None In the lab, an acid is usually chosen as a permanent reference standard inpreference to a base. In selecting an acid to use in a standard solution all of thefollowing factors should beconsidered except A) the acid should be highly dissociatedB) the acid should not be volatileC) salts of the acid should be solubleD) the acid should be a strong oxidizing agent E) a solution of the acid should bestable

When selecting an acid to use as a permanent reference standard in a standard solution, several…

Answered: In the lab, an acid is usually chosen…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 4STP

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The pH values listed in Table 9.1 are generally the average values for the listed materials. Most natural materials, such as body fluids and fruit juices, have pH values that cover a range for different samples. Some measured pH values for specific body fluid samples are given below. Convert each one to [H+], and classify the fluid as acidic, basic, or neutral. a.Blood, pH=7.41 b.Gastric juice, pH=1.60 c.Urine, pH=5.93 d.Saliva, pH=6.85 e.Pancreatic juice, pH=7.85
What are the equilibrium concentration of H3O+, CN and HCN in a 0.025 M solution of HCN? What is the pH of the 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.
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
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?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
Classify the following as acid-base reactions or oxidation-reduction reactions: (a) Na2S(aq)+2HCl(aq)2NaCl(aq)+H2(g) (b) 2Na(s)+2HCl(aq)2NaCl(aq)+H2(g) (c) Mg(s)+Cl2(g)MgCl2(s) (d) MgO(s)+2HCl(aq)MgCl2(aq)+H2+O(l) (e) K3P(s)+2O2(g)K3PO4(s) (f) 2KOH(aq)+H3PO4(aq)K3PO4(aq)+3H2O(l)
According to Arrhenius, ____________ produce hydrogen ions in aqueous solution, Whereas ____ produce hydroxide ions.
Gold metal will not dissolve in either concentrated nitric acid or concentrated hydrochloric acid It will dissolve, however, in aqua regia, a mixture of the two concentrated acids. The products of the reaction are the AuCl4 ion and gaseous NO. Write a balanced equation for the dissolution of gold in aqua regia.
A student is planning an investigation of an acid-base reaction. Which of the following is not an accepted method of monitoring the progress of the neutralization reaction? O a) Digital pH meter O b) Conductivity meter O c) pH paper d) Visual chemical indicator
23. Calculate the volume in liters of a 5.00 M HNO3 standard required to obtain 2.00 L of a 2.50 M solution of this acid. A) 1.50 B) 0.50 C) 1.00 D) 0.07 E) 1.80
Match the following descriptions or examples with the corresponding term. More than one description or example may be matched with each term. If a description or example does not match up with the given terms, select "None of the above". < < a substance from which a standard solution can be prepared directly solution in the buret when the volume of acid equals the volume of base in a titration solution in the flask water when a colour change occurs in a titration cannot be hygroscopic 1. Titrant 2. End Point 3. Primary Standard

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