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...

See similar textbooks

Similar questions

Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
Part B The titration of 0.5538 g of KHP required 25.89 mL of an NaOH solution to reach the equivalence point. What is the concentration of the NaOH solution? Express your answer using four significant figures. ΑΣΦ M NaOH] =
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?
Number 1_ A 0.5707-g sample of a water-soluble fertilizer was dissolved and analysed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.1334 M boric acid. This solution required 26.27 mL of 0.202 M HCl for titration to the methyl red end point. Calculate the % N (AW =14 g/mol) in the fertilizer.
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
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
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
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
In the titration of 10.00 mL sample of vinegar solution with 0.35 M NaOH as titrant, the initial burette reading was 2.50 mL and the final burette reading was 45.30 mL. Calculate the mass percent of acetic acid (Molar mass = 60.05 g/mol) in the vinegar sample. (The density of the vinegar is 1.00 g/mL) % 5.0 .a O % 8.0 .b O % 6.0 .c O % 9.0 .d O % 7.0 .e O
Use the following information to answer the next question Volume of 0.160 mol/L Mg(OH)2 (aq) required to reach equivalence with 10.00 mL of HNO3(aq). Burette Readings Final volume, V₁ (mL) Initial volume, V, (ml.) Amount of titrant added (mL) 0.195 mol/L 00.390 mol/L 0.0974 mol/L Trial 1 13.29 0.00 30 Using the data above, calculate the concentration of the HNO3(aq) 0.474 mol/L Trial 2 25.46 13.29 Trial 3 37/58 25.46 Trial 4 49.81 37.58