Weak Acid-Base Equilibria: 동영상 및 연습문제

Which of the following statements correctly defines a weak acid?

What is the correct equilibrium expression for the dissociation of a weak acid HA in water?

If the pH of a solution is 3.5, what is the concentration of hydronium ions, [H₃O⁺]?

Given a weak acid HA with an initial concentration of 0.1 M and a K_a of 1.8 x 10^-5, use an ICE chart to find the equilibrium concentration of H₃O⁺.

For a weak acid HA with an initial concentration of 0.2 M and a K_a of 4.0 x 10^-6, derive the equilibrium concentration of HA.

A weak acid solution has a pH of 4.5 and a K_a of 3.2 x 10^-5. What is the formal concentration of the weak acid?

For a weak acid HA with K_a = 1.5 x 10^-4 and [H₃O⁺] = 1.0 x 10^-3 M, what is the concentration of A^- at equilibrium?

Why is water not included in the equilibrium expression for the dissociation of a weak acid?

In solving for the original concentration of a weak acid, why is it important to isolate the variable representing the formal concentration?

Which of the following is the correct equilibrium expression for the dissociation of acetic acid (CH₃COOH) in water?

If the pH of a solution is 2.8, what is the concentration of hydronium ions, [H₃O⁺]?

Given a weak acid HA with an initial concentration of 0.05 M and a K_a of 2.5 x 10^-5, use an ICE chart to find the equilibrium concentration of A^-.

For a weak acid HA with an initial concentration of 0.15 M and a K_a of 3.0 x 10^-6, derive the equilibrium concentration of HA.

For a weak acid HA with K_a = 2.0 x 10^-4 and [H₃O⁺] = 2.0 x 10^-3 M, what is the concentration of A^- at equilibrium?

In the equilibrium expression for the dissociation of a weak acid, why is water not included?

Why is isolating the variable representing the formal concentration crucial in solving equilibrium problems for weak acids?

What is the correct equilibrium expression for the dissociation of formic acid (HCOOH) in water?

Two monoprotic acids have $K_{a1}=3.2\times {10}^{-6}$ and $K_{a2}=8.0\times {10}^{-4}$. By what factor is acid 2 larger in $K_a$ than acid 1? Give the answer to 2 significant figures.

A monoprotic weak acid has formal concentration $0.150$ and $K_a=4.0\times {10}^{-5}$. Solve the equilibrium expression exactly and determine the pH of the solution at 25°C. Give the answer to 2 decimal places.

A $0.150M$ solution of a monoprotic weak acid $HA$ has $K_a=6.3\times {10}^{-5}$. Determine the pH of the solution. Round to 2 decimal places.

A $0.220M$ solution of weak base $B$ has $K_b=2.5\times {10}^{-6}$. Determine the pOH of the solution. Round to 2 decimal places.

A weak acid solution is prepared with initial concentration $0.0800M$. At equilibrium, the hydronium concentration is $1.6\times {10}^{-3}M$. Calculate the percent dissociation of the acid. Round to 2 decimal places.

A $0.300M$ solution contains a weak base whose conjugate acid has $K_a=4.0\times {10}^{-10}$ at 25 °C. Determine the pH of the base solution. Round to 2 decimal places.

Calculate the initial pH of a $0.220\text{ M pyridine}$ solution at ${25}^{\circ }C$ if $K_b=1.7\times {10}^{-9}$. Give your answer to 2 decimal places.

A monoprotic acid has $K_a=6.3\times {10}^{-6}$. At what pH are the fractions of $HA$ and $A^{-}$ equal? Give the answer to 2 decimal places.

A monoprotic acid has $p{K}_a=7.25$. At what pH will the solution contain $90.0\%A^{-}$? Give the answer to 2 decimal places.

A monoprotic weak acid solution has formal concentration $0.500$ and $p{K}_a=4.30$. If the equilibrium concentration of $HA$ is $0.100$, calculate the pH. Give the answer to 2 decimal places.