1. Acetic acid is a classic example of aEnter the correct word or phrase:2. If the concentration of H3O+ in aqueous solution is 10-⁹ M, then the pH isEnter the exact value. Ⓒtype of acid because it can donate a proton to water, forming H3O+ (aq).3. Aqueous ammonia is a classic example of aEnter the correct word or phrase:HCN + NaCNHCI + NaOHHNO3 + NaNO34. Which two of the following mixtures would be considered buffer solutions?Select all of the correct answers:OHF + NaF✔HCI + NaCltype of base because it can accept a proton to form NH4+ (aq). 7. Which of the following acids is strongest, based on the values of their acid ionization constants?Select only the best answer:O carbonic acidO hydrazoic acidO sulfuric acidO benzoic acidO oxalic acid8. In the autoionization reaction of water, the conjugate base of H3O+(aq) isSelect only the best answer:OH3O+ (aq)O pHO KwO OH-(aq)Ⓒ H₂O(l)

Arrhenius acid is a substance which dissociates in water and produces H+ ions is called Arrhenius…

1. Acetic acid is a classic example of a Enter the correct word or phrase: 2. If the concentration of H3O+ in aqueous solution is 10-9 M, then the pH is Enter the exact value. Ⓒ 3. Aqueous ammonia is a classic example of a Enter the correct word or phrase: type of acid because it can donate a proton to water, forming H3O+ (aq). HCN + NaCN HCI + NaOH 4. Which two of the following mixtures would be considered buffer solutions? Select all of the correct answers: ⒸHF + NaF HNO3 + NaNO3 ✔HCI + NaCl type of base because it can accept a proton to form NH4+ (aq).

1. Acetic acid is a classic example of a Enter the correct word or phrase: 2. If the concentration of H3O+ in aqueous solution is 10-9 M, then the pH is Enter the exact value. Ⓒ 3. Aqueous ammonia is a classic example of a Enter the correct word or phrase: type of acid because it can donate a proton to water, forming H3O+ (aq). HCN + NaCN HCI + NaOH 4. Which two of the following mixtures would be considered buffer solutions? Select all of the correct answers: ⒸHF + NaF HNO3 + NaNO3 ✔HCI + NaCl type of base because it can accept a proton to form NH4+ (aq).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 116QRT

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Similar questions

What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Define pH and explain why pH, rather than molarity, is used as a concentration measure of H3O+.
What is meant by “pH”? True or false: A strong acid always has a lower pH than a weak acid does. Explain.
. 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 NaOH
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.
A solution of baking soda, NaHCO3, has a pH of 10.08. What is the percent (by mass) of NaHCO3 in a 235-mL solution? (Assume a density of 1.00 g/mL.)
(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic? (d) A 10.0-mL sample of 2.56 M HCl is diluted with water to 250. mL What is the pH of the dilute solution?
To measure the relative strengths of bases stronger than OH, it is necessary to choose a solvent that is a weaker acid than water. One such solvent is liquid ammonia. (a) Write a chemical equation for the autoionization of ammonia. (b) What is the strongest acid and base that can exist in liquid ammonia? (c) Will a solution of HCI in liquid ammonia be a strong electrical conductor, a weak conductor, or a nonconductor? (d) Oxide ion (O2) is a stronger base than the amide ion (NH2). Write an equation for the reaction of O2 with NH3 in liquid ammonia. Will the equilibrium favor products or reactants?
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
Indicate whether each of the following samples is acidic, basic, or neutral. a. butter, pH 6.1 b. lemon juice, pH 2.2 c. peach, pH 3.5 d. milk of magnesia, pH 10.5
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2