Textbook Question
What is the molar solubility of AgI in 0.20 M NaCN? (a) 6.2 x 10^-4 M(b) 1.0 x 10^-1 M(c) 7.6 x 10^-2 M(d) 2.1 x 10^-3 M
Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 38
The strong acid HA is mixed with an equal molar amount of aqueous NaOH. Which of the following pictures represents the equilibrium state of the solution? (Na+ ions and solvent water molecules have been omitted for clarity.)
(A) (B) (C) (D)
Verified step by step guidance1
Identify the reaction: HA (strong acid) + NaOH (strong base) -> NaA + H2O.
Since HA is a strong acid, it will completely dissociate into H+ and A- ions.
NaOH will also completely dissociate into Na+ and OH- ions.
In an equimolar mixture, H+ ions from HA will react with OH- ions from NaOH to form water (H2O).
At equilibrium, the solution will contain water molecules and the conjugate base A- (represented by NO3- in the diagrams).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Neutralization
Acid-base neutralization is a chemical reaction where an acid reacts with a base to produce water and a salt. In this case, the strong acid HA reacts with NaOH, a strong base, resulting in the formation of water (H2O) and the conjugate base A-. This process is essential for understanding the equilibrium state of the solution after mixing the two reactants.
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Lewis Acids and Bases
Equilibrium in Chemical Reactions
Equilibrium in chemical reactions occurs when the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products. In the context of the question, identifying the equilibrium state involves recognizing the distribution of hydronium ions (H3O+) and hydroxide ions (OH-) after the neutralization reaction has reached completion.
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Ionization of Water
The ionization of water is the process where water molecules dissociate into hydronium (H3O+) and hydroxide (OH-) ions. This concept is crucial in understanding the behavior of acids and bases in solution, as the presence of these ions determines the pH and the overall chemical environment. In the equilibrium state, the balance between H3O+ and OH- ions is key to identifying the correct molecular arrangement.
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Related Practice
Textbook Question
A solution containing sulfide ions is added to a solution of 0.036 M Cu2+ and 0.044 M Fe2+. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? (a) 1.4 x 10^-16 M, FeS(b) 3.6 x 10^-35 M, CuS(c) 3.6 x 10^-35 M, FeS(d) 1.4 x 10^-16 M, C
Textbook Question
Consider the following table of standard reduction potentials: (b) Which substances can be oxidized by B2+? Which can be reduced by D?
Textbook Question
The following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.) .(c) Draw a picture that represents the equilibrium state of solution (1) after the addition of two OH-ions.
Textbook Question
The following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.)
. (b) Draw a picture that represents the equilibrium state of solution (1) after the addition of two H3O+ ions.
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Textbook Question
The following pictures represent solutions that contain one or more of the compounds H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. (Na+ ions and solvent water molecules have been omitted for clarity.)
(a) Which of the solutions are buffer solutions?