Asked by Kelsey
This question is based on an experiment to determine the mass of ASA.
Information from the experiment :
• ASA is a weak acid with a Ka value of 3.2 x 10^-4.
• An ASA tablet has an approximate mass of 500 mg.
• The experiment used a titration with a standardized 0.100 mol/L NaOH.
What volume of base will you substitute into the formula when you calculate the number of moles of base used? I know from looking at the balanced equation that NaOH reacts 1:1 molar with the ASA. HC9H7O4(aq) + NaOH(aq) NaC9H7O4(aq) + H2O(l)
I am just unsure of how to calculate what volume of base to substitute. Any help is appreciated.
Information from the experiment :
• ASA is a weak acid with a Ka value of 3.2 x 10^-4.
• An ASA tablet has an approximate mass of 500 mg.
• The experiment used a titration with a standardized 0.100 mol/L NaOH.
What volume of base will you substitute into the formula when you calculate the number of moles of base used? I know from looking at the balanced equation that NaOH reacts 1:1 molar with the ASA. HC9H7O4(aq) + NaOH(aq) NaC9H7O4(aq) + H2O(l)
I am just unsure of how to calculate what volume of base to substitute. Any help is appreciated.
Answers
Answered by
DrBob222
Are you titrating the ASA with NaOH? If so use the volume NaOH in the titration.
Then mols = M NaOH x L NaOH
Then mols = M NaOH x L NaOH
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