A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid).It requires 33.5 mL of sodium hydroxide to reach the endpoint.Use the References to access important values if needed for this question.A. What is the molarity of the sodium hydroxide solution?This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid.Submit AnswerMB. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution?2 question attempts remainingM

A) Given,mass of sodium hydrogen phthalate, (KHC8H4O4) = 1.09 gVolume of sodium hydroxide solution =…

A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 33.5 mL of sodium hydroxide to reach the endpoint. A. What is the molarity of the sodium hydroxide solution? M This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid. B. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution? M

A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 33.5 mL of sodium hydroxide to reach the endpoint. A. What is the molarity of the sodium hydroxide solution? M This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid. B. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution? M

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter6: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 43E

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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.
Reactions represented by the following equations take place in water solutions. Write each molecular equation in total ionic form, then identify spectator ions and write the equations in net ionic form. Solids that do not dissolve are designated by s, gases that do not dissolve are designated by g, and substances that dissolve but do not dissociate appear in blue. a. H2O(l)+Na2SO3(aq)+SO2(aq)2NaHSO3(aq) b. 3Cu(s)+8HNO3(aq)3Cu(NO3)2(aq)+2NO(g)+4H2O(l) c. 2HCl(aq)+CaO(s)CaCl2(aq)+H2O(l) d. CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(aq)+H2O(l) e. MnO2(s)+4HCl(aq)MnCl2(aq)+Cl2(aq)+2H2O(l) f. 2AgNO3(aq)+Cu(s)Cu(NO3)2(aq)+2Ag(s)
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?
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?
Two liters of a 1.5 M solution of sodium hydroxide are needed for a laboratory experiment. A stock solution of 5.0 M NaOH is available. How is the desired solution prepared?
Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.08 11 M NaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?
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)
Describe in words the titration of an acid with a base. Be sure to use the terms equivalence point, indicator, and end point correctly.
A solution of hydrochloric acid has a volume of 250. mL and a pH of 1.92. Exactly 250. mL of 0.0105 M NaOH is added. What is the pH of the resulting solution?
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
Equal quantities of the hypothetical strong acid HX, weak acid HA, and weak base BZ are added to separate beakers of water, producing the solutions depicted in the drawings. In the drawings, the relative amounts of each substance present in the solution (neglecting the water) are shown. Identify the acid or base that was used to produce each of the solutions (HX, HA, or BZ).

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