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 HCl with 0.100 M NaOH. It took 14.33 mL to theendpoint. SHOW WORK!How many moles of HCl did youadd initially?How many moles of NaOH did you use in the titration?_How many moles of HCl were titrated (left over)?_How manyHow 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?III. Provide a purpose of the experiment.moles of HCl reacted with the tablet (subtract titrated from initial).

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II. Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 M solution of HCl. Then you titrated the excess HCl with 0.100 M NaOH. It took 14.33 mL to the endpoint. SHOW WORK! How many moles of HCl did you add initially? How many moles of NaOH did you use in the titration? How many moles of HCl were titrated (left over)?_

II. Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 M solution of HCl. Then you titrated the excess HCl with 0.100 M NaOH. It took 14.33 mL to the endpoint. SHOW WORK! How many moles of HCl did you add initially? How many moles of NaOH did you use in the titration? How many moles of HCl were titrated (left over)?_

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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10 Chem101 Postlab Quiz 11: BIOL 122 - Int x + -> A app.101edu.co Apps Canvas MYACU to Chem101 Q Quizlet O Khan Academy E Google Docs YouTube Question 5 of 5 A 20.0 mL solution of NaOH is neutralized with 35.0 mL of 0.200 M HBr. What is the concentration of the original NaOH solution? M 1 6. 7 +/- MacBook Pro esc 888 %23 %24 % & 2 4 7 R P Q W Y tab J K caps lock > V M shift 3. 2. 4,
Solid iron(III) hydroxide is added to 635 mL of 0.280 M HCl. The resulting solution is acidic and titrated with 1294 mL of 0.111 M NaOH. What mass of iron(III) hydroxide was added to the HCl? _____ g Thanks!
Vinegar? required to neutralize the acetic acid in each sample of vinegar, 16. Complete the calculations to find the molarity and percentage of acetic acid in vinegar. Convert the average volume of NaOH required to reach endpoint from mL to L Average volume of NaOH required to reach endpoint in mL 15. Subtract the initial volume from the final volume to calculate the volume of NaOH I DATA 269 12.55 TITRATION DATA (REPORT YOUR VOLUMES TO 1/100TH MI TRIAL 1 TRIAL 2 Initial base buret reading Final base buret reading Volume of sodium hydroxide (NaOH) required to reach endpoint in mL Volume of vinegar used O15 12.55 TRIAL 3 12:55 24.11 EXTRA TRIAL 24.11 35.39 11.78 12.05 11.56 15.00 mL 15.00 mL 15.00 mL 15.00 mL (Show calculations here.) 12.05711-56+1178 -27.54 27.54ML (Show calculations here.) a7.54ML X IL 0-02754L :0.02754L nd bon 1600 Molarity of NAOH (recorded from the standard solution bottle) 0.1 I CALCULATIONS FOR MOLARITY OF ACETIC ACID IN VINEGAR 1. Using the known molarity of…
||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…
Table 4 Pease help me figure out what I did wrong for these calcauations for Volume of 0.100 M NaOH used, Moles of NaOH used, and Moles of acetylsalicylic acid in sample. Please show all work for thumbs up. Record in significant figures. Trail 2 help on finding the mass of aspirin. Thank you Table 4. Calculations for Aspirin Titration Titration of aspirin sample with NaOH C Table view List view Trial 1 Trial 2 Mass of empty flask (g) 106.3138 121.7022 Mass of flask and aspirin (g) 107.0440 122.4362 Mass of aspirin (g) 0.7302 0.734 Initial buret reading for NaOH (mL) 46.85 49.13 Final buret reading for NaOH(mL) 9.67 12.31 Volume of 0.100 M NaOH used 56.52 61.44 (mL) 37.18 36.82 Moles of NaOH used (mol) Moles of acetylsalicylic acid in 37.18 sample (mol) 36.82
When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH, 32.50 ml of titrant are needed to reach the end point. What is the molarity of the sulfuric acid? Show all work and give the calculator and sig fig anwser.
You are directed to prepare 100 mL of a 500 mEq/L KOH standard. The primary standard used has a concentration of 0.400 Eq/L. When titrating your KOH solution, you discover that 4.0 mL of the primary standard reacted exactly with 5.0 mL of the KOH solution. a. What is the actual Eq/L concentration of the KOH solution? b. How many mEq are required to adjust the volume and concentration of the remaining 85 mL of KOH solution to 100 mL of a 500 mEq/L KOH solution? c. How many mL of 12 Eq/L KOH stock must be added in order to adjust the concentration of the KOH standard to 500 mEq/L?
Calculate the pH for each case in the titration of 50.0 mL of 0.220 M HCIO(aq) with 0.220 M KOH(aq). Use the ionizatio constant for HCIO. What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? Enter numeric value
Determine the concentration of H2SO4 when 10 mL of the surround water was collected near the C & H Sugar Company. Your sample was titrated with 5 ml of 0.5 Molar NaOH solution to neutral the pH. Determine the concentration of H2SO4 in your water sample.
EXPERIMENT 5; Acid-Base Titration A. Trial 1 Trial 2 Trial 3 5.210 g Mass of KHP 5.210 g 5.210 g (C3H,O4) Mole of KHP Initial Burette 0.00 0.50 5.00 Volume NaOH (mL) Final Burette 31.00 26.25 29.95 Volume NaOH (mL) Total Volume of NaOH (mL) Moles of NaOH Molarity of NaOH (mol/L) Calculate the average Molarity of NaOH B. Titration of Vinegar (HC,H3O2) A 2.352 g sample of Vinegar is titrated with 0.08751M NaOH, and it requires 22.31 mL of NaOH to reach the endpoint. Calculate the mass percent of acetic acid (HC,H;O,) in the vinegar sample? Hint for Calculation of Mass percent of Vinegar (HC,H;O2) 1. Calculate mole of HC,H;O2 from concentration (M) and volume of NaOH (L) needed to titrate Vinegar 2. Calculate mass (g) of Vinegar from mole of Vinegar 3. Mass % Vinegar = (calculated mass Vinegar/ 2.352 g) X 100 C. A solution of malonic acid, H;C;H¿O4 ¸was standardized by titration with 0.100 M NaOH solution. If 20.76 mL of the NaOH solution were required to neutralize completely 13.15 mL of…
esc V An analytical chemist weighs out 0.344 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 65.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. g 0x10 mol X 3 ? Explanation Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Access Check C D C Search or type URL
3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).