Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

In a Strong Acid-Strong Base Titration we do not use an ICF Chart or ICE Chart to determine the pH of the solution. 

Strong Acid-Strong Base Titration

Concept #1: Strong Acid-Strong Base Titration

Example #1: Calculate the pH of the solution resulting from the titration of 75.0 mL of 0.100 M HBrO4 with 55.0 mL of 0.100 M NaNH2

If after the titration there is an excess of strong acid left then we can use its concentration to find the pH. 

If after the titration there is an excess of strong base then we can use its concentration to find pOH initially. 

Practice: Calculate the pH of the solution resulting from the mixing of 175.0 mL of 0.250 M HNO3 with 75.0 mL of 0.200M Ba(OH)2.

If there is an equal amount of moles for both the strong acid and strong base then the pH of the solution will be 7. 

Additional Problems
A student is titrating 38.0 mL of 0.0358 M solution of HBr with a 0.0289 M KOH solution. Calculate the pH of the solution after the addition of 43.19 mL of the KOH solution. A. 2.53 B. 3.57 C. 12.46 D. 2.86 E. 1.78
Determine the pH of a solution created by mixing 95.0 mL of 0.200 M nitric acid, HNO3, with 320.0 mL of 0.078 M potassium hydroxide, KOH. A. 2.22 B. 12.16 C. 0.91 D. 11.78 E. 1.84
A 10. mL sample of 0.20 M chloric acid solution is required to neutralize 20. mL of sodium hydroxide solution, NaOH.  a. What is the molarity of the sodium hydroxide solution?       b. What is the molarity of the salt that forms?
A 10. mL sample of 0.20 M hydrochloric acid solution is required to neutralize 20. mL of barium hydroxide, Ba(OH)2 a. What is the molarity of the barium hydroxide solution?       b. What is the molarity of the salt that forms?
Calculate the pH of a solution resulting from the titration of 113.00 mL of 0.0442 M HCIO3 with 82.65 mL of 0.0624 M LiOH. A. 10.92 B. 3.08 c. 10.21 D. 10.54 E. 7.00
A flask contains 50.0 mL of a 0.000968 M solution of Hydrochloric acid, HCl. The acid is to be titrated against 0.0275 M Sodium hydroxide, NaOH. What is the pH of the acid in the flask before the addition of any NaOH? a. 1.32 b. 1.71 c. 3.01 d. 4.32 e. 1.56
Calculate the pH of a solution created by mixing 120.0 mL of 0.375 M Perchloric Acid, HClO4, with 360.0 mL of 0.125 M lithium hydroxide, LiOH. a. 7.000 b. 0.426 c. 13.100 d. 0.602 e. 13.398
Calculate the pH of the solution resulting from the addition of 32.0 mL of 0.220 M HClO4 to 76.0 mL of 0.170 M NaOH. 1. 12.89 2. 7.00 3. 1.26 4. 1.11 5. 13.23 6. 12.74  7. 0.77
A 100.0 mL sample of 0.18 M HBrO 3 is titrated with 0.27 M LiH. Determine the pH of the solution after the addition of 30.0 mL of LiH. A) 0.86 B) 1.21 C) 2.00 D) 1.12 E) 2.86
Initially 7.1 g of HCl (MM = 36.46) and 9.5 g of NaOH (MM = 40.00) is added to water making a solution that has a volume of 12.85 L. What is the pH of the solution? A. 1.82 B. 2.48 C. 7.00 D. 11.52 E. 12.27
A solid sample of Zn(OH)2 is added to 0.310 L of 0.520 M aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.520 M NaOH solution, and it takes 90.5 mL of the NaOH solution to reach the equivalence point.What mass of Zn(OH)2 was added to the HBr solution?
In the titration of a strong acid with a strong base, how would you calculate these quantities?pH beyond the equivalence point
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the initial pH
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the pH at 5.1 mL of added acid
In the titration of a strong acid with a strong base, how would you calculate these quantities?pH at the equivalence point
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the pH at the equivalence point
In the titration of a strong acid with a strong base, how would you calculate these quantities?pH before the equivalence point
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the pH after adding 5.1 mL of acid beyond the equivalence point
A 25.00 mL sample of 0.320 M NaOH analyte was titrated with 0.750 M HI at 25 °C. a) Calculate the initial pH before any titrant was added. b) Calculate the pH of the solution after 5.00 mL of the titrant was added.
Calculate the pH of the resulting solution if 29.0 mL of 0.290 M HCl (aq) is added to 39.0 mL of 0.290 M NaOH (aq).
a. Write a balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional.b. 0.850 L of 0.420 M H2SO4 is mixed with 0.800 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?
A 100.00 mL sample of 0.18 M HClO 4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point).a. 13.03 b. 7.00c. 2.76 d. 0.97 e. 11.24
Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)  2 solution. What is the concentration of the excess H+ or OH– ions left in this solution?
A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Is the resulting solution neutral? If not, calculate the concentration of excess H+ or OH– ions left in solution.
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to: a. 30.0 mL of 0.200 M NaOH(aq) b. 10.0 mL of 0.300 M NaOH(aq)
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH after adding 5.0 mL of base beyond the equivalence point
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(f) 40.10 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(d) 39.90 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(g) 50.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.20.0 mL of the acid
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.23.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.e. 100.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.a. 0.0 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(a) 0 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(b) 15.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(c) 29.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(d) 29.90 mL
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH at the equivalence point
Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)  2 solution. What is the concentration of the excess H+ or OH- ions left in this solution?
A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H+ or OH- ions left in solution.
A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid.What is the pH of the solution as the equivalence point?
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(e) 40.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.24.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.d. 80.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.b. 20.0 mL
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.c. 100.0 mL of 0.50 M HCl titrated by 0.25 M NaOH
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(e) 30.00 mL
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH at 11.1 mL of added base
A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 55.6 mL 0.200 M HNO3.
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(a) 0 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(b) 25.00 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(c) 39.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.26.0 mL of the acid
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.31.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.a. 0.0 mL
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.b. 10.0 mL
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.c. 40.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.c. 30.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.d. 40.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.e. 80.0 mL
Calculate the pH after the addition of 0.0 mL, 4.0 mL, 8.0 mL, 12.5 mL, 20.0 mL, 24.0 mL, 24.5 mL, 25.0 mL, 26.0 mL, 28.0 mL, and 30.0 mL of the NaOH for the titration of 25.0 mL of 0.100 M HNO3 with 0.100 M NaOH. Plot the results of your calculations as pH versus milliliters of NaOH added.
A 20.0-mL sample of 0.125 M HNO3 is titrated with 0.150 M NaOH. Calculate the pH for at least five different points throughout the titration curve and make a sketch of the curve.
A 15.0-mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. Calculate the pH for different points throughout the titration curve and make a sketch of the curve.
Consider the titration of 150.0 mL of 0.100 M HI by 0.250 M NaOH.a. Calculate the pH after 20.0 mL of NaOH has been added.
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(f) 30.10 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(g) 40.00 mL
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCI(aq) is added toa. 30.0 mL of 0.200 M NaOH(aq).b. 10.0 mL of 0.300 M NaOH(aq).
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to:a. 30.0 mL of 0.200 M NaOH(aq)b. 10.0 mL of 0.300 M NaOH(aq)
A 25.0 mL sample of 0.105 M HCl was titrated with 315 mL of NaOH. What is the concentration of the NaOH?
The titration of 42.35 mL of H2SO4 requires 21.17 mL of 0.5000 M NaOH for complete neutralization. Calculate the concentration of H2SO4.(A) 0.2499 M H2SO4 (B) 0.1250 M H2SO4 (C) 0.4998 M H2SO4 (D) 1.000 M H2SO4 (E) 0.36 M H2SO4
Write the balanced neutralization reaction between H2SO4 (sulfuric acid) and KOH (potassium hydroxide) in aqueous solution. Also find the concentration of sulfuric acid remaining after 0.150L of 0.470 M H2SO4 is mixed with 0.100L of 0.230 M KOH. 
What is the pH of a solution made by mixing 40.0 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.A) 0.64B) 1.64C) 12.36D) 13.36E) 10.00
Calculate the pH of the resulting solution if 35.0 mL of 0.350 M HCl(aq) is added toa) 25.0 mL of 0.450 M NaOH(aq)pH = _____b) 45.0 mL of 0.350 M NaOH(aq)pH = _____
Calculate the pH of the resulting solution if 28.0 mL of 0.280 M HCl(aq) is added to(a) 38.0 mL of 0.280 M NaOH(aq)pH =(b) 18.0 mL of 0.380 M NaOH(aq).pH =
Calculate the pH of the resulting solution if 27.0 ml of 0.270 M HCl is added toa) 32.0 ml of 0.270 M NaOH(aq)b) 37.0 ml of 0.320 M NaOH(aq)
A 25.0 mL sample of 0.723 M HCIO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is _____ M. a) 0.4b) 1x10-7c) 0.7d) 3x10-13e) 4x10-2
A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 19.00 mL sample of her gastric juices and titrate the sample with 0.000452 M KOH. The gastric juice sample required 11.3 mL of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia?          (a) No          (b) Yes          (c) Unable to determine
What is the molarity of a sulfuric acid solution if it requires 62.55 mL of 0.09918 M NaOH to completely neutralize 25.00 mL of the acid? H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O (l) Give your answer to 4 significant figures and DO NOT include the units.
What volume of 0.236 M H2SO4 is needed to react with 53.5 mL of 0.104 M NaOH? The equation is H2SO4 aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O (l) 
An aqueous solution of hydrobromic acid is standardized by titration with a 0.162 M solution of calcium hydroxide.If 21.5 mL of base are required to neutralize 27.6 mL of the acid, what is the molarity of the hydrobromic acid solution? 
Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. 0.750 L of 0.450 M H2SO4 is mixed with 0.700 L of 0.230 M KOH. What concentration of sulfuric acid remains after neutralization? 
How many moles of H3O+ or OH- must you add to a liter of strong base solution to adjust its pH from 8.090 to 7.720? Assume a negligible volume change.
Enter your answer in the provided box.If 46.01 mL of a standard 0.2577 M NaOH solution is required to neutralize 41.09 mL of H2SO4, what is the molarity of the acid solution?
100. mL of 0.200 M HCl is titrated with 0.250 M NaOH.i) What is the pH of the solution after 50.0 mL of base has been added? Express the pH numerically.    ii) What is the pH of the solution at the equivalence point? Express the pH numerically.
Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added: 0, 5,10,12 mL