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1. If the HCl used in this experiment was prepared at a concentration of 0.15M. Using...

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Chemistry

1. If the HCl used in this experiment was prepared at aconcentration of 0.15M. Using your volume of HCl neutralized byyour whole tablet, calculate the mass of active ingredient (CaCO3)in the tablet in milligrams.

2. Instead of using ratios for back titrations we can also usemolarities, if our solutions are standardized. A 0.196g sample ofantacid containing an unknown amount of triprotic base Al(OH)3 wasreacted with 25.0mL of 0.111M HCl. The resulting solution was thentitrated with 11.05mL of 0.132M NaOH solution. Calculate the masspercent of Al(OH)3 in the antacid sample.

Answer & Explanation Solved by verified expert
3.6 Ratings (496 Votes)
2 first we have to calculate the noof moles of remaining AlOH3 for that as the resulting solution was then titrated with 1105mL of    See Answer
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