Part AA sample of 0.224 g of an unknown monoproticacid was dissolved in 25.0 mL of water and titratedwith 0.0950 M NaOH. The acid required 30.0 mLof base to reach the equivalence point.What is the molar mass of the acid?Express your answer as a molar mass.ΜΕ ΑΣΦMmol =SubmitRequest AnswerPart B?g/molAfter 15.0 mL of base had been added in the titration, the pH was found to be 6.50. What is the K for the unknown acid?Express your answer using two significant figures.ΜΕ ΑΣΦK₁ =SubmitRequest Answer?

Part A: Let, molar mass of the sample be x g/mol.Weight of the sample is 0.224g As the sample of…

Answered: Part A A sample of 0.224 g of an…

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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A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.
Answer the following questions about a titration between 25.0 mL of a weak base (Kb= 6.9*10-5) and 0.100 M hydrochloric acid). A.What is the concentration of the weak base solution if it requires 37.50 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of ethyl red is ~ 5.4 and the pKa of thymol ~ 8.4. Which indicator would be best to use in the titration?
A 100.0 mL buffer solution is 0.110 mol L-¹ in CH3NH2 and 0.130 mol L-¹ in CH3NH₂Br. Part A What mass of HCI will this buffer neutralize before the pH falls below 9.55? ( Kb (CH3NH₂) = 4.40 × 10-4) Express the mass in grams to two significant figures. mun shummu za
Titration You are titrating 10 mL 0.050 M benzoic acid (pK, = 4.19) with 0.025 M sodium hydroxide.
MISSED THIS? Read Section 18.4 (Page); Watch KCV 18.4B. Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. Hd 14 12 10 8 6420 80 120 160 40 Volume of base added (mL) The figure shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 160 milliliters on the x-axis. The curve of the plot goes up gradually from pH 2.3 at 0 milliliters to pH 5.8 at 49 milliliters, next the plot goes up steeply to pH 11.8 at 51 milliliters, and finally the plot goes up gradually to pH 12.2 at 160 milliliters. ✓ Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in way. Part D At what volume of added base does pH =…
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Select the answer that best describes the experimental setup of the titration curve shown in the image below 12 Hd H] 8 4 0 10 volume of titrant (mL) 20 20 strong base (beaker) and strong acid (burette) weak base (beaker) and strong acid (burette) weak acid (beaker) and strong base (burette) strong acid (beaker) and strong base (burette)
An unknown weak monoprotic acid (20.0 g) with a mass concentration of 1.98 g/L was titrated with a standardized 1.00 M NaOH titrant. The weak acid had a pH of 3.28 and required 0.58 mL of NaOH titrant to reach neutralization. What is the concentration of HA before titration? What is the concentration of H+ before titration? What is the concentration of A- before titration? What is the Ka of the weak acid? Find the pKa of the weak acid.
Pls ans all
A student performed three H2SO4 titrations in Part 2 using their 0.1048 M NaOH solution which they previously standardized in Part 1. They reported the following measurements: Determination #1 Determination #2 Determination #3 Final NaOH Burette Reading 37.65 mL 28.35 mL 26.23 mL Initial NaOH Burette Reading 12.80 mL 4.05 mL 1.73 mL For every 1 mole of H2SO4, how many moles of NaOH are needed to reach equivalence in the titration? Report the integer number only (no units).
Please show your solutions. The correct answer is provided. Thank you. CORRECT ANSWER: 30.00

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