A 0.1195 g sample of solid Na2CO3 was added to a 250 mL

flask, dissolved in 35 mL of boiled distilled water, and had5

drops of phenolphthalein indicator added. Next, 40.00 mL ofa

HCl solution with an unknown concentration was added to the

flask, turning the solution colorless (indicating excess acidwas

present). The resulting solution was boiled gently for 2

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21 Feb 2023

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A 0.1997g sample of primary standard sodium carbonate was weighed out into a 250-ml beaker and diluted with 50ml of distilled water. An HCl solution of unknown concentration was used to titrate the Na2CO3 in the beaker. After passing the first equivilance point at about 22ml where the phenolphthalein indicitator becasue colorloss, a few drops of bromcresol green indicator were added. When the indication began to change from blue to a green color, the titration was stopped and the solution was boiled and the indicator returned to a blue color as carbon dixoide was expelled from the solution. After cooling the sample back to room temperature, the titration was continued untill a total of 45.12 mL of HCl had been added and a distince color change from blue to green was observed.

Calculate the concentration of the HCl titrant solution using the volume to reach the second equivilance point.

A 0.3520g sample of an unknown concentration of soda ash sample was weighed out and titrated by the same procedure using the same HCl titrant solution, and a distinct color change at the sencond equivilance point was observed at 20.09 mL. Using the previously determined HCl solution concentration and the soda ash sample mass, determine the weight percent of sodium carbonate in the soda ash unknown.