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 0.244-g sample of an unknown monoprotic acid was titrated with 0.127 M NaOH and the resulting titration curve is shown here. pH 14 12 10 60 42 0 0 10 20 30 40 50 60 Volume of base added (mL) Part A Determine the molar mass of the acid. Express your answer in grams per mole to two significant figures. 17 ΑΣΦ Submit Part B Request Answer pK₂ = Determine the pK, of the acid. Express your answer to one significant figure. ? 15. ΑΣΦ P g/mol ?
None
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
Number 1_ A 0.5707-g sample of a water-soluble fertilizer was dissolved and analysed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.1334 M boric acid. This solution required 26.27 mL of 0.202 M HCl for titration to the methyl red end point. Calculate the % N (AW =14 g/mol) in the fertilizer.
A solution of 0.1789 M phosphoric acid is used to standardize an unknown solution of sodium hydroxide according to the following equation: H3PO4 + 3 NaOH → Na3PO4 + 3 H20 After performing a quick titration, the following data was collected: Trial 1 Trial 2 Initial volume H3PO4 (mL) 0.13 8.75 Final volume H3PO4 (mL) 15.73 24.08 Initial volume NaOH (mL) 11.40 0.08 Final volume NaOH (mL) 33.06 21.38 What is the concentration of the sodium hydroxide in trial 1? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the concentration of the sodium hydroxide in trial 2? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the average concentration of the sodium hydroxide? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the unit for all of these concentrations?
Consider the titration of 30.0 mL of 0.263 M weak base B (Kb = 1.3 x 10 10) with 0.150 M HI. How many mL of the HI would be required to reach the halfway point?
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
2b
Part A A 350.0 mL buffer solution is 0.150 mol Llin HF and 0.150 mol L-lin NaF. Ka(HF) = 6.3 × 10–4 What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Express your answer using two significant figures. Templates Symbols uado redo reset keyboard shortcuts help m = g Submit Request Answer Part B If the same volume of the buffer was 0.370 mol L-'in HF and 0.370 mol L-lin NaF, what mass of NaOH could be handled before the pH rises above 4.00? Express your answer using two significant figures. Templates Symbols uado redo resat keyboard shortcuts help, m =

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