Concept explainers
(a)
Interpretation:
The conjugate acid of the species should be determined.
Concept Introduction:
The conjugate acid − base pair concept arises from the Bronsted −Lowry definition for acid and base.
According to Bronsted-Lowry model, acid is defined as a proton donor and base as a proton acceptor. On donating a proton, an acid forms conjugate base and on accepting a proton base forms a conjugate acid. Thus, in a conjugate acid-base pair, substances are in relation by accepting and donating a proton.
(b)
Interpretation:
The conjugate acid of the species should be determined.
Concept Introduction:
The conjugate acid − base pair concept arises from the Bronsted −Lowry definition for acid and base.
According to Bronsted-Lowry model, acid is defined as a proton donor and base as a proton acceptor. On donating a proton, an acid forms conjugate base and on accepting a proton base forms a conjugate acid. Thus, in a conjugate acid-base pair, substances are in relation by accepting and donating a proton.
(c)
Interpretation:
The conjugate acid of the species should be determined.
Concept Introduction:
The conjugate acid − base pair concept arises from the Bronsted −Lowry definition for acid and base.
According to Bronsted-Lowry model, acid is defined as a proton donor and base as a proton acceptor. On donating a proton, an acid forms conjugate base and on accepting a proton base forms a conjugate acid. Thus, in a conjugate acid-base pair, substances are in relation by accepting and donating a proton.
(d)
Interpretation:
The conjugate acid of the species should be determined.
Concept Introduction:
The conjugate acid − base pair concept arises from the Bronsted −Lowry definition for acid and base.
According to Bronsted-Lowry model, acid is defined as a proton donor and base as a proton acceptor. On donating a proton, an acid forms conjugate base and on accepting a proton base forms a conjugate acid. Thus, in a conjugate acid-base pair, substances are in relation by accepting and donating a proton.
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Introductory Chemistry: A Foundation
- Explain the difference between a strong acid and a weak acid.arrow_forward. For each hydrogen or hydroxide ion concentration listed. calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+]=5.72104M b. [OH-]=8.91105Mc. [H+]=2.871012Md. [OH-]=7.22108Marrow_forwardA 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000arrow_forward
- For 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_forwardWrite equations to illustrate the acid-base reaction when each of the following pairs of Brnsted acids and bases are combined: Acid Base a.HOCl H2O b.HClO4 NH3 c.H2O NH2 d.H2O OCl e.HC2O4 H2Oarrow_forwardCompare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the acid in Exercise 21d. Explain the large difference in percent dissociation of the acid.arrow_forward
- (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?arrow_forwardEach of the following statements concerns a 0.010 M solution of a weak acid, HA. Briefly describe why each statement is either true or false. a [HA] is approximately equal to 0.010 M. b [HA] is much greater than [A]. c [OH] is approximately equal to [H3O+]. d The pH is 2. e The H3O concentration is 0.010 M. f [H3O+] is approximately equal to [A].arrow_forwardSolution A has a pH of 2.0. Solution B has a pH of 5.0 Which solution is more acidic? Based on the H+ ion concentrations in the two solutions, how many times more acidic?arrow_forward
- Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.arrow_forwardMark each of the following statements True or False: a. The conjugate base of a strong acid is always a weak base. b. The conjugate acid of a strong base is always a weak acid. c. The stronger the acid, the weaker its conjugate base, and vice versa.arrow_forwardWhat two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak base?arrow_forward
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