Consider the titration of a generic weak acid HA with a strong base that gives the following...
Question:
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. {eq}\text{pH}=\text{p}{{K}_{\text{a}}} {/eq}
d. pH depends only on {eq}\left[ \text{HA} \right] {/eq}
e. pH depends only on {eq}\left[ {{\text{A}}^{-}} \right] {/eq}
f. pH depends only on the amount of excess strong base added
Weak acid
Acids that are only partially ionized when dissolved in water are considered weak acids. Examples of weak acids are acetic acid, {eq}CH_3COOH {/eq} and nitrous acid, {eq}HNO_2 {/eq}. Weak acids produce strong conjugate bases. This is the reason why in the titration of a weak acid with a strong base, the pH of the solution at the equivalence point is above 7.00.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe neutralization reaction between the weak acid, HA and a strong base like sodium hydroxide is shown below.
{eq}HA_{(aq)}\;+\;NaOH_{(aq)}\;\to\;Na^...
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
Titrations with Weak Acids or Weak Bases
from
Chapter 11 / Lesson 10
20K
Learn about titrations of weak acids and strong bases, strong acids and weak bases, and weak acids and weak bases. Explore types of titration curves and the pH.
Related to this Question
- 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
- How can we determine the equivalence point (or endpoint) in the curves in titration (strong acid/weak base and weak acid/strong 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.
- When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a. zero b. one c. two d. three
- 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.
- Sketch the general appearence of the curve for the titration of a weak diprotic acid with NaOH. a) Indentify the location of the inflection points in the curve b) Identify the maxima and minima in t
- 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
- Why is the equivalence point of a weak acid-strong base titration above 7.0?
- 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
- 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.
- 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
- 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
- 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?
- In which type of titrations can buffering regions occur? a) Strong acid/strong base titrations b) Strong acid/weak base titrations c) Weak acid/strong base titrations
- 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 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
- 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
- a) What is an acid-base indicator? b) Define the equivalence (stoichiometric) point and the endpoint of a titration. Why should you choose an indicator so that the two points coincide? c) Do the pH values of the two points have to be within \pm 0.01 pH
- A friend of yours has performed three titrations: strong acid with a strong base, weak acid with a strong base, and weak base with a strong acid. He hands you the three titration curves, saying he has forgotten which is which. What attributes of the curve
- Does a single S-shaped curve (sigmoidal curve) for an acid-base titration graph means that the acid used was a diprotic acid.
- Distinguish between a stoichiometric point and an endpoint in an acid-base titration.
- In titration of a weak base with strong acid to determine the value of K_b
- When a weak acid is titrated with a weak base, the pH at the equivalence point: A. is greater than 7.0. B. is equal to 7.0. C. is less than 7.0. D. is determined by the magnitudes of Ka and Kb. E. depends on the pKa of the indicator.
- 1. What is the difference between equivalence point and endpoint? 2. In a titration with a strong acid and a strong base, why used phenolphthalein as the indicator? 3. If the color remains clear, th
- List the species present in solution during titration of a weak acid and a strong base: Half Equivalence Point.
- Why is a weak acid-weak base titration different from strong acid-strong base/weak acid-strong base/strong acid-weak base titration?
- For each of the following, classify the substance as a strong acid, strong base, weak acid, or weak base (or perhaps not acidic or basic). Then determine the pH of the solution and calculate the conce
- 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
- (a) Draw a titration curve for phosphoric acid, H 3 P O 4 , using O H as the titrant. Label the points in the curve where each form of the acid is the principle species. Where buffers are present, label those as well. Given the p K a values of the
- Is it possible to determine the Ka of a weak acid at points other than the halfway point of a titration? Explain.
- Why do titration curves of strong acids and strong bases "flatten out" around pH = 1 and around pH = 13?
- Draw the general titration curve for a strong acid titrated with a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What react
- Choose all the true statements about the equivalence point in an acid-base titration curve. A. It occurs when stoichiometric amounts of acid and base have reacted. B. It occurs when equal volumes of a
- Complete the following for H2SO4. a. Classify the substance as a weak acid, weak base, strong acid, or strong base. b. Based on your classification, predict the approximate pH of a solution containing the substance. c. Based on your classification, predic
- True or false? In the titration of a strong acid with a weak base, the solution is buffered only after the equivalence point.
- 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): 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.
- When a strong acid is titrated with a strong base, the pH at the end point: a. is greater than 7.0. b. is equal to 7.0. c. is less than 7.0. d. is equal to the pKa of the acid. e. is equal to 14.0 - pKb, where pKb is that of the base.
- 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
- List the species present in solution during titration of a strong acid and a strong base: Equivalence point
- List the species present in solution during titration of a strong acid and a strong base: At the half-equivalence point.
- 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
- When a strong acid is titrated with a weak base, the pH at the equivalence point: A. is greater than 7.0. B. is equal to 7.0. C. is less than 7.0. D. is equal to the pKa of the conjugate acid. E. is equal to the pKb of the base.
- Classify the acid and base as either a strong acid (SA), weak acid (WA), a strong base (SB), or weak base (WB): KOH.
- Complete the following for HF. a. Classify the substance as a weak acid, weak base, strong acid, or strong base. b. Based on your classification, predict the approximate pH of a solution containing the substance. c. Based on your classification, predict t
- 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?
- 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
- Classify each of the following as a strong acid, a weak acid, a strong base, or a weak base. a. HCl b. HCOOH c. NaOH d. CH3NH2
- 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)
- What is acid base titration? What is alkalimetry and acidimetry? Discuss the methods in acid base titration, titration of weak acid and base.
- An indicator with a value of PKln is not suitable for the titration of a weak base versus a strong acid. Explain.
- 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.
- Distinguish between the following pairs of terms as they pertain to this experiment. a. monoprotic and diprotic acids b. equivalence point and end point of a titration c. half-equivalence point and
- True or false? In the titration of a strong acid with a weak base, the equivalence point would be less than pH = 7.0.
- Answer the following questions for a titration of ammonium hydroxide (weak base) with nitric acid solution (in buret). i. Sketch the titration curve (make sure to label the axes). ii. At the equivalen
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) CH_3NH_2 (b) HCIO_4
- Classify the acid-base properties of 1.0 M ammonia. a. Strong acid b. Weak acid c. Strong base d. Weak base Which of the following compounds is not an Arrhenius acid? a. CH3CO2H b. CH3NH2 c. H
- True or false? In the titration of a strong acid with a weak base, only water and an acidic salt are present at the equivalence point.
- A good buffer generally contains relatively equal concentrations of a weak acid and its conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acid-conjugate base or weak base-conjugate acid pair to
- 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.
- The pH meter was mistakenly calibrated to be 1.0 pH unit higher than the buffer. a. Will this miscalibration result in a reported molar concentration of the weak acid being too high, too low, or unaffected? b. Is the determined pKa of the weak acid too
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. A) HBr B) HI C) CH_3COOH D) HCN E) KOH F) Ca(OH)_2 G) CH_3NH_2 H) HCIO_4 I) H_2SO_4 J) HCOOH
- Assume that 0.10 M solutions of both acids are titrated with NaOH. At the end point of the titration the acids are completely converted to their conjugate bases. Which solution will have the highest p
- What is the shape of a titration curve if salts of strong and weak acids or bases (sodium acetate, potassium carbonate) are titrated?
- Classify each of the following as a strong acid, a weak acid, a strong base, or a weak base. a. HNO3 b. LiOH c. H2CO3 d. C5H5N
- Classify HClO as a strong base, weak base, strong acid, or weak acid, and then answer the following question. What is the pH of a 0.07 M HClO(aq) solution? a. 1.2 b. 8.7 c. 4.3 d. 9.7 e. 5.3
- Why was phenolphthalein a good indicator to use for determining the equivalence point between the unknown weak acid and strong base?
- 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
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) HBr (b) HI
- Consider the following data on some weak acids and weak bases: Use this data to rank the following solutions in order of increasing pH. A) 0.1 M KNO_2 B) 0.1 M CH_3NH_3Br C) 0.1 M NaF D) 0.1 M C_6H_5
- Classify NaOH as one of the following. a. weak acid b. weak base c. strong acid d. strong base
- Consider a generic buffer solution made of a weak-acid (HA) and conjugate-base (A-) solutions. Are the buffer capacities of that buffer with respect to added acid and base equal or different?
- 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
- 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
- Consider the following hypothetical acid-base reaction A(aq) + B(aq) ↔ C(aq) + D(aq) where : A : weaker acid B : weaker base C : stronger acid D : stronger base In this case : A. The position of the equilibrium
- List the species present in solution during titration of a weak acid and a strong base: Equivalence Point.
- Classify each of the following as a strong acid, weak acid, strong base, or weak base. a. KOH b. NH3 c. LiOH d. HCl
- Why do titration curves for weak acids show regions in which large additions of base result in very small pH changes, while in other regions small additions of base lead to large pH changes?
- When a weak acid is treated with a strong base, the pH at the equivalence point is always: a. greater than 4 b. less than 7 c. less than 1 d. greater than 7 e. equal to 7
- A weak base is mostly neutral if [____]. a. pH>pKb b. The weak base is less than 50% titrated with hydroxide ion. c. The pKb is less than the pH. d. The pH falls anywhere within the buffering range of the weak base. e. pH measures the same as the pKb.
- 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,
- Differentiate between a weak acid and a strong acid, using pH.
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) H_2SO_4 (b) HCOOH
- 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)?
- 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
- 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
- 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
- 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
- Classify each substance as a strong acid, a strong base, a weak acid, or a weak base. (a) KOH (b) Ca(OH)_2
- 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 HCl as one of the following. a. weak acid b. weak base c. strong acid d. strong base
- In the equilibrium reaction, label the stronger acid, the stronger base, the weaker acid, and the weaker base. Estimate the position of each equilibrium. CH_3CH_2O^- + CH_3C equiv CH rightleftharpoons CH_3CH_2OH+CH_3C equiv C^-
- 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)
- Do strong acid strong base titrations have a buffer region?
- If the pH of the following is (H_3O^+) = 3.0 times 10^{-5} M, indicate if the solution is neutral, acid, basic, high, or low.
- Describe the reaction of a weak acid and a strong base. In general, what will the final pH be when the reaction between equal moles of a weak acid and a strong base is complete?
Explore our homework questions and answers library
Browse
by subject