Dilution. 100 mL100 mL of a solution of hydrochloric acid with pH 5.0pH 5.0 is diluted to 1 L1 L. What is the pHPH of the diluted solution?

pH of a solution is equal to the negative logarithm of hydrogen ion concentration. Using this…

Answered: Dilution. 100 mL100 mL of a solution of…

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 92QRT

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Similar questions

A solution is tested for pH and conductivity as pictured below: The solution contains one of the following substances: HCl. NaOH, NH4Cl. HCN, NH3, HF, or NaCN. If the solute concentration is about 1.0 M, what is the identity of the solute?
Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
For an aqueous solution of acetic acid to be called distilled white vinegar it must contain 5.0% acetic acid by mass. A solution with a density of 1.05 g/mL has a pH of 2.95. Can the solution be called distilled white vinegar?
Consider the following six beakers. All have 100 mL of aqueous 0.1 M solutions of the following compounds: beaker A has HI beaker B has HNO2 beaker C has NaOH beaker D has Ba(OH)2 beaker E has NH4Cl beaker F has C2H5NH2 Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more Information required). (a) The pH in beaker A the pH in beaker B. (b) The pH in beaker C the pH in beaker D. (c) The % ionization in beaker A the % ionization in beaker C. (d) The pH in beaker B the pH in beaker E. (e) The pH in beaker E the pH in beaker F. (f) The pH in beaker C the pH in beaker F.
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
Unpolluted rain water has a pH of about 5.5. Acid rain has been shown to have a pH as low as 3.0. Calculate the [H+] ratio of acid rain to unpolluted rain.
Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.
What are the pH and ion concentrations in a solution of 0.10 M sodium formate, NaCHO2? Kb for the formate ion, HCO2 is 5.6 1011. pH [Na+] [CHO2] [OH] (a) 5.63 0.10 0.10 2.4 10-6 (b) 837 0.10 0.10 2.4 10 6 (c) 822 0.050 0.050 17 10- (d) 5.63 0.10 0.10 42 10

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Dilution. 100 mL100 mL of a solution of hydrochloric acid with pH 5.0 pH 5.0 is diluted to 1 L1 L. What is the pHPH of the diluted solution?