The following table shows data from the titration offour 10.0 mL samples of a solution containinghydrochloric acid, HCl(aq), using a 0.242 mol/L sodiumhydroxide standard solution. Bromothymol blue isused as an indicator to detect when the endpoint isreached.Titration of 10.0 mL HCl(aq) with 0.242 mol/LNaOH(aq)Trialfinal burette reading (mL)initial burette reading (mL)volume of NaOH(aq) added(mL)colour at endpoint#1 #2 #3 #417.935.0 22.9 40.10.3 17.9 5.9 22.9blue green green greena) Select the most consistent trials and calculate theaverage volume of titrant added.b) Calculate the concentration of the hydrochloricacid solution.Hint: Write a balanced chemical reaction first.You MUST show your work in the space provided.Then, record your final answers with the correctnumber of significant digits and the proper units.

Answered: Image /qna-images/answer/197362f3-3bb3-4b07-93fe-23e0e53c9afa.jpg

a) Select the most consistent trials and calculate the average volume of titrant added. b) Calculate the concentration of the hydrochloric acid solution. Hint: Write a balanced chemical reaction first.

a) Select the most consistent trials and calculate the average volume of titrant added. b) Calculate the concentration of the hydrochloric acid solution. Hint: Write a balanced chemical reaction first.

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

List the observations of a manual titration experiment and explain your expectations. This should include color change and when the equivalence point (endpoint) might be reached. When do you stop and why.
A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > A 40.0 mL of 0.200 M H₂NNH₂ was titrated with 10.0 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. Before (mol) Change (mol) After (mol) 6.00 x 10 Initial (M) Change (M) Equilibrium (M) -X 0.140-x 0 -6.00 x 10³ 0 1 1 0.200 + x H₂NNH₂(aq) 0.200 0.175 + x 7.00 x 10³ H₂NNH₂(aq) + 2 0.200 0.200 - x 0.175-x 0.100 2 -7.00 x 10" A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a…
I'd like help with the theoretical pH calculation, please. The Ka of both NH3 and CH3COOH is given. Use the picture for reference.
pure water MISSED THIS? Read Section 18.5 (Pages 817 - 822) . Express your answer in moles per liter to three significant figures. • View Available Hint(s) Calculate the molar solubility of CuX (for which = 1.27 x 10-36) in each of the following. Ksp = ? S = M Submit Part B 0.25 M CuCl2 Express your answer in moles per liter to two significant figures. • View Available Hint(s) ? S = M Submit Part C 0.23 M Na2X Express your answer in moles per liter to two significant figures. • View Available Hint(s) ΑΣφ ? S = M
In lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and a 1.0 M NaOH solution. You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. What volume (mL) of the 1.8M acetic acid solution, NaOH solution, and deionized water should you combine? Show all work.
For this virtual lab you will have to determine the concentration of a strong monoprotic acid. You will first have to dilute the 10 M sodium hydroxide solution, as your acid will have a concentration between 0.25 M and 2.5 M. You have to use between 10 mL and 50 mL of your diluted sodium hydroxide solution during the titration.
Some soluble compounds are listed in the table below. Classify each compound using the checkboxes. cccccccc name ammonia potassium nitrate hydroiodic acid potassium hydroxide Answer Submitted: name type of compound (check all that apply) ionic molecular strong weak strong weak acid acid base base 0 type of compound (check all that apply)
You are asked to determine the amounts of calcium ion in a 200 mL water sample using EDTA to titrate the sample. It took 45.5 mL of 0.3 M EDTA to reach endpoint. What is the mass (in grams) of calcium ion in the water sample? Hint: Find out moles of EDTA used to reach endpoint, relate to mol of calcium ion, convert mol of calcium to gram of calcium. The molar mass of Ca is 40.08 g/mol. Round and report your answer to the SECOND decimal place. Numeric value only, no unit.
BONUS: During a titration, ammonia is added to the flask and titrated with HCI. Looking at the titration below and the indicator table, what would be a good indicator to use for this experiment? What color change would be observed? 12 10 20 40 60 80 100 120 140 mL d.1 M HCI TABLE 16.7 Common Acid-Base Indicators Approximate pH Range over which the Color Changes Color Change Gower to higher pH) Indicator Thymol blue Micdni otanpr 3234 Filyl d Mechyl purple Broeno purpk
Please answer Q1
Based on the given tablr, which of the sample/s are non polar?
What do the ions that gave a precipitate when mixed with AgNO3 have in common? Hint given: Identify the ions and the Group of the Periodic Table to which they belong