Question 1

A 25.0 mL sample of 0.150 mol L^-1 aqueous butanoic acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10^-5.

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Question 2

What is the pH of an aqueous buffer solution that is 0.211 mol L^-1 in lactic acid and 0.111 mol L^-1 in sodium lactate? The Of lactic acid is 1.4 × .

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Question 3

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

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Question 4

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

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Question 5

How many millilitres of 0.120 mol L^-1 NaOH(aq)are required to titrate 50.0 mL of 0.0998 mol L^-1 aqueous butanoic acid to the equivalence point? Butanoic acid is monoprotic.The Of butanoic acid is 1.5 × 10^-5.

Accepted Answer

First, we need to determine how many moles of butanoic acid are present in 50.0 mL of 0.0998 mol/L solution:

0.0500 L x 0.0998 mol/L = 0.00499 mol butanoic acid

Since butanoic acid is monoprotic, it will react with one mole of NaOH according to the balanced equation:

CH3CH2CH2COOH + NaOH → CH3CH2CH2COO- Na+ + H2O

Thus, we need 0.00499 mol of NaOH to react completely with the butanoic acid. To calculate the volume of 0.120 mol/L NaOH required, we can use the following formula:

Volume (L) = moles / concentration (mol/L)

Volume = 0.00499 mol / 0.120 mol/L = 0.0416 L = 41.6 mL

Therefore, the answer is C: 41.6.

Question 6

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L^-¹ HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

The reaction between HCl and KOH is a neutralization reaction, where HCl (a strong acid) reacts with KOH (a strong base) to form water and KCl (a salt). The moles of HCl are 25.00 mL * 0.100 mol/L = 2.5 mmol, and the moles of KOH are 40.00 mL * 0.100 mol/L = 4.0 mmol. Since KOH is in excess by 1.5 mmol (4.0 mmol - 2.5 mmol), the solution will be basic. The concentration of excess OH- is 1.5 mmol / (25.00 mL + 40.00 mL) = 1.5 mmol / 65.00 mL = 0.0231 mol/L. The pOH is -log(0.0231) ≈ 1.64, and since pH + pOH = 14, the pH is 14 - 1.64 = 12.36.

Question 7

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

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Question 8

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

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Question 9

What is the pH of a buffer solution that is 0.255 mol L^-1 in hypochlorous acid (HClO)and 0.333 mol L^-1 in sodium hypochlorite (NaClO)? The Of hypochlorous acid is 3.8 × .

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Question 10

A 25.0 mL sample of 0.150 mol L^-1 aqueous hypochlorous acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10^-8.

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Question 11

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is

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Question 12

Calculate the pH of an aqueous solution that is 0.295 mol L^-1 in sodium formate (HCOONa)and In formic acid (HCOOH).The Of formic acid is 1.77 × .

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Question 13

How many millilitres of 0.0850 mol L^-1 NaOH(aq)are required to titrate 25.0 mL of (aq)to the equivalence point?

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Question 14

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 methylamine,CH₃NH₂,with 20.00 mL of 0.10 mol L^-1 methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

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Question 15

A 25.0 mL sample of 0.150 mol L^-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH(aq)solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10^-4.

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Question 16

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is

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Question 17

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

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Question 18

Calculate the pH of an aqueous solution that is 0.210 mol L^-1 in nitrous acid ( ) and 0.290 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is 4.50 × .

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Question 19

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

Accepted Answer

The Henderson-Hasselbalch equation can be used to calculate the ratio of [CH3COO-]/[CH3COOH] necessary to make an aqueous buffer solution with a pH of 4.34. The equation is:pH = pKa + log([CH3COO-]/[CH3COOH])where pKa is the negative logarithm of the acid dissociation constant, Ka. For CH3COOH, Ka = 1.8 × 10^-5, so pKa = -log(1.8 × 10^-5) = 4.74.Substituting the given values into the Henderson-Hasselbalch equation, we get:4.34 = 4.74 + log([CH3COO-]/[CH3COOH])Solving for [CH3COO-]/[CH3COOH], we get:[CH3COO-]/[CH3COOH] = 10^(4.34 - 4.74) = 0.39Therefore, the [CH3COO-]/[CH3COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34 is 0.39:1.

Question 20

What volume of 5.00 × 10^-3 mol L^-1 HNO₃(aq)is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH)₂(aq)to the equivalence point?

Accepted Answer

The reaction between HNO3 and Ca(OH)2 is a neutralization reaction where 2 moles of HNO3 react with 1 mole of Ca(OH)2. Given the concentrations are the same (5.00 × 10^-3 mol/L), and the volume of Ca(OH)2 is 80.00 mL, the volume of HNO3 needed is double that of Ca(OH)2 to reach the equivalence point, hence 160 mL.

Quiz 17: Additional Aspects of Acidbase Equilibria

A 25.0 mL sample of 0.150 mol L^-1 aqueous butanoic acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10^-5.

What is the pH of an aqueous buffer solution that is 0.211 mol L^-1 in lactic acid and 0.111 mol L^-1 in sodium lactate? The Of lactic acid is 1.4 × .

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

How many millilitres of 0.120 mol L^-1 NaOH(aq) are required to titrate 50.0 mL of 0.0998 mol L^-1 aqueous butanoic acid to the equivalence point? Butanoic acid is monoprotic.The Of butanoic acid is 1.5 × 10^-5.

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L^-¹ HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH) ₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

What is the pH of a buffer solution that is 0.255 mol L^-1 in hypochlorous acid (HClO) and 0.333 mol L^-1 in sodium hypochlorite (NaClO) ? The Of hypochlorous acid is 3.8 × .

A 25.0 mL sample of 0.150 mol L^-1 aqueous hypochlorous acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10^-8.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is

Calculate the pH of an aqueous solution that is 0.295 mol L^-1 in sodium formate (HCOONa) and In formic acid (HCOOH) .The Of formic acid is 1.77 × .

How many millilitres of 0.0850 mol L^-1 NaOH(aq) are required to titrate 25.0 mL of (aq) to the equivalence point?

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 methylamine,CH₃NH₂,with 20.00 mL of 0.10 mol L^-1 methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

A 25.0 mL sample of 0.150 mol L^-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10^-4.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the pH of an aqueous solution that is 0.210 mol L^-1 in nitrous acid ( ) and 0.290 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is 4.50 × .

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

What volume of 5.00 × 10^-3 mol L^-1 HNO₃(aq) is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH) ₂(aq) to the equivalence point?

Quiz 17: Additional Aspects of Acidbase Equilibria

A 25.0 mL sample of 0.150 mol L-1 aqueous butanoic acid is titrated with a 0.150 mol L-1 NaOH(aq) solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10-5.

What is the pH of an aqueous buffer solution that is 0.211 mol L-1 in lactic acid and 0.111 mol L-1 in sodium lactate? The Of lactic acid is 1.4 × .

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 NH3 with 5.00 mL of 0.10 mol L-1 NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 HCN with 50.00 mL of 0.010 mol L-1 NaCN? Assume that the volumes of the solutions are additive and that Ka =

How many millilitres of 0.120 mol L-1 NaOH(aq) are required to titrate 50.0 mL of 0.0998 mol L-1 aqueous butanoic acid to the equivalence point? Butanoic acid is monoprotic.The Of butanoic acid is 1.5 × 10-5.

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L-1 CH3COOH with 25.00 mL of 0.010 mol L-1 CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3COOH.

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH) 2 with 50.00 mL of 0.300 mol L-1 NaOH? Assume that the volumes are additive.

What is the pH of a buffer solution that is 0.255 mol L-1 in hypochlorous acid (HClO) and 0.333 mol L-1 in sodium hypochlorite (NaClO) ? The Of hypochlorous acid is 3.8 × .

A 25.0 mL sample of 0.150 mol L-1 aqueous hypochlorous acid is titrated with a 0.150 mol L-1 NaOH(aq) solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10-8.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L-1 in nitrous acid.The acid dissociation constant of nitrous acid is

Calculate the pH of an aqueous solution that is 0.295 mol L-1 in sodium formate (HCOONa) and In formic acid (HCOOH) .The Of formic acid is 1.77 × .

How many millilitres of 0.0850 mol L-1 NaOH(aq) are required to titrate 25.0 mL of (aq) to the equivalence point?

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 methylamine,CH3NH2,with 20.00 mL of 0.10 mol L-1 methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

A 25.0 mL sample of 0.150 mol L-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH(aq) solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10-4.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L-1 in nitrous acid And 0.112 mol L-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Calculate the pH of an aqueous solution that is 0.210 mol L-1 in nitrous acid ( ) and 0.290 mol L-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is 4.50 × .

What is the [CH3COO-]/[CH3COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? Ka = 1.8 × 10-5 for CH3COOH.

What volume of 5.00 × 10-3 mol L-1 HNO3(aq) is needed to titrate 80.00 mL of 5.00 × 10-3 mol L-1 Ca(OH) 2(aq) to the equivalence point?

A 25.0 mL sample of 0.150 mol L^-1 aqueous butanoic acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH before any base is added? Butanoic acid is monoprotic.The Of butanoic acid Is 1.5 × 10^-5.

What is the pH of an aqueous buffer solution that is 0.211 mol L^-1 in lactic acid and 0.111 mol L^-1 in sodium lactate? The Of lactic acid is 1.4 × .

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

How many millilitres of 0.120 mol L^-1 NaOH(aq) are required to titrate 50.0 mL of 0.0998 mol L^-1 aqueous butanoic acid to the equivalence point? Butanoic acid is monoprotic.The Of butanoic acid is 1.5 × 10^-5.

What is the pH of an aqueous solution made by mixing 25.00 mL of 0.100 mol L^-¹ HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of an aqueous solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

What is the pH of an aqueous solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH) ₂ with 50.00 mL of 0.300 mol L^-1 NaOH? Assume that the volumes are additive.

What is the pH of a buffer solution that is 0.255 mol L^-1 in hypochlorous acid (HClO) and 0.333 mol L^-1 in sodium hypochlorite (NaClO) ? The Of hypochlorous acid is 3.8 × .

A 25.0 mL sample of 0.150 mol L^-1 aqueous hypochlorous acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH after 26.0 mL of base is added? The Of hypochlorous acid is 3.0 × 10^-8.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.249 mol L^-1 in nitrous acid.The acid dissociation constant of nitrous acid is

Calculate the pH of an aqueous solution that is 0.295 mol L^-1 in sodium formate (HCOONa) and In formic acid (HCOOH) .The Of formic acid is 1.77 × .

How many millilitres of 0.0850 mol L^-1 NaOH(aq) are required to titrate 25.0 mL of (aq) to the equivalence point?

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 methylamine,CH₃NH₂,with 20.00 mL of 0.10 mol L^-1 methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

A 25.0 mL sample of 0.150 mol L^-1 aqueous hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH(aq) solution.What is the pH at the equivalence point? The Of hydrofluoric acid is 3.5 × 10^-4.

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the pH of an aqueous solution that is 0.210 mol L^-1 in nitrous acid ( ) and 0.290 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is 4.50 × .

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

What volume of 5.00 × 10^-3 mol L^-1 HNO₃(aq) is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH) ₂(aq) to the equivalence point?