Using this data, fill in the following table as part of the laboratory exercise. Draw it and show thecalculations in your logbook. The following table describes four runs for standardization of your baseagainst a KNOWN concentration of acid. What is the concentration of H(an) in your sample? What is thepH?Molarity NaOH = 0.1000M Trial 1 Trial 2 Trial 3 Trial 4Volume of NaOH used, mL 10.00 10.00 10.0010.00mmol of NaOH usedmmol of unknown HCIVolume of NaOH used, mL 32.28 32.70 32.1632.41StdMolarity of unknown HCIAverage molarity of HCIDeviationAverage DeviationParts per Thousand

Given: For the experiment 1: Molarity of NaOH = 0.1 M Volume of NaOH = 10 mL For the experiment 2:…

calculations in your logbook. The following table describes four runs for standardization of your base against a KNOWN concentration of acid. What is the concentration of H (ag) in your sample? What is the pH? Molarity NaOH = 0.1000M Trial 1 Trial 2 Trial 3 Trial 4 Volume of NaOH used, mL 10.00 10.00 10.00 10.00 mmol of NaOH used mmol of unknown HCI Volume of NaOH used, mL 32.28 32.70 32.16 32.41 Std Molarity of unknown HCI Average molarity of HCI Deviation Average Deviation Parts per Thousand

calculations in your logbook. The following table describes four runs for standardization of your base against a KNOWN concentration of acid. What is the concentration of H (ag) in your sample? What is the pH? Molarity NaOH = 0.1000M Trial 1 Trial 2 Trial 3 Trial 4 Volume of NaOH used, mL 10.00 10.00 10.00 10.00 mmol of NaOH used mmol of unknown HCI Volume of NaOH used, mL 32.28 32.70 32.16 32.41 Std Molarity of unknown HCI Average molarity of HCI Deviation Average Deviation Parts per Thousand

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

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.87QE

See similar textbooks

Similar questions

What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
Consider the following six beakers. All have 100 mL of aqueous 0.1 M solutions of the following compounds: beaker A has HI beaker B has HNO2 beaker C has NaOH beaker D has Ba(OH)2 beaker E has NH4Cl beaker F has C2H5NH2 Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more Information required). (a) The pH in beaker A the pH in beaker B. (b) The pH in beaker C the pH in beaker D. (c) The % ionization in beaker A the % ionization in beaker C. (d) The pH in beaker B the pH in beaker E. (e) The pH in beaker E the pH in beaker F. (f) The pH in beaker C the pH in beaker F.
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
A certain sodium compound is dissolved in water to liberate Na+ ions and a certain negative ion. What evidence would you look for to determine whether the anion is behaving as an acid or a base? How could you tell whether the anion is a strong base? Explain how the anion could behave simultaneously as an acid and a base