Learning Task 11: Try to solve the following titration problems. Show your completesolution.1. An acid-base titration is performed in which 26.05 mL of 0.1000M H₂SO4 solutionwas needed to reach the endpoint of a 25mL NaOH solution with unknownconcentration. The chemical reaction involved in this titration is as follows:H₂SO4 (a) + 2NaOH(a)→ H₂O + Na2SO4 (Calculate for the molarity of the NaOH solution.2. Suppose a titration needed 27.15 mL of 0.2497M HCl solution to completely react25.00mL of Ba(OH)2 solution of unknown concentration. Identify and balance thechemical equation involved, then calculate for the concentration of the Ba(OH)2solution.

Answered: Image /qna-images/answer/af2cbee8-8f30-4cd1-9e9e-8a7dfc1004df.jpg

1. An acid-base titration is performed in which 26.05 mL of 0.1000M H₂SO4 solution was needed to reach the endpoint of a 25mL NaOH solution with unknown concentration. The chemical reaction involved in this titration is as follows: H₂SO4 (a) + 2NaOH(aq) → H₂O + Na2SO4 (0) Calculate for the molarity of the NaOH solution. 2. Suppose a titration needed 27.15 mL of 0.2497M HCl solution to completely react 25.00mL of Ba(OH)2 solution of unknown concentration. Identify and balance the chemical equation involved, then calculate for the concentration of the Ba(OH)2 solution.

1. An acid-base titration is performed in which 26.05 mL of 0.1000M H₂SO4 solution was needed to reach the endpoint of a 25mL NaOH solution with unknown concentration. The chemical reaction involved in this titration is as follows: H₂SO4 (a) + 2NaOH(aq) → H₂O + Na2SO4 (0) Calculate for the molarity of the NaOH solution. 2. Suppose a titration needed 27.15 mL of 0.2497M HCl solution to completely react 25.00mL of Ba(OH)2 solution of unknown concentration. Identify and balance the chemical equation involved, then calculate for the concentration of the Ba(OH)2 solution.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 70QAP: Three students titrate different samples of the same solution of HCI to obtain its molarity. Below...

See similar textbooks

Similar questions

Three students titrate different samples of the same solution of HCI to obtain its molarity. Below are their data. Student A: 20.00mLHCl+20.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student B: 20.00mLHCl+40.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student C: 20.00mLHCl+20.00mLH2O 0.100 M Ba(OH)2 used to titrate to the equivalence point. All the students calculated the molarities correctly. Which (if any) of the following statements are true? (a) The molarity calculated by A is half that calculated by B. (b) The molarity calculated by A is equal to that calculated by C. (c) The molarity calculated by B is twice that calculated by C. (d) The molarity calculated by A is twice that calculated by B. (e) The molarity calculated by A is equal to that calculated by B.
You are titrating 10.00 mL 0.100 M H3PO4 with 0.100 M NaOH. At the point where you have added precisely 12.00 mL of the NaOH titrant, which TWO of the following species are the major species (accounting for reactions between the phosphoric acid and sodium hydroxide)? Which is present at higher concentration, which at lower concentration? Classify each of the species as ONE of the following: N = not a major species L = major species, lower concentration H = major species, higher concentration Enter N, L, or H for each of these. (There should be one L, one H, and the rest should be N. No partial credit.) [A] H+ [B] H3PO4 [C] H2PO4- [D] HPO42- [E] PO43- [F] OH-
What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M? A 34.1 % (NH4 )2SO4 (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) NEED HELP ASAP NO WORK NEEDED
A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).
Chem. 1A: Acid-Base titration : to determine molar mass of a diprotic ACID : H2A Put a weighing paper on the pan of balance and tare it. Then add 0.1482 g of an unknown diprotic acid. Transfer the acid to a Erlenmeyer flask add 35.0 mL. water and 4 drops phenophethaleine. The color of solution is colorless. Set up a 50.00 mL. buret: wash the buret with tap water twice, with deionized water twice and and the 0.1029 M NAOH(aq). Fill the buret with 0.1029 M NaOH(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Put the Erlenmeyer flask containing the acid and the phenolphethaleine below the buret with 0.1029 M NAOH(aq). Add NaOH(aq) from buret to the Erlenmeyer flask containing the diprotic acid and phenolphethaleine , until the color of the solution turn to pink by adding one or two drops of NaOH(aq). Then stop adding NaOH(aq) from buret and read the final volume of NaOH(aq). Acid-base titration: buret base of known concentration + stopcock acid of unknown…
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
This question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…
Show your work, use general chemistry rules for significant figures. 6. A solution is made by dissolving 1.0 x 10–4 mol of Na3PO4 in 200.00 mL of water. Then 0.25 mL of 0.200 F HCl is added to the solution. H3PO4 ⇌ H+ + H2PO4– Ka1 = 7.11 x 10–3 H2PO4– ⇌ H+ + HPO42– Ka2 = 6.34 x 10–8 HPO42– ⇌ H+ + PO43– Ka3 = 4.17 x 10–13 (a) What is the pH of the resultant solution? (b) An additional 0.75mL of 0.200 F HCl is added to the solution from the end of part (a). What is the pH of the resultant solution? (c) Finally, an additional 0.50 mL of 0.200 F HCl is added to the solution from the end of part (b). What is the pH of the resultant solution?
Consider the reaction of a 20.0 mL of 0.220 M C;H;NHCI (Ka = 5.9 x 10) with 12.0 mL of 0.239 M CSOH. Write the net ionic equation for the reaction that takes place. What quantity in moles of C;H;NH" would be present at the start of the titration? What quantity in moles of OH" would be present if 12.0 mL of OH were added? -What species would be left in the beaker after the reaction goes to completion? d. What quantity in moles of C,H,NH would be left in the beaker after the reaction goes to completion?
Part 3 Prepare a data table for the titration of NaOH with diluted vinegar. Include enough data columns for at least 3 titrations. PRELAB QUESTIONS 1. Calculate the molar mass of Potassium acid phthalate, KHC8H404 (KHP). You will use this number to do the calculations for part 1 once you do the titration. 2. Calculate the molar mass of acetic acid, HC₂H3O2. You will use this number to do the calculations for part 3 once you do the titration. 3. Solve the following problem: If it takes 35.04 mL of a 0.2455 M NaOH solution to neutralize 25.00 mL of an unknown HCl solution, what is the molarity of the HCl solution? Use the roadmap given under part 2 to calculate this problem. MA Chemistry 60 lab Page 110 3
A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)
< Interconverting pH and hydronium ion concentration 1:23 solution A B Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write ind correct number of significant digits. с H₂O*] PH 5.9 x 10-12 mol/L mol/L 6.1 x 10 mol/LO 1.22 Today 1:22 AM 317 .5G → Edit رت Ep