The strong acid H2SeO4 will completely ionize in water, however the conjugate base can then act...
The strong acid H2SeO4 will completely ionize in water, however the conjugate base can then act as a acid an ionize further.
The second Ka, Ka2 for HSeO4 is 1.2 x 10-2. This second Ka is not insignificant, being stronger than many other weak acids.
A. Calculate the [H3O+] for a solution of 0.150 M H2SeO4.
B. Using the value calculated above, calculate the value of [H3O+] for both ionizations of the acid. Grading will be based on the follow:
Write the chemical equation for the second ionization of the acid, include phase symbols and any charges.
Determine if the S.A. is valid, show your work.
Construct the ICE table.
Solve for [H3O+]
NOTE: Calculation A should be easy as it's a strong acid. For B, write the chemical equation for the second ionization, construct the ICE table, check the S.A., if valid....good, if not, well, you know what to do. Solve for the [H3O+]. Show every step, if using a program indicate your values for a, b, & c. Express answer to the correct SF's.
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The strong acid H2SeO4 will completely
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Thank you!!
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I know some of the measured pH values are a little off due to error in...
I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
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A thorough explanation would sure be appreciated!!!!
Thank you!!
Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
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Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
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I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
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