The correct indicator for a given titration system depends on the strength of the acid being...
Question:
The correct indicator for a given titration system depends on the strength of the acid being titrated. How could we determine the strength of the acid in order to pick an appropriate indicator (i.e. an indicator that is weaker than the acid)?
Acid Strength:
Acids considered to be strong have a high dissociation constant (Ka), while those considered weak have a low dissociation constant. The logarithmic constant (pKa) of acid varies inversely to the dissociation constant.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThere is a variety of methods that can be used to determine the most appropriate indicator to use. One of the methods is the use of a pH meter to...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Acidic Solutions: Properties & Examples
from
Chapter 16 / Lesson 1
25K
Learn about acidic solutions. Understand what an acidic solution is, what makes it an acidic solution, its general properties, the value of pH, and examples.
Related to this Question
- An indicator with a value of PKln is not suitable for the titration of a weak base versus a strong acid. Explain.
- (a) What is the role of an indicator in an acid-base titration? (b) How an appropriate indicator is chosen? (c) Explain how an indicator works.
- How can we determine the equivalence point (or endpoint) in the curves in titration (strong acid/weak base and weak acid/strong base)?
- When choosing a suitable indicator for a titration between a strong acid and a weak base, the indicator should change color in the pH range of: a) exactly 7 b) less than 7(slightly acidic) c) greater than 7(slightly basic) d) near 14(very basic)
- Suggest an indicator, other than phenolphthalein, that would be suitable for weak acid/strong base and weak base/strong acid titration. Explain why it would be effective?
- a) In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? b) How are the pK_a and K_a of the weak acid determined from the half equivalence point?
- Why was phenolphthalein a good indicator to use for determining the equivalence point between the unknown weak acid and strong base?
- Which of the pH indicators from the following would be most appropriate for the titration of 0.30 M hydroxylamine (K_b = 9.1 x 10^{-9}) with 0.15 M hydrochloric acid? A) Methyl orange. B) Litmus. C) Thymol blue. D) trinitrobenzene. E) None.
- 1. Why is phenolphthalein an appropriate indicator for titration of a strong acid with a strong base? Explain based on the pH at the equivalent point and the transition range for phenolphthalein. 2. A
- Why is the equivalence point of a weak acid-strong base titration above 7.0?
- Describe three characteristics of a good acid-base indicator for a particular titration.
- At the equivalence point of an experiment where a strong acid is titrated using a strong base, which of the following statements is/are true? Select as many as appropriate. A) number of moles of acid initially = number of moles of base added B) Phenolphth
- For the acid/base titration of HNO3 and CH3NH2, choose a suitable indicator from the list below. Beside each indicator, the pH range of colour change at its endpoint is provided. (a) methyl orange (3.1 - 4.4) (b) bromothymol (6.0 - 7.7) (c) thymolphthalei
- Give the structure for an acid-base indicator. It can be any acid-base indicator, except phenolphthalein. Explain how an acid-base indicator works (why it changes color when it does). Give the chemical reaction(s) that shows why the color changes in your
- What is acid base titration? What is alkalimetry and acidimetry? Discuss the methods in acid base titration, titration of weak acid and base.
- Sketch the titration curves for the following: a. Titration of a strong acid with a strong base. b. Titration of a weak diprotic acid with a strong base. c. Titration of a weak base with a strong acid.
- In an acid/base titration, why must the indicator (phenolphthalein) be a strong dye?
- How does an acid - base indicator such as methyl orange work in a system at equilibrium? What is the dominant species of the indicator when the solution is acid or base?
- Circle which one of the following indicators you would select for a titration of a strong acid against a strong base. (i) Phenolphthalein (pH range 8.3 - 10.0, colourless \rightarrow pink) (ii) Phenol red (pH range 4.4 - 6.2, red \rightarrow yellow) (iii)
- The classification of an acid or a base as weak or strong is determined by: 1) the extent of dissociation of the dissolved acid or base. 2) the solubility of the acid or base. 3) the concentrations of the acid or base. 4) more than one choice is correct.
- Which of the following conditions is true for a titration of a strong acid with a weak base? a. The equivalence point occurs at a pH greater than 7. b. The equivalence point occurs at a pH equal to 7. c. The equivalence point occurs at a pH below 7. d. Eq
- An acid base indicator like bromocresol green is blue under basic conditions and yellow under acidic conditions. What would be a good methodology to quantify a substance of this sort which has general equilibrium as followed: H_2O + Hln \leftrightarrow
- Choose the correct classification for SO3^2-(aq). a. Polyprotic base b. Polyprotic acid c. Monoprotic acid d. Monoprotic base
- Sketch the following titration curves. a) A strong acid/strong base. b) A weak monoprotic acid/strong base. c) A weak diprotic acid/strong base.
- Choose the correct classification for HCOOH(aq). a. Polyprotic base b. Polyprotic acid c. Monoprotic acid d. Monoprotic base
- A suitable indicator for the titration of 0.1 M NaHS with 0.1 M HCl would be A. methyl violet B. methyl orange C. phenolphthalein D. thymolphthalein
- How can you determine the strength of antacids by titration with stomach acid (HCL)?
- 1. Explain the chemical information that can be determined about an acid using the equivalence point and half-equivalence point of a titration curve. 2. Describe when you can use the Henderson- Hasse
- List the species present in solution during titration of a strong acid and a strong base: Equivalence point
- Which indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq)? For lactic acid, pKa = 3.08.
- Choose the correct classification for HSO3-(aq). a. Polyprotic base b. Polyprotic acid c. Monoprotic acid d. Monoprotic base
- Which of the following are true regarding a Gran Plot? Select all that are appropriate. (a) The equivalence point of the titration is represented by the y-intercept. (b) The slope of the plot depends on Ka for the acid being titrated. (c) Results in a str
- Which of the following indicators would be most suitable for the titration of 0.1 M lactic acid with 0.10 M KOH(aq)? For lactic acid, pKa = 3.08. (a) thymol blue (pKin = 1.7) (b) phenol red (pKin = 7.9) (c) alizarin yellow (pKin = 11.2) (d) methyl orange
- In the titration of a strong acid with a strong base, once the equivalence point has been reached and excess base is added, the pH: a. depends on the hydrolysis of the conjugate base. b. depends on the amount of strong base added after the equivalence poi
- What are the expected differences that should be observed for titration of a strong acid, weak acid, and polyprotic acid with a strong base like NaOH (aq)?
- Determine (OH-) in a base solution of 1.95 M NH3. If the acid is weak, indicate the value that (OH-) is less than.
- How do you determine the strength of an acid?
- Sketch the titration curve for the titration of a generic weak base B with a strong acid. The titration reaction is B + H^+ to BH^+ On the curve indicate the points that correspond to the following. a. The stoichiometric (equivalence) point. b. The region
- Match the statement with the type of titration: 1. strong acid-strong base 2. weak acid-strong base 3. strong acid-weak base it would apply to. Titration types can be used more than once or not at all. (a) Endpoint/Equivalence point pH is basic. (b) Endpo
- Why is a weak acid-weak base titration different from strong acid-strong base/weak acid-strong base/strong acid-weak base titration?
- In the titration of a strong acid with a strong base, the pH of the initial acid solution (before the addition of base): a. depends on the concentration of the acid. b. is raised because of the presence of a conjugate base. c. depends on the K and concent
- Sketch a titration curve of a monoprotic acid and dioprotic acid titrated with a strong base, labeling the equivalence point. In addition label where the solution is a) acidic b) basic c) contains mostly acid with some conjugate base and d) contains only
- The graph shows the titration curves of a 1 M solution of a weak acid with a strong base and a 1 M solution of a strong acid with the same base. What is the pK_a value of the weak acid in the figure?
- Determine OH- in each base solution. If the acid or the base is weak, indicate the value that OH- is less than. a) 0.25 M NaOH b) 0.24 M NH3 c) 0.25 M Sr(OH)2 d) 1.25 M KOH
- List the species present in solution during titration of a weak acid and a strong base: Equivalence Point.
- The pH at the equivalence point of a weak acid-strong base titration is _____ because _____. 1. greater than 7; of the presence of excess strong base 2. greater than 7; the strong base produces a greater pH change above 7 than a weak acid does below 7
- Which of the following is true about indicators? A. They are weak acids or bases. B. They are as accurate as a pH meter. C. They maintain their colors across the range of pH values for which they a
- Identify the strongest acid in the following set and give the correct reasoning.H2O, HF, HCl a) HCl. Strength of binary acids increase down the column due to increasing size. b) HF Strength of binary acids increase across the row due to increasing electro
- Why is the pH of the equivalence point of a weak acid titrated with a strong base greater than 7?
- Sketch two pH curves, one for the titration of a weak acid with a strong base, and one for the titration of a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
- In the titration of a weak acid with a strong base, once the equivalence point is reached, the pH is determined by the: a. weak acid and conjugate base buffer system. b. total amount of strong base added. c. hydrolysis of the conjugate base. d. amount of
- When ranking the strength of acids in aqueous solution, water is acting as: a. a base b. an acid c. both an acid and a base d. neither an acid nor a base
- 1. What is a primary standard substance? Give an example. 2. What is meant by the term, equivalence point, during an acid-base titration? 3. What is an indicator? What role does it play in an acid-b
- List the species present in solution during titration of a strong acid and a strong base: At the half-equivalence point.
- Provide definitions for the following terms: a. Neutralization. b. acid-base indicator. c. volumetric titration.
- For the following acid-base reaction, Identify the weakest base, weakest acid and draw an arrow to show whether the equilibrium goes to the right or left.
- Give the equation for equivalence point for strong acid weak base?
- Answer the following statement, and explain your answer. It is always true that the equivalence point of a standard weak acid/strong base titration is: A) When the pH = 7.00 B) Reached when all of the weak acid has been converted into its conjugate wea
- List the species present in solution during titration of a weak acid and a strong base: Half Equivalence Point.
- 1. Define the following terms: *weak acid *strong base *equivalence point *primary standard 2. A sample of acetic acid (weak acid) was neutralized with 0.05 M NaOH solution by titration. 34 mL of NaOH had been used. CH_3COOH + NaOH --> CH COONa + H_2O a
- How is the strength of a weak acid or a weak base determined? Explain how the pH of the salt of a weak acid may be determined.
- Choose the correct classification for H2PO4-(aq). a. Polyprotic base b. Polyprotic acid c. Monoprotic acid d. Monoprotic base
- Would this spectroscopic method of determining an equilibrium constant work for other acid/base indicators such as thymol blue, cresol red and phenolphthalein? Why or why not? Used a bromothymol blue
- Explain why monoprotic acidic salts behave as strong enough acids to be titratable with NaOH using phenolphthalein as an indicator?
- When ranking the strength of acids in aqueous solution, what is water acting as? A. a base B. an acid C. both an acid and a base D. neither an acid nor a base
- 1. A 0.15 M solution of a weak diprotic acid is 4 7% dissociated. Calculate the acid dissociation constant for this acid. 2. Classify each of the following samples as a strong acid or a weak acid. Us
- Methyl red has the following structure: What is the color change and the pH at the color change when a weak base is titrated with a strong acid using methyl red as an indicator? For which of these two types of titrations is methyl red a possible indicator
- Arrange in the order of increasing strength of the ACID ( if the values are listed for a base, then calculate the equilibrium constant for the conjugated acid): #1 pKb of the conjugated base for acid
- Acid base indications usually show a colour change: a. at exactly the pKin of the indicator b. generally over the range pKin +/- 1 c. at exactly pH =7
- In deciding which of two acids is the stronger, one must know a. the concentration of each acid solution b. the pH of each acid solution c. the equilibrium constant of each acid d. all of these e. both a and c
- In deciding which of two acids is stronger, one must know: A. the concentration of each acid solution B. the pH of each acid solution C. the equilibrium constant of each acid D. all of the above E. both A and C
- What is an acid/base indicator?
- Consider the titration of a generic weak acid HA with a strong base that gives the following titration curve: On the curve indicate the points that correspond to the following. a. the equivalence point b. the maximum buffering region c. pH = pKa d. pH dep
- What is a strong acid? How is a strong acid different than a concentrated acid? What is an example of a calculation where equal concentrations of acid solutions may have different pH levels due to differences in acid strengths?
- Litmus (C_{12}H_7NO_3), shown below, is the acid-base indicator responsible for the color change that occurs with litmus
- What does the color indicate about the strength of an acid or base?
- Determine (OH-) in a base solution of 0.225 M Ba(OH)2. If the acid is weak, indicate the value that (OH-) is less than.
- When a strong acid is used to titrate a weak base, the PH at the equivalence point: a. Is greater than 7.0 b. Is less than 7.0 but more than 3.5 c. Is equal to the pKa of the acid d. Is equal to 3.5
- What is the role of an acid-base indicator?
- ||Indicator||Color of acid form||Color of base form||Ka value |'A'|red|yellow|1.0 x 10¯³ |'B'|yellow|blue|1.0 x 10¯⁹ What are the predominant colors of each indicator at pH 7?
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): KOH.
- A weak base indicator (In) may be considered to be in equilibrium with HIn^+ and OH^ ions. The color of the non-ionized molecule is green and that of HIn is yellow. What would be the color of this indicator in a very acidic solution? Explain.
- The graph below shows the titration curves for two monoprotic acids. Estimate the pKa of the weak acid. [{Image src='graph3801282308883644897.jpg' alt='acid' caption=''}]
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): CH_2CO_2H.
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): HCl.
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): NH_3.
- Indicators: weak acid-base equilibrium A. Water and Methyl Orange HIn = In- + H+ After the addition of 6 M HCl to the test tube, what is the color of the solution? How does the addition of HCl affe
- What is an acid-base indicator and how is it used in a liquid-liquid extraction?
- Is it possible to determine the Ka of a weak acid at points other than the halfway point of a titration? Explain.
- Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid? A. less than zero B. between 0 and 7 C. close to 7.0 D. between 7 and 14 E. greater than 14
- How does an acid-base indicator function?
- What determines the color of an acid-base indicator in an aqueous solution?
- Phenophthalein is often used to identify the endpoint of the titration of a strong acid with a strong base because the start of the colorless to pink-red color transition is easily identifed. However,
- Thus, whether a reaction "goes" or "does not go" can be used to determine the relative strength of the Bronsted acids and bases in the reaction. From the data below, determine the order of the strengths of the three Bronsted acids. Reaction 1: H 3 P O 3
- An acid turns the indicator litmus to what color?
- Which of the following procedures is the best way to determine the acidity or basicity of a volatile liquid with litmus paper? (a) Using a pair of tweezers, hold a water-soaked piece of litmus paper above the surface of the liquid (b) Place at least 1 mL
- Which best describes the pH at the equivalence point of a titration of a weak acid with a strong base? A. less than zero B. between 0 and 7 C. close to 7.0 D. between 7 and 14 E. greater than 14
- What are the chemical and physical properties of litmus? What allows it the ability to act as an acid-base indicator?
- Describe the apparent relationship between H_3O and OH concentrations when an endpoint is reached in acid-base titration.
- Phenolphthalein indicator is often used for HCl/NaOH titrations. The indicator turns faint pink with the first drop of excess base. Which statement(s) correctly explains this behavior? (choose all that apply) A. The acidic form of phenolphthalein does not
Explore our homework questions and answers library
Browse
by subject