astering.pearson.com.couiseid-12449557&key=504176635134952610222023#/MISSED THIS? Read Section 18.4 (Page); WatchKCV 18.4BConsider the curve shown here for the titration of aweak monoprotic acid with a strong base.Hd14121086.42004080 120 160Volume of base added (mL)The figure shows pH as a function of volume ofbase added. The pH is measured from 0 to 14 onthe y-axis, while the volume of base added ismeasured from 0 to 160 milliliters on the x-axis.The curve of the plot goes up gradually from pH2.3 at 0 milliliters to pH 5.8 at 49 milliliters, nextthe plot goes up steeply to pH 11.8 at 51milliliters, and finally the plot goes up graduallyto pH 12.2 at 160 milliliters.✓ CorrectThe equivalence point is the point in the titration when the number of moles of base is stoichiometrically equal tothe number of moles of acid. The equivalence point is located at the point of inflection in the middle of thetitration curve. For the presented curve, the volume of added base at the equivalence point is 60 mL.Part CAt what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentrationand Ka of the weak acid?Express your answer in milliliters as an integer.V = 0 mLSubmit✓ CorrectAn equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for anaqueous solution of the weak acid. This is true for the initial state of titration, when no base has been added. Thaddition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in a differerway.Part DPrevious AnswersV =At what volume of added base does pH = pKa?Express your answer in milliliters as an integer.IVE ΑΣΦSubmit Request AnswerdPart E Complete previous part(s)?mL

Titration is an analytical method to determine the concentration of a substance. In the titration…

At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and Ka of the weak acid? Express your answer in milliliters as an integer. V = 0 mL Submit Previous Answers Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for an aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been added. T addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in a differe way. ▾ Part D At what volume of added base does pH =pK₁? Express your answer in

At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and Ka of the weak acid? Express your answer in milliliters as an integer. V = 0 mL Submit Previous Answers Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for an aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been added. T addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in a differe way. ▾ Part D At what volume of added base does pH =pK₁? Express your answer in

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak base pyridine is titrated with HCl. (b) Formic acid is titrated with NaOH. (c) Ethylenediamine, a weak diprotic base, is titrated with HCl. Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that o few indicators hove color changes over two different pH ranges.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?