Use the excel data information to answer the question. FileHome InsertPage Layout Formulas DataReview View HelpX CutCalibri11A ATab Wrap TextGeneralCopyPasteVFormat PainterClipboardFontBIU MONEAlignmentMerge & Center ▾$ % 950000LГУNumberHConditional Format asFormatting Table▾StylesB11ODX ✓ £22.5ABCDEFGHJKLMN1 pH2 Moles NaOH3 Moles Unknown Acid4 Molarity Unknown Acid5 Total Moles Acid6 Molar Mass of Acid7 Initial NaOH (mL)42.58 Initial pH2.919 Volume 1st half7.510 Volume 1st EP12.511 Volume 2nd half22.512 Volume 2nd EP26.51314151617181920212223 Supporting Calculations.Include an annotated sample calculation showing how you determined the molar mass ofthe unknown diprotic acid (i.e. How did you find the equivalence point, and use that valueto calculate the molar mass of the unknown acid?).Include an annotated calculation showing how you determined the K₁₁ and Kaz (i.e. Howdid you find Kai and Ka2?).Provide a percent error comparing your experimental molar mass to theaccepted value.

1To calculate the molar mass of an unknown diprotic acid from a titration experiment, follow these…

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Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 62P

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Similar questions

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.
When might a pH meter be better than an indicator to determine the end point of an acid-base titration?
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.
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.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
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.
Use the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.)
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
0.185 M in HCHO2 (Ka = 1.8 ×x 10-4) and 0.230 M in HC2H3O2 (Ka = 1.8 × 10-5) Express your answer to two decimal places. ? Find the pH of each mixture of acids. pH = 2.11 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining In a mixture of two acids that have similar K, values, the dissociation of one acid affects the dissociation of the other acid, and vice versa. Prepare two ICE tables (where I means initial, C means change, and E means equilibrium), one for the dissociation of HCHO2 and one for the dissociation of HC2H3O2. Use the given acid-dissociation constants to calculate the amount of H3O+ produced by each acid in the pair. Part D 6.00x10-2 M in acetic acid (Ka = 1.8 × 10-5) and 6.00×102 M in hydrocyanic acid (Ka = 4.9 × 10-10) Express your answer to two decimal places. ? pH =

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