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Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF

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Explain the following observations: (c) although sulfuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO4 ions than SO42– ions.

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Explain the following observations: (b) HF is called a weak acid, and yet it is very reactive

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Explain the following observations: (a) NH 3 contains no ions, and yet its aqueous solutions are basic

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What is the difference between (c) an acid and a base?

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What is the difference between (b) a weak acid and a strong acid

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What is the difference between (a) a monoprotic acid and a diprotic acid?

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Which of the following solutions is the most basic? (a) 0.6 M NH 3, (b) 0.150 M KOH, (c) 0.100 M Ba(OH)2.  Explain.

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Which of the following solutions has the largest concentration of solvated protons: (a) 0.2 M LiOH, (b) 0.2 M HI, (c) 1.0 M methyl alcohol (CH3OH)? Explain

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You know that an unlabeled bottle contains a solution of one of the following: AgNO 3, CaCl2, or Al2(SO4)3. A friend suggests that you test a portion of the solution with Ba(NO 3)2 and then with NaCl solutions. Explain how these two tests together would be sufficient to determine which salt is present in the solution.

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Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb(NO3)2, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br, CO32–, NO3?

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Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could the solution contain: K+, Pb2+, Ba2+

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Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (b) Fe(NO3)2 (aq) + KOH (aq) →

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Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (b) Ba(NO3)2 (aq) + K2SO4 (aq) →

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Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) Cr2(SO4)3 (aq) + (NH4)2CO3 (aq) →

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Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (c) (NH4)3PO4(aq) and CaCl2(aq)

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Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (b) Pb(NO3)2(aq) and Na2S(aq)

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Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (a) Na2CO3(aq) and MgSO4(aq)

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Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (c) FeSO4 and Pb(NO3)2

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Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (b) NaNO3 and NiSO4

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Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Na2CO3 and AgNO3

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Specify what ions are present upon dissolving each of the following substances in water: (d) NaCH3COO.

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Specify what ions are present upon dissolving each of the following substances in water: (c) HClO4

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Specify what ions are present upon dissolving each of the following substances in water: (b) Al(NO3)3

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Specify what ions are present upon dissolving each of the following substances in water: (a) MgI2

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