An aqueous solution contains 0.417 M nitrous acid.Calculate the pH of the solution after the addition of 5.38x10-2 moles of sodium hydroxide to 250 mL of this solution.(Assume that the volume does not change upon adding sodium hydroxide).pH =*3#Submit Answer80EC$4RFRetry Entire Group 5 more group attempts remaining%Use the References to access important values if needed for this question.5VCengage Learning | Cengage Technical SupportTG6BYH&7UN*8JAIM(9K7O<)014P^.PreviousEmail Instructor Save and Exit+ 11{[ONext=Lde

Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

An aqueous solution contains 0.417 M nitrous acid. Calculate the pH of the solution after the addition of 5.38x102 moles of sodium hydroxide to 250 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH =

An aqueous solution contains 0.417 M nitrous acid. Calculate the pH of the solution after the addition of 5.38x102 moles of sodium hydroxide to 250 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH =

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 16.36QE

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

An aqueous solution contains 0.417 M nitrous acid.
Calculate the pH of the solution after the addition of 5.38x10-2 moles of sodium hydroxide to 250 mL of this solution.
(Assume that the volume does not change upon adding sodium hydroxide).
pH =
*3
#
Submit Answer
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Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.
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.
The following are representations of acidbase reactions: a. Label each of the species in both equations as an acid or a base and explain your answers. b. For those species that are acids, which labels apply: Arrhenius acid, BrnstedLowry acid, Lewis acid? What about the bases?
A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH], and the pH for this solution. [Hint: Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/mL.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?