To determine the amount of a hypothetical compound KHA · H2A 2H2O in a pure sample, Senku asked his friend Chrome to titrate it with 0.100M NaOH. Unfortunately, an accident occurred while he was away and all of the 50.0 mL NaOH solution was mixed into the sample. To remedy the situation, Senku decided to perform back titration with a 2.375 mL of 0.0800M H2SO4 solution. a) How many excess moles of NaOH were added to the solution? b) How many moles of the compound KHA·H¿A-2H2O are present in the sample? c) When the reaction between the same sample of KHA:H2A•2H2O and NaOH was carried out in a coffee cup calorimeter, the measured total temperature rise from 25.0°C was 54.0°C. Determine the magnitude of the heat of the neutralization of KHA·H»A•2H2O and NaOH in Joules. Assume that the Cp of the solution is 18.0 cal/mol-K. (

To determine the amount of a hypothetical compound KHA · H2A 2H2O in a pure sample, Senku asked his friend Chrome to titrate it with 0.100M NaOH. Unfortunately, an accident occurred while he was away and all of the 50.0 mL NaOH solution was mixed into the sample. To remedy the situation, Senku decided to perform back titration with a 2.375 mL of 0.0800M H2SO4 solution. a) How many excess moles of NaOH were added to the solution? b) How many moles of the compound KHA·H¿A-2H2O are present in the sample? c) When the reaction between the same sample of KHA:H2A•2H2O and NaOH was carried out in a coffee cup calorimeter, the measured total temperature rise from 25.0°C was 54.0°C. Determine the magnitude of the heat of the neutralization of KHA·H»A•2H2O and NaOH in Joules. Assume that the Cp of the solution is 18.0 cal/mol-K. (

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solution with unknown concentration was prepared. A 25.00 mL sample of the stock HCH5O2 solution was titrated with 0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an indicator. The titration took 20.26 mL of titrant (sodium hydroxide). (b) Write a balanced complete ionic equation for the chemical reaction that occurs in this titration.
Excess solid Ni(OH)2 was added to water and the resulting solution was allowed to stand for several days. The solution was then filtered to remove excess solid Ni(OH)2. A 0.250 L aliquot of the solution was then titrated with 10.54 mL of a standardized 0.000500 M HCl solution. What is the Ksp of Ni(OH)2?
51. Suppose 100.0 mL of a 0.3750 M solution of the strong base Ba(OH)2 is titrated with a 0.4540 M solution of the strong acid HCIO4. The neutralization reaction is Ba(OH), (aq) + 2 HCIO, (aq) –→ Ba(CIO,)2 (aq) + 2 H,0(e) Compute the pH of the titration solution before is added, when the titration is 1.00 mL short of the equiv- alence point, when the titration is at the equivalence point, and when the titration is 1.00 mL past the equivalence point. (Note: Each mole of Ba(OH)2 gives two moles of OH in solution.) any acid
17.69 mL of the I2 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H2O) + 2I2 → 2(H3AsO4) + 4HI
You are running an acid-base titration with hydrochloric acid and calcium hydroxide. The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M. You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator. To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution. Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached. You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial. You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator. You refill the buret to an initial volume of 1.42 mL. When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial. You add 25.6 mL of hydrochloric acid solution…
Standard silver nitrate solutions can be used in a precipitation titration to determine iodide levels. What is the molarity of an iodide solution when 20.00 mL of the solution required 15.50 mL of a 0.0045 M AgNO3 standard? The reaction is I- + AgNO3 --> AgI + NO3-.
A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If 21.68 mLmL of the NaOHNaOH solution were required to neutralize completely 13.00 mLmL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O
63.0 mL of Ca(OH)2 solution was titrated with 21.5 mL of 0.467 MHNO3. Determine the molarity of the Ca(OH)2 solution.
A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
Use the following balanced chemical equation to answer the below question: 2H&PO4 (aq) +3Mg(OH)2 (aq) 6H2O m + Mg3(PO4)2 (s) The titration of a 14.0 mL sample of H3PO, requires 3.51 mL of 0.400 M Mg(OH)2 to reach the equivalence point. What is the concentration of H3PO,?
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
You have three flasks with 0.03 M chloride, bromide & iodide ions. If you titrated a mixture containing the three ions with silver nitrate, what order will the equivalence points appear in the titration curve? Ksp AgCl = 1.8 x 10^-10 Ksp AgBr = 5.0x10^-13 Ksp Agl = 8.3 x 10^-17