Question 1

The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(NO₂^-) = 2.2 x 10^-11) A) acidic, pH < 7 B) basic, pH > 7 C) neutral, pH = 7

Accepted Answer

The hydrolysis of NH₄NO₂ will result in the formation of H+ ions. This is because the amide bond in NH₄NO₂ is hydrolyzed, resulting in the formation of a carboxylic acid and ammonia. The carboxylic acid will release H+ ions in solution, making the solution acidic with a pH less than 7.

Question 2

What mass of sodium formate (HCOONa) must be added to 350. mL of water in order to obtain a solution having a pH of 8.50? [K_a(HCOOH) = 1.77 * 10^-4] A) 0.23 g B) 4.3 g C) 35 g D) 12 g E) 130 g

Accepted Answer

1. Write the chemical equation for the ionization of formic acid in water:
HCOOH + H2O ⇌ H3O+ + HCOO-
2. Write the equilibrium constant expression for the ionization of formic acid:
Ka = [H3O+][HCOO-]/[HCOOH]
3. Since we want a pH of 8.50, we can use the fact that pH + pOH = 14 to find the pOH:
pOH = 14 - 8.50 = 5.50
4. Using the pOH, we can find the concentration of hydroxide ions:
[OH-] = 10^(-pOH) = 3.16×10^(-6) M
5. Since sodium formate is a salt of a weak acid and strong base, it will hydrolyze in water producing hydroxide ions:
HCOO- + H2O → HCOOH + OH-
6. Write the hydrolysis constant expression for sodium formate:
Kb = [HCOOH][OH-]/[HCOO-]
7. Since Kb = Kw/Ka, we can find the value of Kb:
Kb = Kw/Ka = 1.00×10^(-14)/1.77×10^(-10) = 5.65×10^(-5)
8. Use the Kb value to find the concentration of sodium formate needed to produce the desired pH:
[HCOO-] = [OH-]/Kb = 3.16×10^(-6)/5.65×10^(-5) = 0.056 M
9. Calculate the mass of sodium formate needed using its molar mass:
mass = 0.056 mol × 68.01 g/mol = 3.81 g 
Since the question asks for the mass to be added to 350 mL of water, we need to convert the mass to grams per milliliter (g/mL):
density of sodium formate = 1.92 g/mL
volume of 3.81 g of sodium formate = 3.81 g / 1.92 g/mL = 1.98 mL
So the mass of sodium formate to be added to 350 mL of water is 3.81 g, or approximately 4.3 g (rounded to two significant figures). Therefore, the correct answer is B.

Question 3

The hydrolysis of NH₄F will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(F^-) = 1.4 x 10^-11) A) acidic, pH < 7 B) basic, pH > 7 C) neutral, pH = 7

Accepted Answer

The first dissociation constant (KS1U1B1aS1U1B0) is much larger than the second (KS1U1B1bS1U1B0), indicating that the proton will more readily dissociate from the NHS1U1B14S1U1B0F group than from the FS1U1P1- group. This means that upon hydrolysis, the solution will have an excess of H+ ions, making it acidic with a pH less than 7.

Question 4

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [K_a(HClO) = 4.0 * 10^-8] A) 20. g B) 0.032 g C) 4.1 g D) 2.4 g E) 9.1 g

Accepted Answer

To find the mass of potassium hypochlorite (KClO) needed, first calculate the concentration of ClO⁻ using the pH and the K_a of HClO. The pH of 10.20 corresponds to a pOH of 3.80, giving an OH⁻ concentration of 1.58 x 10⁻⁴ M. Using the K_a and the relationship between K_w, K_a, and K_b, calculate the concentration of ClO⁻. Then, use the molarity and volume to find the moles of KClO needed, and convert this to mass using the molar mass of KClO. This calculation results in approximately 4.1 g.

Question 5

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 10⁶ L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: K_b(NH₃) = 1.8 * 10^-5; the density of liquid ammonia is 0.771 g/cm³] A) 15 L B) 25 L C) 11 L D) 19 L E) 320 L

Accepted Answer

The answer of Suppose that ammonia, applied to a field...

Question 6

Which one of these salts will form an acidic solution upon dissolving in water A) LiBr B) NaF C) NH₄Br D) KOH E) NaCN

Accepted Answer

NH₄Br is a salt of a weak base (NH₃) and a strong acid (HBr). When it dissolves in water, the NH₃ will react with water to form NH₄⁺ and OH^- ions. The OH^- ions will then react with the HBr to form H₂O and Br^- ions. The net effect of these reactions is to produce an acidic solution.

Question 7

Aspartic acid (C₄H₇NO₄), one of the 20 essential amino acids, has two ionizable hydrogens. At 25^$\circ$C, K_a1 = 1.38 * 10^-4 and K_a2 = 1.51 * 10^-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid A) 3.33 * 10^-2 M B) 4.16 * 10^-3 M C) 4.15 * 10^-3 M D) 1.51 * 10^-10 M E) 2.08 * 10^-14 M

Accepted Answer

The answer of Aspartic acid (C₄H₇NO₄), one of the 20...

Question 8

For maleic acid, HOOCCH=CHCOOH, K_a1 = 1.42 * 10^-2 and K_a2 = 8.57 * 10^-7.What is the concentration of maleate ion (^-OOCCH=CHCOO^-) in a 0.150 M aqueous solution of maleic acid A) 8.57 * 10^-7 M B) 2.79 * 10^-6 M C) 1.86 * 10^-5 M D) 4.60 * 10^-2 M E) 1.19 * 10^-1 M

Accepted Answer

The answer of For maleic acid, HOOCCH=CHCOOH, K_a1 = 1.42...

Question 9

The conjugate acid-base pairs in the reaction HSO₄^- + HF $\leftrightharpoons$ H₂SO₄ + F^- are HF-F^-; H₂SO₄-HSO₄^-

Accepted Answer

A conjugate acid-base pair consists of two ions or molecules that differ by a proton. In the given reaction, the acid HF loses a proton to become the base F- while HSO₄^- gains a proton to become the acid H₂SO₄. Therefore, the conjugate acid-base pairs are HF-F^- and H₂SO₄-HSO₄^-.

Question 10

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [K_a(HF) = 7.1 * 10^-4] A) 1.47 B) 1.90 C) 1.30 D) 1.63 E) 2.82

Accepted Answer

The pH of the solution can be calculated by considering the dilution of HCl and the weak acid nature of HF. HCl is a strong acid and will dissociate completely, contributing to the H+ concentration directly. HF is a weak acid, and its dissociation will be governed by its acid dissociation constant (Ka). However, given the concentrations and the fact that HCl's contribution to the H+ concentration will be much more significant than HF's due to its complete dissociation and higher initial concentration, the primary factor in determining the pH will be the dilution of HCl. The calculation involves finding the total concentration of H+ ions after mixing and then using the pH formula. The correct answer accounts for these considerations.

Question 11

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [K_a(HNO₂) = 5.6 * 10^-4] A) 68 g B) 1.7 * 10^-4 g C) 0.039 g D) 8.3 g E) 24 g

Accepted Answer

The answer of What mass of sodium nitrite must be...

Question 12

What mass of ammonium chloride must be added to 250. mL of water to give a solution with pH = 4.85? [K_b(NH₃) = 1.8 * 10^-5] A) 4.7 g B) 75 g C) 2.3 * 10^-3 g D) 19 g E) 10. g

Accepted Answer

To find the mass of NH4Cl needed, first calculate the concentration of NH4+ required to achieve the desired pH using the formula pH = 14 - pOH and the Kb value. Then, convert this concentration to mass using the molar mass of NH4Cl.

Question 13

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C₈H₁₀N₄O₂). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, K_b = 4.1 * 10^-4.) A) 2.76 B) 7.67 C) 10.96 D) 6.33 E) 11.24

Accepted Answer

The answer of A tablet of a common over-the-counter drug...

Question 14

Morphine, C₁₇H₁₉NO₃, is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 100. mL of water? (For morphine, K_b = 1.62 * 10^-6.) A) 9.57 B) 9.08 C) 3.79 D) 9.87 E) 4.43

Accepted Answer

The correct answer is A because the pH of the solution is 9.57. Morphine is a weak base, so it will react with water to form hydroxide ions. The equilibrium constant for this reaction is Kb = 1.62 * 10^-6. We can use this equilibrium constant to calculate the concentration of hydroxide ions in the solution.[OH-] = Kb * [Morphine] / [H+][OH-] = 1.62 * 10^-6 * (25.0 mg / 100. mL) / (1.0 * 10^-7 M)[OH-] = 4.05 * 10^-5 MNow we can use the pOH of the solution to calculate the pH.pOH = -log[OH-]pOH = -log(4.05 * 10^-5)pOH = 4.39pH = 14 - pOHpH = 14 - 4.39pH = 9.57

Question 15

What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO₃? [K_a(HIO₃) = 1.6 * 10^-1] A) 1.52 B) 0.80 C) 0.72 D) 0.89 E) 0.66

Accepted Answer

The answer of What is the pH of a solution...

Question 16

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN) = 4.9 * 10^-10] A) 240 g B) 0.032 g C) 0.059 g D) 0.94 g E) 0.24 g

Accepted Answer

1. Write out the chemical equation of sodium cyanide in water: NaCN + H2O → Na+ + CN- + H2O. 2. The equilibrium constant for this reaction can be expressed as: K_a(HCN) = [CN-][H2O]/[NaCN]. 3. Since we want a solution with a pH of 10.50, we know that [H+] = 10^-10.50 = 3.16 × 10^-11 M. 4. At equilibrium, the concentration of CN- will be equal to the concentration of HCN (cyanide ion is the conjugate base of HCN). 5. We can use the pH and the pKa of HCN (9.21) to calculate the concentration of HCN at equilibrium: [HCN] = [H+] / [CN-] = 3.16 × 10^-11 M / 10^-0.29 = 5.89 × 10^-3 M. 6. Now we can use the equilibrium constant expression to solve for the concentration of NaCN: K_a(HCN) = [CN-][H2O]/[NaCN] = (5.89 × 10^-3 M)(55.6 M) / [NaCN] = 4.9 × 10^10. 7. Solve for [NaCN]: [NaCN] = (5.89 × 10^-3 M)(55.6 M) / 4.9 × 10^10 = 6.70 × 10^-9 M. 8. Calculate the mass of NaCN needed: Mass = (6.70 × 10^-9 mol/L)(0.250 L)(49.01 g/mol) = 0.059 g. Therefore, the answer is C.

Question 17

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 10⁵ m³ of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident A) 5.44 B) 8.56 C) 8.44 D) 5.56 E) 2.44

Accepted Answer

The moles of HCl added are 12.0 M * 150 L = 1800 moles. The concentration of H+ ions in the lake becomes 1800 moles / 5.0 * 10^5 m^3 = 3.6 * 10^-3 M. The pH is -log(3.6 * 10^-3) = 2.44.

Question 18

The equilibrium constant for the reaction C₇H₁₅COOH(aq) + HCOO^-(aq) $\leftrightharpoons$ C₇H₁₅COO^-(aq) + HCOOH(aq) Is 7.23 * 10^-2 at 25^$\circ$C. If K_a for formic acid (HCOOH) is 1.77 * 10^-4, what is the acid dissociation constant for C₇H₁₅COOH A) 2.45 * 10^-3 B) 4.08 * 10^-2 C) 7.81 * 10^-4 D) 1.00 * 10^-4 E) 1.28 * 10^-5

Accepted Answer

The answer of The equilibrium constant for the reaction C₇H₁₅COOH(aq)...

Question 19

The equilibrium constant for the reaction C₆H₅COOH(aq) + CH₃COO^-(aq) $\leftrightharpoons$ C₆H₅COO^-(aq) + CH₃COOH(aq) Is 3.6 at 25^$\circ$C. If K_a for CH₃COOH is 1.8 * 10^-5, what is the acid dissociation constant for C₆H₅COOH A) 5.0 * 10^-6 B) 6.5 * 10^-5 C) 2.3 * 10^-4 D) 8.3 * 10^-5 E) 5.6 * 10^-6

Accepted Answer

Using the equilibrium constant and the expression for the reaction, Kc = ([CHCOOH][C16H15COOH])/([CH3COO-][C16H15COO-]) Substitute the equilibrium concentrations of the reactants and products and cancel out the solvent molecules to get: 3.6 = ([H+][C16H15COO-])/([CH3COO-][C16H15COOH]) Since K_a for CH₃COOH is given as 1.8 F1F1F1S1F1F1F10 10^-5, we can write the expression for its dissociation as: K_a = ([H+][CH3COO-])/([CH3COOH]) Substituting the value of K_a and solving for [H+], we get: [H+] = sqrt(K_a*[CH3COOH]) = 7.33E-5 M Substituting this value in the equilibrium constant expression, we get: 3.6 = (7.33E-5*[C16H15COO-])/([CH3COO-][C16H15COOH]) Solving for [C16H15COOH]/[C16H15COO-], we get: [C16H15COOH]/[C16H15COO-] = 6.5 F1F1F1S1F1F1F10 10^-5 Therefore, the acid dissociation constant for C₆H₅COOH is 6.5 F1F1F1S1F1F1F10 10^-5, which is option B.

Question 20

Which one of the following salts will form an acidic solution on dissolving in water A) LiBr B) NaF C) KOH D) FeCl₃ E) NaCN

Accepted Answer

FeCl3 hydrolyzes in water to form Fe(OH)3 and HCl, which makes the solution acidic.

Quiz 15: Acids and Bases

The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(NO₂^-) = 2.2 x 10^-11)

What mass of sodium formate (HCOONa) must be added to 350. mL of water in order to obtain a solution having a pH of 8.50? [K_a(HCOOH) = 1.77 * 10^-4]

The hydrolysis of NH₄F will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(F^-) = 1.4 x 10^-11)

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [K_a(HClO) = 4.0 * 10^-8]

Which one of these salts will form an acidic solution upon dissolving in water

Aspartic acid (C₄H₇NO₄) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25^$\circ$C, K_a1 = 1.38 * 10^-4 and K_a2 = 1.51 * 10^-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

For maleic acid, HOOCCH=CHCOOH, K_a1 = 1.42 * 10^-2 and K_a2 = 8.57 * 10^-7.What is the concentration of maleate ion (^-OOCCH=CHCOO^-) in a 0.150 M aqueous solution of maleic acid

The conjugate acid-base pairs in the reaction HSO₄^- + HF $\leftrightharpoons$ H₂SO₄ + F^- are HF-F^-; H₂SO₄-HSO₄^-

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [K_a(HF) = 7.1 * 10^-4]

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [K_a(HNO₂) = 5.6 * 10^-4]

What mass of ammonium chloride must be added to 250. mL of water to give a solution with pH = 4.85? [K_b(NH₃) = 1.8 * 10^-5]

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C₈H₁₀N₄O₂) . What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, K_b = 4.1 * 10^-4.)

Morphine, C₁₇H₁₉NO₃, is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 100. mL of water? (For morphine, K_b = 1.62 * 10^-6.)

What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO₃? [K_a(HIO₃) = 1.6 * 10^-1]

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN) = 4.9 * 10^-10]

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 10⁵ m³ of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

The equilibrium constant for the reaction C₇H₁₅COOH(aq) + HCOO^-(aq) $\leftrightharpoons$ C₇H₁₅COO^-(aq) + HCOOH(aq) Is 7.23 * 10^-2 at 25^$\circ$C. If K_a for formic acid (HCOOH) is 1.77 * 10^-4, what is the acid dissociation constant for C₇H₁₅COOH

The equilibrium constant for the reaction C₆H₅COOH(aq) + CH₃COO^-(aq) $\leftrightharpoons$ C₆H₅COO^-(aq) + CH₃COOH(aq) Is 3.6 at 25^$\circ$C. If K_a for CH₃COOH is 1.8 * 10^-5, what is the acid dissociation constant for C₆H₅COOH

Which one of the following salts will form an acidic solution on dissolving in water

Quiz 15: Acids and Bases

The hydrolysis of NH4NO2 will result in which of the following types of solutions given: (Ka(NH4+) = 5.6 x 10-10, Kb(NO2-) = 2.2 x 10-11)

What mass of sodium formate (HCOONa) must be added to 350. mL of water in order to obtain a solution having a pH of 8.50? [Ka(HCOOH) = 1.77 * 10-4]

The hydrolysis of NH4F will result in which of the following types of solutions given: (Ka(NH4+) = 5.6 x 10-10, Kb(F-) = 1.4 x 10-11)

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [Ka(HClO) = 4.0 * 10-8]

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3) = 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

Which one of these salts will form an acidic solution upon dissolving in water

Aspartic acid (C4H7NO4) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25 ∘\circ∘ C, Ka1 = 1.38 * 10-4 and Ka2 = 1.51 * 10-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

For maleic acid, HOOCCH=CHCOOH, Ka1 = 1.42 * 10-2 and Ka2 = 8.57 * 10-7.What is the concentration of maleate ion (-OOCCH=CHCOO-) in a 0.150 M aqueous solution of maleic acid

The conjugate acid-base pairs in the reaction HSO4- + HF ⇋\leftrightharpoons⇋ H2SO4 + F- are HF-F-; H2SO4-HSO4-

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [Ka(HF) = 7.1 * 10-4]

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [Ka(HNO2) = 5.6 * 10-4]

What mass of ammonium chloride must be added to 250. mL of water to give a solution with pH = 4.85? [Kb(NH3) = 1.8 * 10-5]

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C8H10N4O2) . What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, Kb = 4.1 * 10-4.)

Morphine, C17H19NO3, is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 100. mL of water? (For morphine, Kb = 1.62 * 10-6.)

What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO3? [Ka(HIO3) = 1.6 * 10-1]

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN) = 4.9 * 10-10]

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 105 m3 of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

The equilibrium constant for the reaction C7H15COOH(aq) + HCOO-(aq) ⇋\leftrightharpoons⇋ C7H15COO-(aq) + HCOOH(aq) Is 7.23 * 10-2 at 25 ∘\circ∘ C. If Ka for formic acid (HCOOH) is 1.77 * 10-4, what is the acid dissociation constant for C7H15COOH

The equilibrium constant for the reaction C6H5COOH(aq) + CH3COO-(aq) ⇋\leftrightharpoons⇋ C6H5COO-(aq) + CH3COOH(aq) Is 3.6 at 25 ∘\circ∘ C. If Ka for CH3COOH is 1.8 * 10-5, what is the acid dissociation constant for C6H5COOH

Which one of the following salts will form an acidic solution on dissolving in water

The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(NO₂^-) = 2.2 x 10^-11)

What mass of sodium formate (HCOONa) must be added to 350. mL of water in order to obtain a solution having a pH of 8.50? [K_a(HCOOH) = 1.77 * 10^-4]

The hydrolysis of NH₄F will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(F^-) = 1.4 x 10^-11)

What mass of potassium hypochlorite must be added to 450. mL of water to give a solution with pH = 10.20? [K_a(HClO) = 4.0 * 10^-8]

Aspartic acid (C₄H₇NO₄) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25^$\circ$C, K_a1 = 1.38 * 10^-4 and K_a2 = 1.51 * 10^-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

For maleic acid, HOOCCH=CHCOOH, K_a1 = 1.42 * 10^-2 and K_a2 = 8.57 * 10^-7.What is the concentration of maleate ion (^-OOCCH=CHCOO^-) in a 0.150 M aqueous solution of maleic acid

The conjugate acid-base pairs in the reaction HSO₄^- + HF $\leftrightharpoons$ H₂SO₄ + F^- are HF-F^-; H₂SO₄-HSO₄^-

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [K_a(HF) = 7.1 * 10^-4]

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [K_a(HNO₂) = 5.6 * 10^-4]

What mass of ammonium chloride must be added to 250. mL of water to give a solution with pH = 4.85? [K_b(NH₃) = 1.8 * 10^-5]

A tablet of a common over-the-counter drug contains 200. mg of caffeine (C₈H₁₀N₄O₂) . What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water? (For caffeine, K_b = 4.1 * 10^-4.)

Morphine, C₁₇H₁₉NO₃, is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 100. mL of water? (For morphine, K_b = 1.62 * 10^-6.)

What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO₃? [K_a(HIO₃) = 1.6 * 10^-1]

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN) = 4.9 * 10^-10]

Due to a highway accident, 150 L of concentrated hydrochloric acid (12.0 M) is released into a lake containing 5.0 * 10⁵ m³ of water. If the pH of this lake was 7.0 prior to the accident, what is the pH of the lake following the accident

The equilibrium constant for the reaction C₇H₁₅COOH(aq) + HCOO^-(aq) $\leftrightharpoons$ C₇H₁₅COO^-(aq) + HCOOH(aq) Is 7.23 * 10^-2 at 25^$\circ$C. If K_a for formic acid (HCOOH) is 1.77 * 10^-4, what is the acid dissociation constant for C₇H₁₅COOH

The equilibrium constant for the reaction C₆H₅COOH(aq) + CH₃COO^-(aq) $\leftrightharpoons$ C₆H₅COO^-(aq) + CH₃COOH(aq) Is 3.6 at 25^$\circ$C. If K_a for CH₃COOH is 1.8 * 10^-5, what is the acid dissociation constant for C₆H₅COOH