Acid-Base Equilibrium and pH

What is the pH of a solution with a hydrogen ion concentration of $1 \times 10^{-5}$ M?

Which of the following is a characteristic of a strong acid in an aqueous solution?

What is the primary function of a buffer solution?

What is the equivalence point in an acid-base titration?

According to Le Chatelier's Principle, what happens to a system at equilibrium when the concentration of a reactant is increased?

Which of the following defines an Arrhenius acid?

In a conjugate acid-base pair, what is the relationship between the acid and the base?

What does a low value of Ka indicate about the strength of an acid?

Which of the following describes a polyprotic acid?

Given the equilibrium reaction: $HA \rightleftharpoons H^+ + A^-$, if the pH of the solution is equal to the pKa of the acid, what is the ratio of $[A^-]$ to $[HA]$?

Which of the following statements is true regarding the pH of a strong acid solution compared to a weak acid solution of the same concentration?

What components are typically present in a buffer solution?

What is the purpose of an indicator in an acid-base titration?

How does increasing the temperature affect the equilibrium of an endothermic acid-base reaction?

Which of the following is a Bronsted base?

In the following reaction, $NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-$, identify the conjugate acid of $NH_3$.

If the pH of a weak acid solution is 4.0 and its concentration is 0.1 M, what additional information is needed to calculate the Ka of the acid?

Which of the following is an example of a binary acid?

A solution of a weak acid, HA, has a pH of 3.5. If the initial concentration of HA is 0.20 M, what is the approximate value of the acid dissociation constant, Ka?

Which buffer system would be most appropriate for maintaining a pH of 9.0?

During the titration of a weak base with a strong acid, at what point is the pH equal to the pKa of the conjugate acid?

Consider the equilibrium: $2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)$. Given that the forward reaction is endothermic, what effect will increasing the temperature have on the pH of pure water?

Which of the following is an example of an oxyacid?

Consider a buffer solution made of benzoic acid ($C_6H_5COOH$, Ka = $6.3 \times 10^{-5}$) and its conjugate base, benzoate ($C_6H_5COO^−$). If the concentration of benzoic acid is 0.20 M and the concentration of benzoate is 0.25 M, what is the pH of the buffer solution?

Calculate the pH of a 0.020 M solution of hydrofluoric acid (HF), given that its Ka is $6.8 \times 10^{-4}$.

What is the main reason that strong acids have lower pH's than weak acids, assuming equal molar concentrations?

How many endpoints will be observed in the titration of a solution of carbonic acid ($H_2CO_3$) with a solution of sodium hydroxide ($NaOH$)?

Which of the following is true about Kw, the ion product of water?

A researcher adds a small amount of hydrochloric acid (HCl) to a buffer solution containing acetic acid ($CH_3COOH$) and sodium acetate ($CH_3COONa$). How does the buffer system respond to maintain a stable pH?

Consider the titration of a weak monoprotic acid with a strong base. Which of the following statements accurately describes the pH at the equivalence point?

Which of the following changes will shift the equilibrium of the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ + heat to favor the formation of ammonia ($NH_3$)?

Identify the conjugate base of sulfuric acid ($H_2SO_4$).

If the pH of a solution of acetic acid ($CH_3COOH$) is 2.87, and the pKa of acetic acid is 4.76, what is the ratio of [acetate, $CH_3COO^−$] to [acetic acid, $CH_3COOH$]?

Ascorbic acid ($H_2C_6H_6O_6$) is a diprotic acid with $K_{a1} = 7.9 \times 10^{-5}$ and $K_{a2} = 1.6 \times 10^{-12}$. What is the pH of a 0.10 M solution of ascorbic acid, considering only the first dissociation?

You have a solution of 0.1 M acetic acid ($CH_3COOH$, $K_a = 1.8 \times 10^{-5}$). What concentration of sodium acetate ($CH_3COONa$) must be added to create a buffer with a pH of 5.0?

A chemist prepares a buffer solution by mixing 25.0 mL of 0.200 M $NH_3$ with 25.0 mL of 0.250 M $NH_4Cl$. What is the pH of the resulting buffer? (The $pK_b$ of $NH_3$ is 4.75)

What is the pH at which $Mg(OH)2$ precipitates from a solution with a $Mg^{2+}$ concentration of $1.0 \times 10^{-3}$ M? ($K{sp} = 5.6 \times 10^{-12}$)