1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write...
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write the neutralization reaction for HF and KOH. What is the value of Kn (equilibrium constant for neutralization)? (Ka(HF)=3.5*10^-4). If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic, or neutral?
Answer: Kn= 3.5*10^10; neutralization reaction is 100% complete since Kn is so large; pH > 7 at equivalence.
Just need this explained please :)
Homework Answers
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1) When a weak acid is neutralized by a strong base, is the
neutralization complete? Write...
HF is a weak acid (a monoprotic one). When HF is titrated with a strong base...
HF is a weak acid (a monoprotic one). When HF is titrated with a strong base (like NaOH), it will eventually reach an equivalence point where exactly all of the HF has been reacted with exactly the needed amount of NaOH. What will the pH be when HF reaches equivalence point? (Hint: think about what products will be present and whether they are weak acids, weak bases or neutral...) pH will be 7.0 pH will be greater than 7.0 pH...
2. In the neutralization of 50.0 mL of 0.1 M HA (a weak acid with Ka-1.8x10-4)...
2. In the neutralization of 50.0 mL of 0.1 M HA (a weak acid with Ka-1.8x10-4) with 0.10 M KOH (a strong base), the most correct description of the solution at half way the equivalence point (i.e., half neutralized), is
dilu SLUHY Udses, velduse ule ujuydte udbe vid Struny dulu is too weak to establish any...
dilu SLUHY Udses, velduse ule ujuydte udbe vid Struny dulu is too weak to establish any meaningful equilibrium in solution. Figure 2: After Neutralization, F. Re-establishes an Equilibrium. Free Free Conclusions 1. The initial reaction between a weak acid and a strong base is not an equilibrium. Each mole of base deprotonates one mole of acid in an "irreversible" (very large K value) reaction. 2. Neutralization of a weak acid with strong base produces a conjugate base that will react...
Consider the titration of a weak acid with a strong base. Which statement below is true...
Consider the titration of a weak acid with a strong base. Which statement below is true regarding the equivalence point in this titration? It occurs at a pH less than 7.0 because an acidic salt is formed. h It occurs at a pH greater than 7.0 because an acidic salt is formed. It occurs at a pH 7.0 because the acid has been neutralized It occurs at a pH greater than 7.0 because a basic salt is formed e It...
Consider the titration of a weak acid with a strong base. Which statement below is true...
Consider the titration of a weak acid with a strong base. Which statement below is true regarding the equivalence point in this titration? It occurs at a pH less than 7.0 because a basic salt is formed. O It occurs at a pH greater than 7.0 because an acidic salt is formed. O It occurs at a pH = 7.0 because the acid has been neutralized. O It occurs at a pH less than 7.0 because an acidic salt is...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA,...
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA, with a Ka value of 5.61 x 10 Constants Periodic Table A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH (aq) +...
Explain why the neutralization reaction of a strong acid and a weak base gives a weakly...
Explain why the neutralization reaction of a strong acid and a weak base gives a weakly acidic solution.
A weak acid is titrated with a strong base and the pH vs. volume plot is...
A weak acid is titrated with a strong base and the pH vs. volume plot is shown. Approximately what is denoted with B)? A) The equilibrium of the acid B) The starting pH C) The equivalence point D) The end point E) The pKa of the weak acid D) pH B) A) Volume titrant added O E OB OA Ос OD о Bi E A weak acid is titrated with a strong base and the pH vs. volume plot is...
This reaction is classified as: Strong Acid + Strong Base, Weak Acid + Strong Base, Strong Acid + Weak Base, Weak Aci...
This reaction is classified as: Strong Acid + Strong Base, Weak
Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak
Base.
The extent of this reaction is: Below 50%, 50%, Above 50%,
100%
When 35.0 mL of 0.300 M
perchloric acid and 35.0 mL of
0.150 M barium hypochlorite are
combined, the pH of the resulting solution will be greater than,
equal to, less than seven.
Write the balanced NET IONIC equation for the reaction that...
2. In the neutralization of 50.0 mL of 0.1 M HA (a weak acid with Ka-1.8x10-4) with 0.10 M KOH (a strong base), the most correct description of the solution at half way the equivalence point (i.e., half neutralized), is
dilu SLUHY Udses, velduse ule ujuydte udbe vid Struny dulu is too weak to establish any meaningful equilibrium in solution. Figure 2: After Neutralization, F. Re-establishes an Equilibrium. Free Free Conclusions 1. The initial reaction between a weak acid and a strong base is not an equilibrium. Each mole of base deprotonates one mole of acid in an "irreversible" (very large K value) reaction. 2. Neutralization of a weak acid with strong base produces a conjugate base that will react...
Consider the titration of a weak acid with a strong base. Which statement below is true regarding the equivalence point in this titration? It occurs at a pH less than 7.0 because an acidic salt is formed. h It occurs at a pH greater than 7.0 because an acidic salt is formed. It occurs at a pH 7.0 because the acid has been neutralized It occurs at a pH greater than 7.0 because a basic salt is formed e It...
Consider the titration of a weak acid with a strong base. Which statement below is true regarding the equivalence point in this titration? It occurs at a pH less than 7.0 because a basic salt is formed. O It occurs at a pH greater than 7.0 because an acidic salt is formed. O It occurs at a pH = 7.0 because the acid has been neutralized. O It occurs at a pH less than 7.0 because an acidic salt is...
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA, with a Ka value of 5.61 x 10 Constants Periodic Table A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH (aq) +...
A weak acid is titrated with a strong base and the pH vs. volume plot is shown. Approximately what is denoted with B)? A) The equilibrium of the acid B) The starting pH C) The equivalence point D) The end point E) The pKa of the weak acid D) pH B) A) Volume titrant added O E OB OA Ос OD о Bi E A weak acid is titrated with a strong base and the pH vs. volume plot is...
This reaction is classified as: Strong Acid + Strong Base, Weak
Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak
Base.
The extent of this reaction is: Below 50%, 50%, Above 50%,
100%
When 35.0 mL of 0.300 M
perchloric acid and 35.0 mL of
0.150 M barium hypochlorite are
combined, the pH of the resulting solution will be greater than,
equal to, less than seven.
Write the balanced NET IONIC equation for the reaction that...
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