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
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) 0.64 B) 1.64 C) 12.36 D) 13.36 E) 10.00
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 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.
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
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.
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)
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. 
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 0.723 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 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?