You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) ofsulfuric acid (H2SO4).InitialFinalVolDelivered|(mL)BuretteBuretteReading(mL)Reading(mL)Trial 10.5619.20??Trial 20.5719.7Trial 30.9219.56For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units.Answer:

Initial burette reading = 0.56 ml Final burette reading = 19.20 ml Volume delivered (ml ) = ?

You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Final Vol Burette Initial Burette Delivered Reading (mL) Reading (mL) (mL) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units. Answer:

You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Final Vol Burette Initial Burette Delivered Reading (mL) Reading (mL) (mL) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units. Answer:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

See similar textbooks

Similar questions

Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M NaOH ii. 100.0 mL of 0.10 M NaOH titrated by 0.10 M HCl iii. 100.0 mL of 0.10 M CH3NH2 titrated by 0.10 M HCl iv. 100.0 mL of 0.10 M HF titrated by 0.10 M NaOH Rank the titrations in order of: a. increasing volume of titrant added to reach the equivalence point. b. increasing pH initially before any titrant has been added. c. increasing pH at the halfway point in equivalence. d. increasing pH at the equivalence point. How would the rankings change if C5H5N replaced CH3NH2 and if HOC6H5 replaced HF?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
An automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?
Consider the titration of a 23.0 mL sample of 0.110 M HC₂H3 O2 with 0.120 M NaOH. Determine each of the following. - the pH at one-half of the equivalence point Express your answer using two decimal places. pH = Submit Part E pH = ΠΙ ΑΣΦ the pH at the equivalence point Express your answer using two decimal places. Submit Request Answer VE ΑΣΦ Request Answer Pearson ? ?
What volume of 0.85 M NaOH (in mL) is needed to reach the equivalence point in a titration of 83.0 mL of 0.90 M HCIO4? Your Answer: Answer units
8. You are titrating 50.0 mL of 0.200 M propanoic acid with 0.100 M NaOH. Use the data in the table to answer the questions. Name Propanoic acid Structure CH3CH2CO2H pka 4.874 Ka 1.34 × 10-5 a) Assuming that the equivalence point is considered 100% completion, calculate the pH at the following points: 0%, 10%, 50%, 90%, 100%, and 120%. b) Sketch the titration curve. c) What would be an ideal pKa for an indicator to use in this titration?
Data Table: (include units!) Unknown Acid # Your NaOH concentration 0.10 Trial 1 Trial 2 Volume of Acid (in mL) 17ml 15ml Initial Buret reading for 15.00ml 0.00ml your NaOH Final Buret reading for 39.06ml 21.23ml your NaOH Total volume of NaOH 0.024L 0.021L used in titration