=M2V2

SO IRRESPECIVE OF THE ACID THE CONCENTARTION REAMAINS THE SAME BECAUSE THE VOLUME & CONCENTARTION OF NaOH ARE NOT CHANGING...

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