Asked by Onye
A chemist performs an acid–base titration using 0.176 M aqueous NaOH as the titrant with 26.15 mL of 0.102 M H2SO4. The endpoint of the titration is detected using phenolphthalein as the indicator.
The balanced equation for the reaction is shown below:
$$
What volume of NaOH is expected to be required to consume all of the acid initially present?
The balanced equation for the reaction is shown below:
$$
What volume of NaOH is expected to be required to consume all of the acid initially present?
Answers
Answered by
DrBob222
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
mols H2SO4 = M x L = 0.102 x 0.02615 = ?
Using the coefficients in the balanced equation, convert mols H2SO4 to mols NaOH. That is 2 mol NaOH to 1 mol H2SO4; therefore, mols NaOH = 2 x mols H2SO4.
Then M NaOH = mols NaOH/L NaOH. You know M and mols, solve for L and convert to mL if desired.
Post your work if you get stuck.
mols H2SO4 = M x L = 0.102 x 0.02615 = ?
Using the coefficients in the balanced equation, convert mols H2SO4 to mols NaOH. That is 2 mol NaOH to 1 mol H2SO4; therefore, mols NaOH = 2 x mols H2SO4.
Then M NaOH = mols NaOH/L NaOH. You know M and mols, solve for L and convert to mL if desired.
Post your work if you get stuck.
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