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A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out of oxalic acid , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used of sodium hydroxide solution. What is the molarity of the student's sodium hydroxide solution? Round your answer to 3 significant digits.

 
 

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Christian Tuso
Christian TusoLv10
20 Jan 2021

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Related questions

Can someone help me with this question?

An analytical chemist weighs out 0.199g of an unknown diprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0800M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 29.9mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.

Units should be in g/mol

Thanks

An analytical chemist weighs out 0.093g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1600M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 6.5mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

160 g of a 0.80% sodium hydroxide solution.

The following question involves the reaction of sodium hydroxide and succinic acid. Succinic acid is diprotic: the acid (H2C4H4O4) reacts with two of its hydrogens to give C4H4O42-. The balanced “molecular” equation for the reaction has coefficients of 2 for NaOH and 1 for succinic acid:

2 NaOH (aq) + H2C4H4O4 (aq) --> Na2C4H4O4 (aq) + 2 H2O (l)

A student weighs 1.700 g of succinic acid and dissolves it in water in a 250.0 mL volumetric flask. A 25.00 mL sample of this solution is withdrawn and placed in a 125 mL Erlenmeyer flask, to which 5 drops of the acid-base indicator phenolphthalein is added. This solution is titrated with a sodium hydroxide solution of unknown molarity in a buret.

a) How many moles of succinic acid were weighed and dissolved in the volumetric flask?

0.0572 M

b) How many moles of succinic acid were placed in the Erlenmeyer flask?

1.43 x 10-3 mol

c) If the unknown sodium hydroxide solution was known to be approximately 0.20 M, at approximately what buret volume would you expect the end point of the titration? Show the calculation, including the use of the appropriate coefficients, as a 2 significant figure estimate:

14.30 mL NaOH

d) If the measured volume at the end point was 13.32 mL of sodium hydroxide added, calculate the actual molarity of the sodium hydroxide solution.

0.214 M NaOH

You are going to standardize a 0.80% solution of sodium hydroxide solution for which the molarity is approximately 0.20 M. You will have dry succinic acid, a 250 mL volumetric flask, a 25.00 mL pipet, a 50.00 mL buret, a phenolphthalein indicator solution, and other standard laboratory equipment. For each titration you will withdraw a 25.00 mL sample of the succinic acid solution with a volumetric pipet. Therefore, you will deliver exactly one-tenth of your initial mass of succinic acid (to four significant figures) in each titration. In deciding the amount of succinic acid to weigh, assume that you will be using approximately 15 mL of the sodium hydroxide of approximate 0.20 M concentration for each titration, and you need enough succinic acid for ten titrations. Show how to calculate the mass of succinic acid you will need to weigh.

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