12.0 1 10.0 pH of solution in flask 8.0 Equivalence Point 6.0 4.0 2.0 5 10 15 20 25 30 35 40 45 mL of 0.115 M NAOH added to flask A 50.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. a). What would be the molar mass of the unknown acid if the density of the solution is 1.00g/mL and mass concentration of the acid is 3.00 g/L. Molar Mass = g/mole Please use 3 sig figs for the ans, just provide the value no need for units). (Note: use the plot to estimate the volume needed to reach the equivalence point) ɔ). What would be the pKa of the unknown acid? pka = (please use two sig igs for the ans) (use the plot above to estimate) c). What would be the concentration of the HA and conjugate A- when 9.00 mL of 0.115 M NaOH is used for the titration. (please use 3 sig figs for the ans and just imput the units) (Hint: use the mmoles of HA estimated from part a) O OO O

12.0 1 10.0 pH of solution in flask 8.0 Equivalence Point 6.0 4.0 2.0 5 10 15 20 25 30 35 40 45 mL of 0.115 M NAOH added to flask A 50.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. a). What would be the molar mass of the unknown acid if the density of the solution is 1.00g/mL and mass concentration of the acid is 3.00 g/L. Molar Mass = g/mole Please use 3 sig figs for the ans, just provide the value no need for units). (Note: use the plot to estimate the volume needed to reach the equivalence point) ɔ). What would be the pKa of the unknown acid? pka = (please use two sig igs for the ans) (use the plot above to estimate) c). What would be the concentration of the HA and conjugate A- when 9.00 mL of 0.115 M NaOH is used for the titration. (please use 3 sig figs for the ans and just imput the units) (Hint: use the mmoles of HA estimated from part a) O OO O

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl. Kb for CN is 2.0 105. Calculate the pH of the solution: a prior to the start of the titration; b after the addition of 15.0 mL of 0.200 M HCl; c at the equivalence point; d after the addition of 30.0 mL of 0.200 M HCl.
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.
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
A buffer solution is composed of 1.360 g of KH2PO4 and 5.677 g of Na2HPO4. (a) What is the pH of the buffer solution? (b) What mass of KH2PO4 must be added to decrease the buffer solution pH by 0.50 unit from the value calculated in part (a)?
K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic acid with 46.1 mL of 0.182 M sodium acetate. Calculate the pH of this solution at 25C after the addition of 5.82 mL of 0.125 M NaOH.
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL b. 50.0 mL c. 100.0 mL d. 150.0 mL e. 200.0 mL f. 250.0 mL
A 65.0-mL sample of 0.010 M Pb(NO3)2 was added to a beaker containing 40.0 mL of 0.035 M KCl. Will a precipitate form?
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.)