Open Question
Classify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for values of equilibrium constants. (a) NH4F (b) (NH4)2SO3
Ch.16 - Aqueous Equilibria: Acids & Bases
Chapter 16, Problem 137
Arrange the following substances in order of increasing H3O+ concentration for a 0.10 M solution of each. (a) Zn(NO3)2 (b) Na2O (c) NaOCl (d) NaClO4 (e) HClO4
Verified step by step guidance1
Identify the nature of each substance: Determine if each substance is an acid, base, or neutral salt. This will help predict how they affect the H3O+ concentration in solution.
Consider the dissociation of each substance in water: Write the chemical equation for the dissociation of each compound in water to understand the ions produced.
Evaluate the effect on H3O+ concentration: For acids, consider how they increase H3O+ concentration. For bases, consider how they decrease H3O+ concentration by producing OH- ions. Neutral salts typically do not affect H3O+ concentration significantly.
Rank the substances: Based on the dissociation and the nature of each substance, arrange them in order of increasing H3O+ concentration.
Check for strong acids or bases: Identify if any of the substances are strong acids or bases, as they will have a more significant impact on the H3O+ concentration compared to weak acids or bases.
Related Practice
Textbook Question
Calculate the pH and the percent dissociation of the hydrated
cation in the following solutions. See Appendix C for
the value of the equilibrium constant.
(a) 0.010 M Cr1NO323
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Open Question
Baking powder contains baking soda, NaHCO3, and an acidic substance such as sodium alum, NaAl(SO4)2 ~ 12 H2O. These components react in an aqueous medium to produce CO2 gas, which “raises” the dough. Write a balanced net ionic equation for the reaction.
Open Question
For each of the Lewis acid–base reactions in Problem 16.139, draw electron-dot structures for the reactants and products, and use the curved arrow notation to represent the donation of a lone pair of electrons from the Lewis base to the Lewis acid.
Textbook Question
Classify each of the following as a Lewis acid or a Lewis
base.
(e) OH-
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Textbook Question
Which would you expect to be the stronger Lewis acid in
each of the following pairs? Explain.
(a) BF3 or BH3
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