Titration Data KHP Mass of KHP: 0.5370 g Total volume of KHP solution: 25.00 mL Titration #1 – Standardization KHP burette volume Trial 1: Initial 0.00 mL Final 1.00 mL Trial 2: Initial 0.00 mL Final 1.05 mL Trial 3: Initial 0.00 mL Final 1.03 mL NaOH burette volume Trial 1: Initial 0.00 ml Final 1.00 mL Trial 2: Initial 0.00 mL Final 1.05 mL Trial 3: Initial 0.00 mL Final 1.03 ml Titration #1 – Standardization Vinegar burette volume Trial 1: Initial 0.25 mL Final 0.52 mL Trial 2: Initial 0.52 mL Final 0.78 mL Trial 3: Initial 0.78 mL Final 1.03 ml NaOH burette volume Trial 1: Initial 0.00 ml Final 2.22 mL Trial 2: Initial 0.00 mL Final 2.23 mL Trial 3: Initial 0.00 mL Final 2.18 ml

Titration Data KHP Mass of KHP: 0.5370 g Total volume of KHP solution: 25.00 mL Titration #1 – Standardization KHP burette volume Trial 1: Initial 0.00 mL Final 1.00 mL Trial 2: Initial 0.00 mL Final 1.05 mL Trial 3: Initial 0.00 mL Final 1.03 mL NaOH burette volume Trial 1: Initial 0.00 ml Final 1.00 mL Trial 2: Initial 0.00 mL Final 1.05 mL Trial 3: Initial 0.00 mL Final 1.03 ml Titration #1 – Standardization Vinegar burette volume Trial 1: Initial 0.25 mL Final 0.52 mL Trial 2: Initial 0.52 mL Final 0.78 mL Trial 3: Initial 0.78 mL Final 1.03 ml NaOH burette volume Trial 1: Initial 0.00 ml Final 2.22 mL Trial 2: Initial 0.00 mL Final 2.23 mL Trial 3: Initial 0.00 mL Final 2.18 ml

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

See similar textbooks

Similar questions

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Molarity of titrant (NaOH): 0.4550 M Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL Write the balanced neutralization reaction that occurs when you titrate the acetic acid (HC2H3O2) with sodium hydroxide (NaOH). Hint: It’s in the background. HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Using data from all 4 titrations, calculate the average volume of standard NaOH solution required to titrate 10.00 mL of the vinegar solution (Show your work). Average volume to titrate 18.47+18.44+18.71+18.56/4= Average Volume = 18.545 mL Calculate the average number of moles of NaOH used in the titrations (show your work). Average Moles NaOH = moles Calculate or determine (give reasoning) the number of moles of acetic acid in the 10.00 mL…
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NAOH(aq): Third Rough titration First Second titration titration titration Final burette reading: 18.48 33.58 48.40 23.72 (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 38.68 20.62 23.80 5.75 4. (a) The sodium ion did not take part in this chemical reaction. What do we call such an ion? (b) Draw a simple diagram which shows how the sodium ion mixes with water in solution. What do we call this physical process? 4
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NAOH(aq): Third Rough titration First Second titration titration titration Final burette reading: 18.48 33.58 48.40 23.72 (mL) Initial burette reading: (mL) Volume of NAOH(aq) Titrated (added) (mL) 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 38.68 20.62 23.80 5.75 3. What type(s) of reactions occurred in this titration?
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L Volumes of NaOH(aq): Third titration Rough First titration Second titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) 18.48 33.58 48,40 23.72 3.48 18.48 33.60 8.73 Titrated (added) (mL) Fourth Fifth titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (ml 38.68 20.62 23.80 5.75 4 6. Calculate the molarity of the stock solution of H2SO4.
Show the complete mole ratio of S2O3- and IO3- in computing for the Molarity of the titrant. Redox Titration mass IO3(g) initial volume mL final volume mL trial 1 0.1587 0.00 3.60 trial 2 0.1571 3.60 7.17 trial 3 0.1552 7.17 10.72
A 0.9600 M NaOH solution was diluted with a factor of 4.Then the diluted solution of NaOH was titrated against an unknown acid.The volumes of NaOH(aq) titrated are shown in the table below.Volumes of NaOH(aq):RoughtitrationFirsttitrationSecondtitrationThirdtitrationThirdtitrationFinal burette reading:(mL)19.00 34.05 20.86 36.01 23.57Initial burette reading:(mL)19.00 19.07 5.76 21.02 8.54The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used ineach titration is 14.80 mL.(i) Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations andreasoning.(ii) What type of chemical reaction is this? _________________ or _______________
The molar solubility of the CdCO3 in saturated solution is given below. X = 2.3 x 10-6 What mass of CdCO3 dissolves in 250 mL to create a saturated solution? The molar mass of CdCO3 is 172.42 g/mol. CdCO3 = [?] x 10¹²] Coefficient (green) Exponent (yellow) g Enter