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Questions and Answers
What primary factor dictates whether a salt solution will behave as acidic, basic, or neutral?
What primary factor dictates whether a salt solution will behave as acidic, basic, or neutral?
- The concentration of the salt within the solution.
- The pressure exerted on top of the solution.
- The pH of the water used to create the solution.
- The temperature at which the solution is maintained.
- The relative acid/base strengths of the parent acid and base that formed the salt. (correct)
If a salt's base dissociation constant ($K_b$) is significantly greater than its acid dissociation constant ($K_a$), what property will the salt solution exhibit?
If a salt's base dissociation constant ($K_b$) is significantly greater than its acid dissociation constant ($K_a$), what property will the salt solution exhibit?
- The solution will demonstrate acidic characteristics.
- The solution will show basic characteristics. (correct)
- The salt will precipitate out of the solution.
- The solution will be essentially neutral in nature.
- The solution will undergo rapid decomposition.
Which salt, when dissolved in water, will produce a solution with a pH closest to 7?
Which salt, when dissolved in water, will produce a solution with a pH closest to 7?
- $NaCl$ (correct)
- $CH_3COONa$
- $Al(NO_3)_3$
- $FeBr_3$
- $NH_4Cl$
Given that the hydronium ion concentration ($H_3O^+$) in a solution is $1.0 imes 10^{-4} M$, what is the corresponding pH of the solution?
Given that the hydronium ion concentration ($H_3O^+$) in a solution is $1.0 imes 10^{-4} M$, what is the corresponding pH of the solution?
If a solution has a hydroxide ion concentration ($OH^−$) of $1.0 imes 10^{−9} M$, what is the pOH of this solution?
If a solution has a hydroxide ion concentration ($OH^−$) of $1.0 imes 10^{−9} M$, what is the pOH of this solution?
Which of the following acids fully dissociates into its ions upon dissolution in water, making it a strong acid?
Which of the following acids fully dissociates into its ions upon dissolution in water, making it a strong acid?
What chemical species remains after CH3COOH donates a proton?
What chemical species remains after CH3COOH donates a proton?
What molecular entity is formed when ammonia ($NH_3$) gains a proton?
What molecular entity is formed when ammonia ($NH_3$) gains a proton?
Which of the listed cations, when present in an aqueous solution, will cause the solution to have a pH less than 7?
Which of the listed cations, when present in an aqueous solution, will cause the solution to have a pH less than 7?
Which of the following anions will increase the hydroxide ion concentration when in aqueous solution?
Which of the following anions will increase the hydroxide ion concentration when in aqueous solution?
What is the expected behavior of a salt solution where the acid dissociation constant ($K_a$) is approximately equal to the base dissociation constant ($K_b$)?
What is the expected behavior of a salt solution where the acid dissociation constant ($K_a$) is approximately equal to the base dissociation constant ($K_b$)?
What is the energy required to break one mole of H-I bonds in the gaseous phase?
What is the energy required to break one mole of H-I bonds in the gaseous phase?
Which of the following compounds will produce the highest concentration of hydroxide ions upon dissociation?
Which of the following compounds will produce the highest concentration of hydroxide ions upon dissociation?
Upon dissolution in water, what chemical species are produced from sodium hydroxide (NaOH)?
Upon dissolution in water, what chemical species are produced from sodium hydroxide (NaOH)?
What is the chemical formula of the anion that remains when sulfuric acid ($H_2SO_4$) donates one proton?
What is the chemical formula of the anion that remains when sulfuric acid ($H_2SO_4$) donates one proton?
In an aqueous solution, which of the following ions has virtually no impact on the solution's pH level?
In an aqueous solution, which of the following ions has virtually no impact on the solution's pH level?
Which of these anions has a negligible effect on the pH of a solution?
Which of these anions has a negligible effect on the pH of a solution?
If the pOH of an aqueous solution is measured to be 3.00, what is the corresponding pH of the solution?
If the pOH of an aqueous solution is measured to be 3.00, what is the corresponding pH of the solution?
Which of the listed acids is not classified as one of the common strong acids?
Which of the listed acids is not classified as one of the common strong acids?
Which of the following cations acts as a proton donor in solution?
Which of the following cations acts as a proton donor in solution?
Which of the following anions will act as a proton acceptor in aqueous solution?
Which of the following anions will act as a proton acceptor in aqueous solution?
Which of the following cations is the resulting species when a weak base accepts a proton?
Which of the following cations is the resulting species when a weak base accepts a proton?
Which of the following salts, when dissolved in water, will result in a solution with a pH greater than 7?
Which of the following salts, when dissolved in water, will result in a solution with a pH greater than 7?
What effect does the hydrolysis of an acidic salt have on the pH of the surrounding solution?
What effect does the hydrolysis of an acidic salt have on the pH of the surrounding solution?
Which of the following ions does not undergo hydrolysis in water, resulting in a pH-neutral solution?
Which of the following ions does not undergo hydrolysis in water, resulting in a pH-neutral solution?
If a solution's hydroxide ion concentration is $1.0 imes 10^{−3} M$, what is the pH of the solution?
If a solution's hydroxide ion concentration is $1.0 imes 10^{−3} M$, what is the pH of the solution?
Which of the following cations will increase the acidity of a solution?
Which of the following cations will increase the acidity of a solution?
Which of the following salts will dissolve in water to generate a essentially pH-neutral solution?
Which of the following salts will dissolve in water to generate a essentially pH-neutral solution?
Which of the following salts dissolves in water to produce an acidic solution?
Which of the following salts dissolves in water to produce an acidic solution?
Which of the following salts, when dissolved in water, generates a basic solution?
Which of the following salts, when dissolved in water, generates a basic solution?
With a solution pH is measured to be 9, what is the corresponding pOH?
With a solution pH is measured to be 9, what is the corresponding pOH?
If the pOH of a solution is 4, what is the concentration of hydroxide ions ($OH^−$)?
If the pOH of a solution is 4, what is the concentration of hydroxide ions ($OH^−$)?
What is the pH of a solution containing a hydronium ion concentration ($[H_3O^+]$) of $1.0 imes 10^{−8} M$?
What is the pH of a solution containing a hydronium ion concentration ($[H_3O^+]$) of $1.0 imes 10^{−8} M$?
After water ($H_2O$) donates a proton, what is the resulting chemical species?
After water ($H_2O$) donates a proton, what is the resulting chemical species?
What chemical species is produced when a hydroxide ion ($OH^−$) accepts a proton?
What chemical species is produced when a hydroxide ion ($OH^−$) accepts a proton?
Which of the following ions has virtually no effect on the pH of a solution when dissolved in water?
Which of the following ions has virtually no effect on the pH of a solution when dissolved in water?
Which of the following hydroxide compounds releases two moles of hydroxide ions ($OH^−$) per mole of compound in solution?
Which of the following hydroxide compounds releases two moles of hydroxide ions ($OH^−$) per mole of compound in solution?
Which of the following hydroxide compounds exhibits very low solubility in water?
Which of the following hydroxide compounds exhibits very low solubility in water?
What is the chemical formula of the conjugate base of sulfuric acid ($H_2SO_4$)?
What is the chemical formula of the conjugate base of sulfuric acid ($H_2SO_4$)?
Which of the following salts is formed when a strong acid reacts with a strong base?
Which of the following salts is formed when a strong acid reacts with a strong base?
Which of the following bonds requires the highest amount of energy to break?
Which of the following bonds requires the highest amount of energy to break?
Which of the following anions is produced when a weak acid donates a proton?
Which of the following anions is produced when a weak acid donates a proton?
Which of the following cations is NOT a conjugate acid of a weak base?
Which of the following cations is NOT a conjugate acid of a weak base?
Which of the following cations is a conjugate acid capable of donating a proton?
Which of the following cations is a conjugate acid capable of donating a proton?
Based on bond enthalpy, which of the following acids is the weakest?
Based on bond enthalpy, which of the following acids is the weakest?
Flashcards
Salt solution acidity
Salt solution acidity
The relative strengths of the weak acid and weak base from which the salt is derived.
Salt solution with Kb > Ka
Salt solution with Kb > Ka
The solution is basic
Salt forming a neutral solution
Salt forming a neutral solution
NaCl
pH of 1.0 × 10-4 M H3O+
pH of 1.0 × 10-4 M H3O+
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pOH of 1.0 × 10-5 M OH-
pOH of 1.0 × 10-5 M OH-
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A strong acid
A strong acid
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Conjugate base of CH3COOH
Conjugate base of CH3COOH
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Conjugate acid of NH3
Conjugate acid of NH3
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Cation making a solution acidic
Cation making a solution acidic
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Anion making a solution basic
Anion making a solution basic
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Salt solution with Ka ≈ Kb
Salt solution with Ka ≈ Kb
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Bond enthalpy of H-I
Bond enthalpy of H-I
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A strong base (hydroxide)
A strong base (hydroxide)
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NaOH dissolves in water
NaOH dissolves in water
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Conjugate base of H2SO4
Conjugate base of H2SO4
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Cation not affecting pH
Cation not affecting pH
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Anion that does NOT affect the pH of a solution
Anion that does NOT affect the pH of a solution
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pH when pOH is 3.00
pH when pOH is 3.00
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NOT a strong acid
NOT a strong acid
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Cation: Conjugate acid of weak base
Cation: Conjugate acid of weak base
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Which anion is the conjugate base of a weak acid?
Which anion is the conjugate base of a weak acid?
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Cation: Conjugate acid of a weak base
Cation: Conjugate acid of a weak base
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Salt creating a basic solution
Salt creating a basic solution
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pH during acidic salt hydrolysis?
pH during acidic salt hydrolysis?
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Does not hydrolyze in water
Does not hydrolyze in water
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pH for [OH-] = 1.0 × 10−3 M
pH for [OH-] = 1.0 × 10−3 M
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Cation - Contributing to acidity
Cation - Contributing to acidity
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Producing neural solution
Producing neural solution
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Produces acidic solution
Produces acidic solution
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Produces basic solution
Produces basic solution
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pOH of pH 9
pOH of pH 9
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[OH-] at pOH is 4?
[OH-] at pOH is 4?
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pH of [H3O+] = 1.0 × 10−8 М
pH of [H3O+] = 1.0 × 10−8 М
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Conjugate base with H2O?
Conjugate base with H2O?
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Conjugate acid of OH- ?
Conjugate acid of OH- ?
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Ion with no affect of pH
Ion with no affect of pH
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The following moles of OH
The following moles of OH
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Insoluble in water hydroxide?
Insoluble in water hydroxide?
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Conjugate base for H2SO4?
Conjugate base for H2SO4?
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Has strength with acid/base?
Has strength with acid/base?
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Study Notes
Salt Solution Acidity
- A salt solution is acidic, basic, or neutral based on the relative strengths of the weak acid and base it is derived from
- If Kb > Ka, expected pH behavior is basic for the solution.
- NaCl is likely to form a neutral solution.
pH and pOH Calculations
- Solution with a H₃O⁺ concentration of 1.0 × 10⁻⁴ M has a pH of 4.00
- Solution with an OH⁻ concentration of 1.0 × 10⁻⁹ M has a pOH of 9.00
- If the pOH is 3.00, the pH of a solution is 11.00 (pH + pOH = 14)
Acids and Bases
- HCl is a strong acid
- CH₃COO⁻ is the conjugate base of CH₃COOH
- NH₄⁺ is the conjugate acid of NH₃
- NH₄⁺ cation will make a solution acidic
- CN⁻ anion will make a solution basic
- A salt solution with Ka ≈ Kb will have a neutral pH.
- H-I has a bond enthalpy of 298.3 kJ/mol per Table 16.9.
- LiOH is a strong base
- NaOH ionizes into Na⁺ and OH⁻ when dissolved in water
- HSO₄⁻ is the conjugate base of H₂SO₄
- Na⁺ cation does NOT affect the pH of a solution
- NO₃⁻ anion does NOT affect the pH of a solution
- If [H₃O⁺] = 1.0 × 10⁻⁸ M, the pH of a solution is 8.00
- Hydroxide ion concentration is 1.0 × 10⁻⁴ M if the pOH is 4
- Hydroxide producing two moles of OH⁻ per formula unit in solution is Ca(OH)₂
- Fe(OH)₃ is insoluble in water
- NaCl salt is derived from a strong acid and strong base
Other Key Facts
- If a solution has a hydroxide ion concentration of 1.0 × 10⁻³ M, the pH is 11.00
- NH₄⁺ cation contributes to the acidity of a solution
- NaCl will produce a neutral solution in water
- NH₄NO₃ will produce an acidic solution in water
- CH₃COONa will produce a basic solution in water
- H-F has the highest bond enthalpy
- CN⁻ anion is the conjugate base of a weak acid
- Na⁺ cation is NOT the conjugate acid of a weak base
- H₃O⁺ cation is a strong acid
- HF acid is the weakest based on bond enthalpy
- LiOH hydroxide is a Group 1 hydroxide
- Ca(OH)₂ hydroxide is a Group 2 hydroxide
- NH₄⁺ species is a conjugate acid of a weak base
- NH₄Cl salt results in an acidic solution when dissolved in water.
- NaCN salt results in a basic solution when dissolved in water
- NaCl is a neutral salt that does not hydrolyze
- NH₄Cl salt will create an acidic solution in water when dissolved
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