Concept explainers
(a)
Interpretation:
The given statement ‘
(a)
Explanation of Solution
The given acids are
Thus, the given statement is an incorrect statement.
(b)
Interpretation:
The given statement ‘
(b)
Explanation of Solution
The given acids are
Thus, the given statement is an incorrect statement.
(c)
Interpretation:
The given statement ‘
(c)
Explanation of Solution
The given acids are
Thus, the given statement is an incorrect statement.
(d)
Interpretation:
The statement ‘
(d)
Explanation of Solution
The given acid is
Thus, the given statement is an incorrect statement.
(e)
Interpretation:
The statement ‘
(e)
Explanation of Solution
The given acids are
The given statement is the correct statement.
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Chapter 13 Solutions
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- In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()arrow_forwardAn aqueous solution contains formic acid and formate ion. Determine the direction in which the pH will change if each of the following chemicals is added to the solution. (a) HCl (b) NaHSO4 (c) CH3COONa (d) KBr (e) H2Oarrow_forwardClassify each of the following substances as an acid, a base, or a salt. a. AlPO4 b. KOH c. HNO3 d. HC2H3O2arrow_forward
- Explain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H3PO4 and a salt of its conjugate base NaH2PO4.arrow_forwardIn each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()arrow_forwardThe base ethylamine (CH3CH2NH2) has a Kb of. A closely related base, ethanolamine(HOCH2CH2NH2), has a Kb of 3.2105. (a) Which of the two bases is stronger? (b) Calculate the pH of a 0.10M solution of the strong base?arrow_forward
- Classify 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(a) Which is the stronger Bronsted acid, HCO3 or NH4+? Which has the stronger conjugate base? (b) Is a reaction between HCO3- ions and NH3 product- or reactant-favored at equilibrium? HCO3(aq) + NH3(aq) CO32(aq) + NH4+(aq) (c) You mix solutions of sodium hydrogen phosphate and ammonia. The net ionic equation for a possible reaction is HPO42(aq) + NH3(aq) PO43(aq) + NH4+(aq) Does the equilibrium lie to the left or to the right for this reaction?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
- Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegative chlorine atom pulls electrons away from the OH bond and thus weakens it. Calculate the hydronium-ion concentration and the pH of a 0.0020 M solution of chloroacetic acid, Ka is 1.3 103.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. HNO3 and HNO2 b. HF and HBr c. H2CO3 and HClO3 d. HCN and HClarrow_forwardClassify each of the following substances as an acid, a base, or a salt. a. HBr b. NaI c. NH4NO3 d. Ba(OH)2arrow_forward
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