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(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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Chapter 13 Solutions
Bundle: Chemistry: An Atoms First Approach, 2nd, Loose-Leaf + OWLv2, 4 terms (24 months) Printed Access Card
- 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
- Strong 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_forwardEach box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?arrow_forwardAqueous Solutions of Acids, Bases, and Salts a For each of the following salts, write the reaction that occurs when it dissociates in water: NaCl(s), NaCN(s), KClO2(s), NH4NO3(s), KBr(aq), and NaF(s). b Consider each of the reactions that you wrote above, and identify the aqueous ions that could be proton donors (acids) or proton acceptors (bases). Briefly explain how you decided which ions to choose. c For each of the acids and bases that you identified in pan b, write the chemical reaction it can undergo in aqueous solution (its reaction with water). d Are there any reactions that you have written above that you anticipate will occur to such an extent that the pH of the solution will be affected? As pan of your answer, be sure to explain how you decided. e Assume that in each case above, 0.01 mol of the salt was dissolved in enough water at 25C to make 1.0 L of solution. In each case what additional information would you need in order to calculate the pH? If there are cases where no additional information is required, be sure to state that as well. f Say you take 0.01 mol of NH4CN and dissolve it in enough water at 25C to make 1.0 L of solution. Using chemical reactions and words, explain how you would go about determining what effect this salt will have on the pH of the solution. Be sure to list any additional information you would need to arrive at an answer.arrow_forward
- How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?arrow_forward. Consider 0.25 M solutions of the following salts: NaCl. RbOC1, KI, Ba(ClO4),, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.arrow_forwardWhat two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak base?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_forwardConsider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000?arrow_forwardWhat is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?arrow_forward
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