Suggest an indicator, other than phenolphthalein, that would be suitable for weak acid/strong...
Question:
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?
Indicator:
Indicators are used to indicate a change in the color of a solution at the end point in the acid-base titration. They are used in a small quantity. Phenolphthalein, methyl red, methyl blue are some common examples of indicators.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer
The choice of reagent depends upon the required pH range. the pH of methyl orange is between 3 to 4. Methyl orange tends to exhibit red colour in an...
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
Indicator Words: Definition & Examples
from
Chapter 6 / Lesson 21
70K
Explore premise and conclusion indicator words. Learn the definition of indicator, differentiate between premise and conclusion indicators, and view 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.
- Why was phenolphthalein a good indicator to use for determining the equivalence point between the unknown weak acid and strong base?
- The pH of a solution at the phenolphthalein endpoint is 9.0. For which type of titration could you use phenolphthalein as an indicator? (Select one) a) Titrations of strong acids only. b) Titration of all strong and most weak acids. c) Titrations of weak
- 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
- 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)
- Describe three characteristics of a good acid-base indicator for a particular titration.
- In an acid/base titration, why must the indicator (phenolphthalein) be a strong dye?
- Why is a weak acid-weak base titration different from strong acid-strong base/weak acid-strong base/strong acid-weak base titration?
- 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)?
- 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)
- Identify the following as a strong acid, weak acid, strong base, weak base, or neither: HS. a) Strong acid b) Weak acid c) Strong base d) Weak base e) Neither an acid nor a base
- Why is the equivalence point of a weak acid-strong base titration above 7.0?
- A titration curve of an unknown acid whose equivalence point is at pH = 7 suggests that: a) This is a weak acid because the equivalence point of all strong acids is below pH = 7. b) This is a strong acid because the equivalence point of all strong acids i
- (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.
- 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
- 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.
- Is CH3COOH classified as a strong acid, weak acid, strong base, or weak base? Explain.
- Is (CH3)2NH classified as a strong acid, weak acid, strong base, or weak base? Explain.
- Is HBr classified as a strong acid, weak acid, strong base, or weak base? Explain.
- Is HNO2 classified as a strong acid, weak acid, strong base, or weak base? Explain.
- In an aqueous solution, would (CH3)3N be classified as a strong acid, a weak acid, a strong base, or a weak base? Explain.
- What other acid indicators are there other than phenolphthalein? Are there any better indicators than phenolphthalein?
- 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
- 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): NH_3.
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): HCl.
- In titration of a weak base with strong acid to determine the value of K_b
- 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
- 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.
- What is acid base titration? What is alkalimetry and acidimetry? Discuss the methods in acid base titration, titration of weak acid and base.
- 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
- List the species present in solution during titration of a weak acid and a strong base: Equivalence Point.
- Identify the following as a strong acid, weak acid, strong base, weak base, or neither: NaCl. a) Strong acid b) Weak acid c) Strong base d) Weak base e) Neither an acid nor a base
- Is CsOH classified as a strong acid, weak acid, strong base, or weak base? Explain.
- An indicator is what type of compound? a. reducing agent b. oxidizing agent c. weak base or acid d. strong base or acid
- Complete the following neutralization reaction, and identify the strong acid, strong base, weak acid, and/or weak base. HCl + NH_3 to
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): KOH.
- 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.
- Identify each of the following substances as a strong acid, a weak acid, a strong base, a weak base, or a salt. a) K_3PO_4 b) CaBr_2 c) Mg(OH)_2 d) NH_4CI
- Identify each of the following substances as a strong acid, weak acid, a strong base, weak base, or salt. a. K_3PO_4 b. CaBr_2 c. MG(OH)_2 d. NH_4CL
- Phenolphthalein is an indicator that changes colour to pink/purple between pH 8 to 10, however, neutralization occurs when pH = 7. Why can phenolphthalein still be used as the indicator during a stron
- 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
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) HBr (b) HI
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) CH_3COOH (b) HCN
- Classify each substance as a strong acid, strong base, weak acid, or weak base. a. HCl b. HNO_3 c. HBr d. H_2SO_4 e. HNO_2 f. Ca(OH)_2 g. LiOH h. HCN i. NaOH j. Ba(OH)_2 k. NH_3 l. HCOOH
- Is C6H5COOH a strong acid, strong base, weak acid, or weak base?
- Is Sr(OH)2 a strong acid, strong base, weak acid, or weak base?
- Is Ca(OH)2 classified as a strong acid, weak acid, strong base, or weak base? Explain.
- 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
- 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
- Why is the pH of the equivalence point of a weak acid titrated with a strong base greater than 7?
- 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
- Explain why monoprotic acidic salts behave as strong enough acids to be titratable with NaOH using phenolphthalein as an indicator?
- 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)?
- List the species present in solution during titration of a weak acid and a strong base: Half Equivalence Point.
- What will be the effect of a weak acid in a back titration using a strong base?
- Determine (OH-) in a base solution of 1.95 M NH3. If the acid is weak, indicate the value that (OH-) is less than.
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for H_2CO_3.
- Which of the following is correctly identified? a) NH_3, strong acid b) NaOH, strong base c) HCl, weak acid d) H_2CO_3, strong acid e) Ca(OH)_2, weak base
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for (CH_3)_3N.
- Is HF classified as a strong acid, weak acid, strong base, or weak base? Explain.
- In order to lower the pH of water, salt of [{Blank}] should be added to it. a) Weak acid and strong base. b) Weak acid and weak base. c) Strong acid and strong base. d) Strong acid and weak base.
- Is HNO3 classified as a strong acid, weak acid, strong base, or weak base? Explain.
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for NaOH.
- 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?
- 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
- A substance of Ka of 1 x 10^5 would be classified as a. A. strong acid B. weak acid C. strong base D. weak base
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): HNO_3.
- Is HI a strong acid, strong base, weak acid, or weak base?
- Is NH3 a strong acid, strong base, weak acid, or weak base?
- List the species present in solution during titration of a strong acid and a strong base: Equivalence point
- Is CH3NH2 classified as a strong acid, weak acid, strong base, or weak base? Explain.
- Classify H2TeO2: a. strong acid b. weak acid c. strong base d. weak base
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) KOH (b) Ca(OH)_2
- Classify NaOH as one of the following. a. weak acid b. weak base c. strong acid d. strong 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
- Is a solution that turns the pH paper orange a weak acid, a strong acid, a weak base, or a strong base? Explain.
- Which of the following is correctly identified? a. NaOH, weak base b. H2SO4, strong acid c. NH3, strong acid d. H2CO3, strong acid
- 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
- Is HClO4 classified as a strong acid, weak acid, strong base, or weak base? Explain.
- Is a solution that turns the pH paper blue a weak acid, a strong acid, a weak base, or a strong base? Explain.
- How can we determine the equivalence point (or endpoint) in the curves in titration (strong acid/weak base and weak acid/strong base)?
- 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
- During a titration of a weak acid with a strong base, add an additional small amount of base after reaching the equivalence point. How does the K_a of the acid change? (a) Increase (b) Decrease (c) Remain unchanged
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for Ba(OH)_2.
- Classify the compounds given below as a strong acid, weak acid, strong base, or weak base. Place the compounds in the appropriate bins. strong acid, weak acid, strong base, or weak base Ca(OH)_2, H
- Is HCl classified as a strong acid, strong base, weak acid, or weak base?
- Which of the following is correctly identified? a. H2CO3, strong acid b. NH3, strong acid c. NaOH, strong base d. HCI, weak acid e. Ca(OH)2, weak base
- In the following acid-base reaction, classify each substance as the stronger acid, weaker acid, stronger base, or weaker base. A table of acids and their conjugate bases, listed by relative strength,
- Does a higher or lower Ka value indicate a strong acid? Explain why. Does a higher or lower pKa value indicate a weak acid?
- The addition of a strong base to a weak acid in a titration creates a buffer solution. What is a buffer solution?
- Is NaOH classified as a weak or strong acid or base? Explain.
- 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
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for HNO_3.
- Will a weak acid/strong base neutralization have the same molar heat of neutralization as the strong acid/strong base neutralization? Explain.
- Label each compound as one of the following : Strong acid, Weak acid, Strong base, Weak base, conjugate acid and conjugate base as well as balance where it needs be. NaOH + HNO3 \rightarrow H2O + HNO2
- Carbonic acid has a Ka value of 4.5 x 10-7. Based on this value, carbonic acid can be classified as a: a. weak acid b. strong base c. strong acid d. weak base
- In an aqueous solution, classify the compound as a strong acid, weak acid, strong base, weak base, or other for HF.
- Is NH3 classified as a weak or strong acid or base? Explain.
- The indicator you used in the titration was thymol blue. This indicator changes color at the end point from red (acidic) to yellow at pH 2.0. Suppose you chose phenolphthalein, which changes color at the end point from colorless (acidic) to pink at pH 8.5
Explore our homework questions and answers library
Browse
by subject