Question

# <br/> -As described in the lab procedure for Experiment 7, titrate

sodium hydroxide with solid oxalic acid dihydrate, H2C2O4 · 2H2O. Before the titration, the oxalic acid crystals are dissolved in water. When the oxalic acid is dissolved in water, the water separates from the oxalic acid. This means that it needs to include the water when calculating the molar mass of the oxalic acid, but do not need to include it in the chemical equation.  Given the following titration data, calculate the molarity of the NaOH solution that was titrated?
Mass of flask 143.870 g Mass of flask + oxalic acid 144.236 g

2/ must then titrate sulfuric acid with 0.2207 M sodium hydroxide and get the following data:
Sulfuric acid, initial buret reading0.34 mL Sulfuric acid, final buret reading23.74 mL

Calculate the molarity of the sulfuric acid solution?

3/What is the mass percent of sulfuric acid in your solution if you have a 0.23 M sulfuric acid solution with a density of 1.001 g/mL?

4/0.539 g of an unknown triprotic acid, H3A, is dissolved in 47.3 mL of water and then titrated with 0.319 M NaOH. It takes 25.42 mL of the NaOH solution to completely neutralize the acid. What is the molar mass of this acid?

Step-by-step explanation
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