Choose the false statement. O The pH of the acetic acid solution at the equivalence point is less than 7.00 O In contrast to strong acids and bases, the shape of the titration curve for a weak acid or a weak base depends on the identity of the acid or the base and the corresponding Ka or Kb. The end point of titration is the point at which the number of moles of base (or acid) added equals the number of moles of acid (or base) originally present in the solution. O The shape of the curve for a titration involving a strong acid and a strong base depends on only the concentrations of the acid and base, not their identities.

Choose the false statement. O The pH of the acetic acid solution at the equivalence point is less than 7.00 O In contrast to strong acids and bases, the shape of the titration curve for a weak acid or a weak base depends on the identity of the acid or the base and the corresponding Ka or Kb. The end point of titration is the point at which the number of moles of base (or acid) added equals the number of moles of acid (or base) originally present in the solution. O The shape of the curve for a titration involving a strong acid and a strong base depends on only the concentrations of the acid and base, not their identities.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The K of a certain indicator is 7× 107. The color of HIn is green and that of Inis red. A few drops of the indicator are added to an HC1 solution, which is then titrated against an NaOH solution. Over which pH range will the indicator change color? Select the single best answer. 7.2 to 9.2 ○ 4.2 to 6.2 O 6.2 to 8.2 O 5.2 to 7.2 O 3.2 to 5.2
Select all that are true for a titration at the equivalence point: Group of answer choices The number of moles of acid (ie H2SO4) added are the same as the number of moles of base (ie NaOH) added. The number of moles of hydronium ion added are the same as the number of moles of hydroxide ion added. The indicator is selected in order to have a color change when the equivalence point is reached.
A beaker with 195 mLmL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 MM. A student adds 7.70 mLmL of a 0.440 MM HClHCl solution to the beaker. How much will the pH change? The pKapKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.
In a weak base with strong acid titration, which of the following is correct? O the equivalence point pH is less than 7 because only the conjugate acid remains the equivalence point pH is less than 7 because the acid is stronger than the base O the equivalence point pH equals 7 because (H3O*) = [OH'] O the equivalence point pH is greater than 7 because the acid is stronger than the base O the equivalence point pH is greater than 7 because only the conjugate base remains
You have an unknown solution whose initial pH is 2.90. Addition of 10 ml of the titrant increased the pH to 4.15. Adding small-volume increments of the titrant causes the pH to increase very slightly. At equivalence point, the pH of the solution is at 8.70. Abrupt increase in pH to 10.00 was observed when 0.1 ml of titrant was added after equivalence point. Addition of few more drops of the titrant just increase the pH even more with no buffering region. Which among the choices best describes the analyte? The analyte is a strong monoprotic acid. The analyte is a weak monoprotic acid. The analyte is a weak monoprotic base. O The analyte is a weak diprotic acid. O The analyte is a weak diprotic base.
Write the equation for the equilibirum that determines the pH at the following points in the titration curve of a weak acid (HA) being titrated with a strong base (OH) before any base has been added halfway to the equivalence point at the equivalence point
Use the following two titration curves to answer each of the following statements. Select the choice that completes the statement correctly. 14 pH 7 0 Graph A 25 volume of titrant added (mL) In graph A, the end point occurs at a In graph B, the equivalence point occurs at a + 141 pH 7 0 Graph B 25 volume of titrant added (mL)
Part A When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K of HA is 5.66 x 10-7. Express the pH numerically to three decimal places. HA(aq) = H+ (aq) + A-(aq) • View Available Hint(s) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base the base will react with Ht, reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into H+ and A. In both instances, H+] tends to remain constant. added, V AZO The pH of a buffer is calculated by using the Henderson-Hasselbalch pH = equation: pH =…
Chemistry Determine the pH during the titration of 16.5 mL of 0.290 M hydroiodic acid by 8.86×10-2 M barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 13.5 mL of barium hydroxide (3) At the equivalence point (4) After adding 34.6 mL of barium hydroxide.
12.0 10.0 8.0 A pH 6.0 4.0 2.0 0.0 C 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the choices below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.
Need help calculating the bold underlined (pH at equivalence point using an ICE table) In a strong acid-strong base titration, a potassium hydroxide (KOH) solution of an unknown concentration reacts with 0.105 M sulfuric acid (H2SO4) solution. Write the balanced chemical equation for the reaction between KOH and H2SO4 Calculate the concentration (molarity) of the KOH solution, if 23.10 mL of H2SO4 acid solution reacts with 30.00 mL of KOH solution. What is the pH of the solution at the equivalence point?