Determine the following using the data obtained for the HCl titration experiment (note Table above). Please make certain to show your work and that your final answers are well marked.1. Volume of NaOH2. The mmoles of 0.2M NaOH added3. The mmoles of acid4. The concentration of the HCl titrated5. The concentration of the HCl before dilution ### Titration Data from Acid-Base ExperimentThis table presents data from a titration experiment conducted using various acids: HCl, CH₃COOH, C₆H₈O₇, and H₂SO₄, all of unknown concentration. Different dilutions of H₂SO₄ were prepared: a 1:2 dilution, a 1:5 dilution, and a 1:10 dilution.#### Table 1: Titration Data| Parameter | HCl | Acetic Acid Monoprotic | Citric Acid Triprotic | 1:2 Diprotic | 1:5 Diprotic | 1:10 Diprotic ||-----------|-----|------------------------|-----------------------|--------------|--------------|---------------|| pH of Diluted Acid Solution | 1 | 3 | 2 | 0 | 1 | 1 || Volume of Acid Titrated (mL) | 30 | 30 | 30 | 20 | 20 | 20 || Initial Volume of NaOH (mL) | 0.65 | 5.20 | 0.55 | 0.10 | 1.75 | 2.45 || Final Volume of NaOH (mL) | 5.20 | 10.05 | 15.15 | 12.2 | 6.65 | 4.95 || Volume NaOH (mL) | | | | | | || Amount of 0.20M NaOH Added (mmol) | | | | | | || Amount of Acid (mmol) | | | | | | || Concentration of Acid Titrated (M) | | | | | | || Concentration of Acid Before Dilution (M)* | | | | | | |Note: Additional calculations needed for complete data on NaOH volume, amount in mmol, and concentrations.This data can be used to calculate the exact concentration of acids, considering the titration endpoints and volumes.

Initial volume of sodium hydroxide = 0.65 ml Final volume of sodium hydroxide = 5.20 ml Volume of…

Determine the following using the data obtained for the HCI titration experiment (note lable above). Please make certain to show your work and that your final answers are well marked. 1. volume of NaOH 2. the mmoles of 0.2M NaOH added 3. the mmoles of acid 4. the concentration of the HCI titrated

Determine the following using the data obtained for the HCI titration experiment (note lable above). Please make certain to show your work and that your final answers are well marked. 1. volume of NaOH 2. the mmoles of 0.2M NaOH added 3. the mmoles of acid 4. the concentration of the HCI titrated

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

#49 I keep getting.2179 but the book says half of that, at.1090
HCl is a: strong acid strong base weak acid weak base NaOH is a: strong acid strong base weak acid weak base What should be the equivalence point pH be for this experiment? a. less than 7 b.equal to 7 c. greater than 7 Assume it takes 2.80 mL of 0.1100 M NaOH to titrate 5.00 mL of HCl. Calculate the concentration of HCl using this data (and show your work!)
1. The Kb of HONH2 is 1.1 x 10-8. Calculate the pH and percent dissociation of a solution containing 0.100 M HONH2. а. b. Calculate the pH and percent dissociation of a mixture containing 0.100 MHONH2 and 0.100 M HONH3CI.
the pH at the equivalence point MISSED THIS? Read Section 18.4 (Pages 803 - 817) ; Watch_KCV 18.4A, IWE 18.6 . Express your answer as a whole number. Consider the titration of a 38.0 mL sample of 0.170 M HBr with 0.200 M KOH. Determine each of the following: pH = Submit Request Answer Part E the pH after adding 5.0 mL of base beyond the equivalence point Express your answer using two decimal places ? pH = Submit Request Answer
Pls help me !! A 150.0 mL sample of 0.21 M HF is titrated with 0.50 M NaOH. Determine the pH at these points: a.At the beginning (before base is added) b.After adding 40.0 mL of NaOH After adding c.63.0 mL of NaOH 9
2. From the graph at the right, determine a. If the acids/bases are strong or weak b. Whether the acid or base was added from the buret c. Volume required to reach the equivalence point 14 12- 10- 8- Hd 6- 9 4 2. 0 10 20 30 Volume of NaOH (mL) 40 50 -50
2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186
Please answer this question with steps thanks.
35 A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K² of bases at 25 °C tables for additional information. a Part 1 of 4 0.00 mL Added, pH = Part 2 of 4 10.0 mL Added, pH = x10 X x10 X
1. The acid form of bromophenol blue (???) is yellow; the base form (??−) is blue. Approximately what wavelength of visible light do you think each of these forms will absorb? Briefly explain. 2. Solution ?3 is considered to be the acid form of the indicator. Solution ?3 is considered to be the basic form of the indicator. Consider Le Chatelier’s Principle and explain why this is so.
please see attached image. Im trying to calulate moles of HCl the volume I drew was 5.0 the volume titrated bas 8.15.
#15 Writing K Expressi 1. Balance each equation and write an expression for the equilibrium constant, Kc.l a. NO₂Cl (9) NO₂ (g) + Cl₂ (9) b. C. d. e. POCI3 (9) NH3 (9) O₂ (g) NO (9) d. HF a. HBrO b. HC2H302 c. HCIO₂ + 03 (9) PC13 (9) + O₂ (g) N₂ (g) 03 (9) NO₂ (g) 2. Write a balanced Bronsted Lowry acid base reaction with each of the following weak acids and water. Also, write a Ka expression for each weak acid. + H₂O (9) O₂ (g) MHD