Concept explainers
(a)
Interpretation:
Among the given letters in the boxes which is appropriate for having
Concept Introduction:
(b)
Interpretation:
Among the given letters in the boxes which is appropriate for having a conjugate acid or conjugate base of another item in the grid has to be determined.
Concept Introduction:
Acid-base conjugate pairs differ by one
(c)
Interpretation:
Among the given letters in the boxes which is having a
Concept Introduction:
(d)
Interpretation:
Among the given letters in the boxes which is appropriately describing a polyprotic acid has to be determined.
Concept Introduction:
A polyprotic acid has more than one acidic hydrogen.
(e)
Interpretation:
Among the given letters in the boxes which is appropriate for describing
Concept Introduction:
If a compound can act both as an acid and as a base, the value of
(f)
Interpretation:
Among the given letters in the boxes which is appropriate for describing a basic salt has to be determined.
Concept Introduction:
A basic salt is a salt that contains an anion that is the conjugate acid of a weak acid.
(g)
Interpretation:
Among the given letters in the boxes which is appropriate for having
Concept Introduction:
(h)
Interpretation:
Among the given letters in the boxes which is appropriate for describing a Lewis acid has to be determined.
Concept Introduction:
Lewis acid is an electron pair acceptor.
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Chapter 14 Solutions
Chemistry: The Molecular Science
- 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_forwardAssuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.arrow_forwardCalculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxidearrow_forward
- Two strategies are followed when solving for the pH of an acid in water. What is the strategy for calculating the pH of a strong acid in water? What major assumptions are made when solving strong acid problems? The best way to recognize strong acids is to memorize them. List the six common strong acids (the two not listed in the text are HBr and HI). Most acids, by contrast, are weak acids. When solving for the pH of a weak acid in water, you must have the Ka value. List two places in this text that provide Ka values for weak acids. You can utilize these tables to help you recognize weak acids. What is the strategy for calculating the pH of a weak acid in water? What assumptions are generally made? What is the 5% rule? If the 5% rule fails, how do you calculate the pH of a weak acid in water?arrow_forwardIn the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.arrow_forwardComplete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+arrow_forward
- Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2arrow_forwardHow do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.arrow_forward
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