(a)
Interpretation:
The circumstances under which the endpoint and equivalence point be the same is to be stated.
Concept introduction:
The reaction of an acid with a base results in the formation of salt and water. This reaction is known as neutralization reaction. Titration is a quantitative method used to find the concentration of either acid or a base in a given solution.
(b)
Interpretation:
The circumstance at which the endpoint and equivalent point be different is to be stated.
Concept introduction:
The reaction of an acid with a base results in the formation of salt and water. This reaction is known as neutralization reaction. Titration is a quantitative method used to find the concentration of either acid or a base in a given solution
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemistry for Today: General, Organic, and Biochemistry
- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?arrow_forwardPotassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.arrow_forward3) 2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution reaches to the equivalence point when 25 mL of an acid solution containing 1.22 g unknown monoprotic weak acid is added. (a) Calculate the molar mass of the unknown acid. (b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined to be 4.7. What is the Ka of the unknown acid? (NaOH = 40.0 g/mol)arrow_forward
- An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1.The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2.Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the pH.3.Some CH3CO2–(aq) will react with H3O+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium. b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3arrow_forward2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution reaches to the equivalence point when 25 mL of an acid solution containing 1.22 monoprotic weak acid is added. (a) Calculate the molar mass of the unknown acid. (b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined to be 4.7. What is the Ka of the unknown acid? (NaOH = 40.0 g/mol) unknownarrow_forwardFor the titration of an aqueous nitrous acid solution, HNO,(aq), with an aqueous strontium hydroxide solution, Sr(OH)2{aq), what do you expect the pH of the solution to be at the equivalence point? O Basic (pH > 7.00) O Unable to determine the pH of the solution at the equivalence point without additional information O Acidic (pH < 7.00) O Neutral (pH = 7.00)arrow_forward
- Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4 and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.arrow_forwardYou are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.arrow_forwardConsider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d pleasearrow_forward
- A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.arrow_forwardA chemistry graduate student is given 300. mL of a 0.60 M ammonia (NH,) solution. Ammonia is a weak base with K, = 1.8 x 10. What mass of NH,Br should the student dissolve in the NH, solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. do Ar x10 ?arrow_forwardA mixture of 100 ml of 0.025 M NH3 and 150 mL of 0.025 M NH4Cl was made. For this problem you need to show your calculation for each number. (A) What is the resulting concentration of the two solutes after mixing the solutions?(B) What is the pH of the solution produced?(C) What will happen if additional 100 mL water is added to the mixture?arrow_forward
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
- Chemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks ColeIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning