The identity of an unknown monoprotic organic acid is determined by titration. A 0.528 g sample of the acid is titrated with 0.197 M NaOH. What is the molar mass of the compound if 21.9 mL of the NaOH solution is required to neutralize the sample? molar mass: mol The compound is 68.8% C, 4.95% H, and 26.2% 0. What is the molecular formula of the organic acid? formula:

The identity of an unknown monoprotic organic acid is determined by titration. A 0.528 g sample of the acid is titrated with 0.197 M NaOH. What is the molar mass of the compound if 21.9 mL of the NaOH solution is required to neutralize the sample? molar mass: mol The compound is 68.8% C, 4.95% H, and 26.2% 0. What is the molecular formula of the organic acid? formula:

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 16.99QE: A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid...

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A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid must be neutralized (forming the potassium salt) for an important experiment. Calculate the volume of 0.221 M KOH that is needed to neutralize 24.93 g of the acid, forming K2A.
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?
Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?
The (aq) designation listed after a solute indicates the process of hydration. Using KBr(aq) and C2H5OH(aq) as your examples, explain the process of hydration for soluble ionic compounds and for soluble covalent compounds.
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
Three acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2 Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3 Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). b When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization?
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
A 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample. a Write the net ionic equation for the complete reaction of sodium carbonate with hydrochloric acid b If 28.7 mL of 0.108 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? c What is the percent composition of the original sample?
Complete the right side of each of the following molecular equations. Then write the net ionic equations. Assume all salts formed are soluble. Acid salts are possible. a Ca(OH)2(aq) + 2H2SO4(aq) b 2H3PO4(aq) + Ca(OH)2(aq) c NaOH(aq) + H2SO4(aq) d Sr(OH)2(aq) + 2H2CO3(aq)
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.

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