Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
8th Edition
ISBN: 9780134421377
Author: Charles H Corwin
Publisher: PEARSON
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Chapter 14, Problem 6CE
Interpretation Introduction
Interpretation:
The titration among strong acid with strong base, strong acid with weak base, and weak acid with strong base which describes the titration of
Concept introduction:
According to
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Which of the following describes the titration of HCl(aq) with Ba(OH)2(aq): strong acid with strong base, strong acid with weak base, or weak acid with strong base?
Consider the titration of 100 mL of 0.25 M formic acid (HCOOH) with 1.0 M NaOH. The Ka of formic acid is 1.77 × 10−4.
HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l)
What is the pH of the formic acid solution before any titrant (NaOH) is added?
A student is conducting a titration between a weak, monoprotic acid and sodium hydroxide, NaOH. The student titrates 20.0 mL of the weak acid with 0.300 M sodium hydroxide, NaOH(aq). When 5.00 mL of NaOH(aq) has been delivered the pH of the weak acid is 5.328. Determine the Ka of the weak acid.
Chapter 14 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
Ch. 14 - Prob. 1CECh. 14 - Prob. 2CECh. 14 - Prob. 3CECh. 14 - Prob. 4CECh. 14 - Prob. 5CECh. 14 - Prob. 6CECh. 14 - Prob. 7CECh. 14 - Prob. 8CECh. 14 - Prob. 9CECh. 14 - Prob. 10CE
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- Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.arrow_forwardGiven the acid-base indicators in Question 37, select a suitable indicator for the following titrations. (a) sodium formate (NaCHO2) with HNO3 (b) hypochlorous acid with barium hydroxide (c) nitric acid with HI (d) hydrochloric acid with ammoniaarrow_forwardSodium bicarbonate, NaHCO3, is used in baking powder formulations and in the manufacture of plastics and ceramics, among other things. If 26.3 g of the compound is dissolved in enough water to make 200. mL of solution, what is the concentration of NaHCO3? What are the concentrations of the ions in solution?arrow_forward
- Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardA solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka propionic acid = 1.4 x 10^-5 ). a) calculate the moles of the reactants. Which is the limiting reactant? b) What will be the moles of the products? What are the moles of the excess reactant? c) calculate the pH of the acid bufferarrow_forward
- A 25.00-mL sample of propionic acid, HC3H5O2, of unknown concentration was titrated with 0.145 M KOH. The equivalence point was reached when 43.02 mL of base had been added. What was the original concentration of the propionic acid?arrow_forwardFor a conductivity experiment a student mixed 25 mL of a .2 M HNO2 (4.5 x 10^-4) with 25 mL of a .2M NaOH in a 100.0 mL glass beaker. To increase the conductivity of the mixture to adjust the pH the student dissolved 1.321g of calcium nitrite in solution. What is the pH of the solution? To 3 sig figsarrow_forward8.When a small amount of 12 M HNO3(aq) is added to a buffer solution made by mixing CH3NH2(aq) and CH3NH3Cl(aq), the pH of the buffer solution changes from 10.64 to 10.62. Which of the following equations represents the reaction that accounts for the fact that the pH does not change significantly when the HNO3(aq) is added? a) CH3NH2(aq) + H+(aq) → CH3NH3+(aq) b)CH3NH3+(aq) + H+(aq) → CH3NH42+(aq) c) NO3- (aq) + H+(aq) → HNO3(aq) d) OH- (aq) + H+(aq) → H2O(l)arrow_forward
- If 100.0 mL of 0.250 M HBr is titrated with 0.150 M KOH answer the following questions. What is the pH of the solution before the titration begins? How many milliliters of NaOH must be added to reach the equivalence point? HBr (aq) + KOH (aq) KBr (aq) + H2O (l) What is the pH of the solution at the equivalence point? What is the pH of the solution when 30.0 mL of KOH has been added? What is the pH of the solution when 180.0 mL of KOH has been added?arrow_forwardAn important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. (a) What is the ratio of [H2CO3] to [HCO3− ]?(b) What does the pH become if 14% of the bicarbonate ions are converted to carbonic acid? (c) What does the pH become if 26% of the carbonic acid molecules are converted to bicarbonate ions?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_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY