can someone please help with this process Type of acid in unknown: H3ABalanced chemical equation for neutralization of acid with NaOHSavedBI IIU XI XI- EIEENormalTable viewList viewTable 5. Calculations for concentration of acid solutionSample 1Sample 2Sample 31] Volume of acid (mL)25.025.025.0[2] Burette reading of NAOH, initial (mL)2.132.483.68[3] Burette reading of NAOH, final (mL)24.1024.5225.5614] Volume of NaOH, dispensed (mL)[5] Molar concentration of NaOH (partA)[6] Molar concentration of acid solution(M)[7] Average molar concentration of acid solution (M) OoldtionTable 1. Measurements for standardization of NaOHTrial 1Trial 2Trial 31] Tared mass of KHC3H4O4 (9)0.3740.3250.35712] Burette reading of NaOH, initial (mL)4.593.614.03[3] Burette reading of NaOH, final (mL)22.0318.7721.17Part B. Molar Concentration of an Acid SolutionEnter the number corresponding to the type of acid you have1. HA32. H2A3. H3AEnter the unknown number.21Table 2. Measurements for titration of unknown acidTrial 1Trial 2Trial 3[1] Volume of acid (mL)25.025.025.0[2] Burette reading of NaOH, initial (mL)2.132.483.68[3] Burette reading of NaOH, final (mL)24.1024.5225.56Part C. Percentage by Mass of an Unknown SolidEnter the number corresponding to the type of acid you have1. HA32. H2A3. H3AEnter the unknown number.30Molar mass of the unknown acid192.14Table 3. Measurements for titriation of solidTrial 1Trial 2Trial 3[1] Mass of sample (g)26.33429.15727.111[2] Burette reading of NaOH, initial (mL)3.211.481.22[3] Burette reading of NaOH, final (mL)22.7723.4220.99

Average concentration of NaOH = 0.000105 M

Type of acid in unknown: H3A Balanced chemical equation for neutralization of acid with NaOH Saved BIIIU XI XI- EIEE 图| Normal Table view List view Table 5. Calculations for concentration of acid solution Sample 1 Sample 2 Sample 3 1] Volume of acid (mL) 25.0 25.0 25.0 [2] Burette reading of NAOH, initial (mL) 2.13 2.48 3.68 [3] Burette reading of NAOH, final (mL) 24.10 24.52 25.56 14] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (part A) [6] Molar concentration of acid solution (M) [7] Average molar concentration of acid solution (M)

Type of acid in unknown: H3A Balanced chemical equation for neutralization of acid with NaOH Saved BIIIU XI XI- EIEE 图| Normal Table view List view Table 5. Calculations for concentration of acid solution Sample 1 Sample 2 Sample 3 1] Volume of acid (mL) 25.0 25.0 25.0 [2] Burette reading of NAOH, initial (mL) 2.13 2.48 3.68 [3] Burette reading of NAOH, final (mL) 24.10 24.52 25.56 14] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (part A) [6] Molar concentration of acid solution (M) [7] Average molar concentration of acid solution (M)

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

ChapterA1: Evaluation Of Analytical Data

Section: Chapter Questions

Problem A1.22QAP

See similar textbooks

Similar questions

If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.
The calculated concentration of Ag+(aq) from the student’s data is lower than the actual concentration of the original solution. The student claims that the calculated concentration is too low because some of the AgCl(s) passed through the filter paper. Do you agree or disagree? Justify your answer.
Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.
PS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTA
for a 0.0342 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw = 1.0E-14. What are the major and minor species present? Include phase.What is the major species (other than water)? HCNOEdit What is the minor species (other than H3O+ and OH-)? (H+ are lost from or gained on the N.) CNO,e−Edit What is the concentration of the minor species present in the solution? M The number of significant digits is set to 2; the tolerance is +/-4% What is the concentration of the major species present in the solution? M The number of significant digits is set to 3; the tolerance is +/-4% What is the concentration of H3O+? M The number of significant digits is set to 2; the tolerance is +/-4% What is the…
Solid silver nitrite is slowly added to 125 mL of a sodium cyanide solution until the concentration of silver ion is 0.0523 M. The maximum amount of cyanide remaining in solution is M. Please post the answer asap please make sure the answer doesnot contain error becasue last answer provided had error so i need to resubmit the question. Thanks!
Fast pls i will give u like for sure solve this question correctly in 5 min pls A student analyzed a CaCO3 antacid tablet by neutralizing the base with an excess of .60 M HCL and back-titrating the excess with .50M NaOH. He recorded the following data: mass of tablet = 1.3g amount of active ingredient CaCO3 per label = 500 mg volume of HCl added: 25 mL initial buret reading : 34 mL final buret reading : 47.4 mL If the concentration of the provided HCl is actually higher than .60M, would the determined mass of CaCO3 in the antacid tablet be too high or too low?
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Measured mass of the precipitate 1. Filter paper was dried prior to filtration. EX _____ ET TOPIC: Standardization of Titrant 2. Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX ______ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) 3. No blank correction EX ______ ET
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided. TOPIC: Measured mass of the precipitate 1. Overignition which causes the conversion of BaSO4 precipitate to BaO. EX _____ ET2. Precipitate was not washed thoroughly. Ex _____ ET TOPIC: Standardization of Titrant 3.Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX _______ ET
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Measured mass of the precipitate Question 4 Overignition which causes the conversion of BaSO4 precipitate to BaO. EX ___ ET Question 5 Precipitate was not washed thoroughly. Ex ___ ET TOPIC: Standardization of Titrant Question 6 Adding insufficient amount of titrant to reach acceptable endpoint color: EX ___ ET
Given the equation and following values, what is the concentration of the acid? (With solution) (10*Vb)/Ma Where, Vb = final - Va Va = 10+phenolphValues: Initial Volume of Analyte: 10.150 mL Initial Volume of Titrant: 50.000 mL Final Volume of Analyte: 11.620 mL Final Volume of Titrant: 48.530 mL
A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanation