MaVa=MbVb can be used for simple strong acid-strong base titration calculations. Suppose 125 mL of the basic analyte has an unknown concentration, and the buret is filled with a standardized acid solution: Concentration: 1.73 M Volume: 43.0 mL What is the concentration of the base? Answer: _______ M (Enter your answer with 3 sig figs.)

MaVa=MbVb can be used for simple strong acid-strong base titration calculations. Suppose 125 mL of the basic analyte has an unknown concentration, and the buret is filled with a standardized acid solution: Concentration: 1.73 M Volume: 43.0 mL What is the concentration of the base? Answer: _______ M (Enter your answer with 3 sig figs.)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

See similar textbooks

Similar questions

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?
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction? CH3COOH + NaOH → NaCH3COO + H2O 2CH3COOH + NaOH → NaCH3COO + H2O C20H14O4 + NaOH → NaC20H14O4 + H2O CH3COOH + 2NaOH → NaCH3COO + H2O
You want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample?
Volume vinegar used (mL)= 5.00 mL % from labe= l5 % Molarity of NaOH = 0.0976 M Titration volume measurements Trial 1 Trial 2 Trial 3 Inital volume NaOH (mL) 0.69 0.86 0.16 Final volume NaOH (mL) 43.47 43.36 43.03 Volume NaOH used (mL) Average volume NaOH used (mL) Average volume NaOH used (L) Moles NaOH used (from avg volume) Moles CH3COOH Molarity CH3COOH (mol/L) Mass CH3COOH (g) % (m/v) CH3COOH in vinegar
The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.
A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS
Pls do fast and i will rate instantly for sure Solution must be in typed form A 25.0 mL volume of 0.0106 M KIO3 is pipetted into a 250-mL Erlenmeyer flask. The solution is titrated to the stoichiometric point with 16.25 mL of a sodium thiosulfate solution. What is the molar concentration of the sodium thiosulfate solution?
Molarity of (NH3) solution (M) from bottle- 5.0 Initial reading of buret (NH3) (mL)- .27 Final reading of buret (NH3) (mL)- 8.25 Volume of Cd(NO3)2 solution (mL)- 10.00 Volume of Na2C2O4 solution (mL)- 10,00 please find Total volume of solution after titration (mL) Total moles of C2O42- (mol) Molarity of C2O42- (M) Total moles of Cd2+ (mol) Moles of [Cd(NH3)4]2+ (mol) Molarity of [Cd(NH3)4]2+ (M) Moles of NH3 added by titration (mol) Moles of NH3 that did not react with Cd2+ (mol) Molarity of NH3 that did not react with Cd2+ (M) Kf for [Cd(NH3)4]2+
A standard solution of (FeSCN)2+ was prepared by mixing 5.00 mL of 0.00200 M KSCN , 6.00 mL of 0.220 M Fe(NO3)3 , and 14.00 mL of 0.050 M HNO3. What is the total volume of solution in the container after all reagents have been mixed? (please type answer not by hend )
A 24.8mL sample of vegetable juice is titrated with 15.65mL of NaOH solution. The molar concentration of the NaOH is .106 M. The molar mass of citric acid is 192.12 g-mol-1. Express all with three significant figures. 1. If the label on the bottle lists the citric acid content as 1 g per serving with a serving size of 240 mL determine the percent error in the titration results. express finale answer with 2 sig figs.
Answer the following: Maria was given a capsule of multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the sample. The student analyzed 1.032 g sample using volumetric titration. Use the table as a reference of the data to be used for your solution. Given Choices: A. 66.0 % B. 54.6% C. 65.6% D. 7.30%
A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible.What is the MW of calcium carbonate?102 g/mol98 g/mL100 g/mL100 g/molWhat is the molar concentration of the standardized EDTA solution?0.08m0.8M0.08N0.08MHow many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?0.18250.18521.8251.1852