Concept explainers
(a)
Interpretation:
Whether
(a)
Explanation of Solution
From the table
(b)
Interpretation:
Whether
(b)
Explanation of Solution
According to table
(c)
Interpretation:
Whether
(c)
Explanation of Solution
The conjugate base of a weak acid is strong. Since
(d)
Interpretation:
Whether
(d)
Explanation of Solution
The formula
(e)
Interpretation:
Whether
(e)
Explanation of Solution
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Chapter 13 Solutions
EBK INTRODUCTION TO CHEMISTRY
- Classify each of the following substances as an acid, a base, or a salt. a. HBr b. NaI c. NH4NO3 d. Ba(OH)2arrow_forwardClassify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3arrow_forwardA Liquid HF undergoes an autoionization reaction: 2HFH2F++F (a) Is KF an acid or a base in this solvent? (b) Perchloric acid, HCIO4, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction. (c) Ammonia is a strong base in this solvent. Write the chemical equation for the ionization reaction. (d) Write the net ionic equation for the neutralization of perchloric acid with ammonia in this solvent.arrow_forward
- Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2CO3 (carbonic acid) b. H2C3H2O4 (malonic acid)arrow_forward12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’arrow_forwardClassify each of the following acids as monoprotic, diprotic, or triprotic. a. HClO3 (chloric acid) b. HC3H5O4 (glyceric acid) c. H3C6H5O7 (citric acid) d. H3PO4 (phosphoric acid)arrow_forward
- Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2arrow_forwardTwo strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?arrow_forwardConsider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.arrow_forward
- Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?arrow_forwardFor each of the following pairs of acids, indicate whether the first member of the pair is a stronger or weaker acid than the second member of the pair. a. HClO4 and HClO2 b. H2SO3 and H2SO4 c. H3PO4 and HI d. HClO and HClarrow_forwardClassify each of the following salts as a strong acid strong base salt, a strong acidweak base salt, a weak acidstrong base salt, or a weak acidweak base salt. a. NaCl b. KC2H3O2 c. NH4Br d. Ba(NO3)2arrow_forward
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