Concept explainers
(a)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
(b)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
(c)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
(d)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
(e)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
(f)
Interpretation: The given salt solutions are to be classified as basic, acidic or neutral. A balanced chemical equation is to be stated for the reactions that are not neutral, that causes the solutions to be acidic or basic.
Concept introduction: The acidic or basic character of a salt is estimated on basis of the type of acid and base that are involved in the formation of the salt. A salt formed from a strong acid and a strong base is relatively neutral.
To determine: The given salt solution is to be classified as a basic, acidic or neutral solution; a balanced chemical equation for the reaction if it is not neutral, that cause the solution to be acidic or basic.
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Check out a sample textbook solutionChapter 13 Solutions
Chemistry: An Atoms First Approach
- Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OClarrow_forwardFor oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.arrow_forwardNovocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.arrow_forward
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- 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.arrow_forwardStrong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.arrow_forward. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions. a. 1.10 M NaOH b. 2.0104M KOH c. 6.2103M CsOH d. 0.0001 M NaOHarrow_forward
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