12.0 10.0 pH of solution in flask 80 Equivalence Point 6.0 40 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). b). What would be the pka of the unknown acid? pKa = (please use two sig figs for the ans) 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: you can neglect the x. Concentration of HA = M Concentration of A- = O OO0

12.0 10.0 pH of solution in flask 80 Equivalence Point 6.0 40 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). b). What would be the pka of the unknown acid? pKa = (please use two sig figs for the ans) 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: you can neglect the x. Concentration of HA = M Concentration of A- = O OO0

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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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Plz answer

12.0
10.0
pH of
8.0
Equivalence
Point
solution
6.0
in flask
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).
b). What would be the pKa of the unknown acid? pka =
(please use two sig figs
for the ans)
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: you can neglect
the x.
Concentration of HA =
M
Concentration of A- =

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