II.Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 Msolution of HCl. Then you titrated the excess HCI with 0.100 M NaOH. It took 14.33 mL to theendpoint. SHOW WORK!1.00MHCLHow many moles of HCl did you add initially?_·025 mol HCIHow many moles of NaOH did you use in the titration?How many moles of HCl were titrated (left over)?How many moles of HCl reacted with the tablet (subtract titrated from initial)..How many moles of calcium carbonate were present?_How many grams of calcium carbonate were present? (MW 100.10).se no moreWhat is the percent of calcium carbonate in the tablet?_

Here we are required to calculate the percentage of CaCO3 in the tablet . 1L=1000ml

Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 M solution of HCI. Then you titrated the excess HCI with 0.100 M NaOH. It took 14.33 mL to the endpoint. SHOW WORK! 1.00MHC How many moles of HCl did you add initially? ·025mol HCI How many moles of NaOH did you use in the titration? How many moles of HC1 were titrated (left over)? How many moles of HCl reacted with the tablet (subtract titrated from initial). How many moles of calcium carbonate were present? How many grams of calcium carbonate were present? (MW 100.10)_ What is the percent of calcium carbonate in the tablet? 1

Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 M solution of HCI. Then you titrated the excess HCI with 0.100 M NaOH. It took 14.33 mL to the endpoint. SHOW WORK! 1.00MHC How many moles of HCl did you add initially? ·025mol HCI How many moles of NaOH did you use in the titration? How many moles of HC1 were titrated (left over)? How many moles of HCl reacted with the tablet (subtract titrated from initial). How many moles of calcium carbonate were present? How many grams of calcium carbonate were present? (MW 100.10)_ What is the percent of calcium carbonate in the tablet? 1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A sample of antacid tablet that contains NaHCO3 is analyzed in the lab. The student dissolves 1.50g tablet in 35.0 mL of HCl solution containing 0.0300 mole of HCl. The back-titration of the excess HCl require 10.5 mL of 2.05M NaOH solution. 1) If that tablet label showed that each tablet contains 0.950 gram of NaHCO3. Determine the percent error in the student experiment. 2) Calculate the mass percent of the NaHCO3 in the tablet.
25 mL of a solution of barium hydroxide on titration with 0.1 molar solution of hydrochloric acid gave titer value of 35 mL. The reaction involved in the titration is: Ba(OH)2 + 2HCI -------> BaCl2 + 2H2O The equation that is used to find the molarity of unknown solutions in titrations is: M,V1/n1 = M2V2/n2 What is the molarity of barium hydroxide solution? 0.28 0.35 0.14 0.07
10.00mL of 0.10M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: Ignore the volume of the indicator added, as the volume is tiny compared to 100mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00mL of 0.100M NaOH? Question 3 options: 7.22 6.9 8.35 7.00
An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?
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Please using the data below please do the calculations in the image attached Both images go together Please please answer super super fast it's super important
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A 28.00mL volume of aqueous sulfuric acid, H2SO4, is titrated using 0.200M NaOH and an indicator that turn color only after all the sulfuric acid protons have reacted with -^OH ions. The solution turns color when 48.32mL of base has been added. What is the molar concentration of the sulfuric acid ? (HINT: a balanced chemical equation will help) Show Work Please
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