A student weighed out a sample of acid powder and found the mass to be 1.17 g. When the solution turned pink..

A student weighed out a sample of acid powder and found the mass to be 1.17 g. When the solution turned pink, the student read the buret accurately and found it to be 39.46 mL. If the base concentration is 0.1592 M, what is the molecular weight of the unknown acid?

Answer:
these are funnnnn

ok so find moles of base added

0.03946 L x 0.1592 M = 0.00628 mol

we assume the acid and base are 1:1 in terms of reaction thus 0.00628 mol of acid must have also been needed

Molar mass = g/mol = 1.17g/0.00628 = 186.31

The answers post by the user, for information only, FunQA.com does not guarantee the right.



More Questions and Answers:
  • Question about buffer capacity?
  • What do you mean by enrichment of ores ?
  • Why ammonia(NH3) has a higher boiling point than phasphine(PH3)?
  • Who discovered that circumcision should be done?
  • How is the atomic mass of an element calculated from isotope data?
  • Why arn't alipathic amines very enantioselective in early transition metal hydroamination catalysis?
  • What is the name of this molecule: CH3CH2CHOCH2CH2CH3?
  • Explain the reasons for equilibrium shift observed in step 1-4 in an experiment.?
  • In which direction would the following equilibrium run. If the volume of the container were increased?