20.0-mL sample of 0.123 M diprotic acid (H2A) solution is titrated with 0.1013 M KOH. The acid ionization constants for...
20.0-mL sample of 0.123 M diprotic acid (H2A) solution is titrated with 0.1013 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10.
Part A:
At what added volume of base does the first equivalence point occur?
Part B:
At what added volume of base does the second equivalence point occur?
Homework Answers
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20.0-mL sample of 0.123 M diprotic acid (H2A) solution is titrated with 0.1013 M KOH. The acid ionization constants for...
18.0-mL sample of 0.126 M diprotic acid (H2A) solution is titrated with 0.1040 M KOH. The...
18.0-mL sample of 0.126 M diprotic acid (H2A) solution is titrated with 0.1040 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. Part A At what added volume of base does the first equivalence point occur? Part B At what added volume of base does the second equivalence point occur?
22.0-mL sample of 0.122 M diprotic acid (H2A) solution is titrated with 0.1016 M KOH. The...
22.0-mL sample of 0.122 M diprotic acid (H2A) solution is titrated with 0.1016 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. A. At what added volume of base does the first equivalence point occur? ____ mL B. At what added volume of base does the second equivalence point occur? _____ mL 12
Review I Constants I Periodic Table 20.0-mL sample of 0.123 M diprotic acid (H2 A) solution...
Review I Constants I Periodic Table 20.0-mL sample of 0.123 M diprotic acid (H2 A) solution is titrated with 0.1021 M KOH. The acid ionization constants for the acid are Part A Ka1 5.2 x 10 and Ka, =3.4 x 10-10. At what added volume of base does the first equivalence point occur? η ΑΣφ V= 21.7 mL Previous Answers Request Answer Submit X Incorrect; Try Again; 14 attempts remaining Part B At what added volume of base does the...
Part A.) Consider that you are titrating a diprotic weak base "B" which has pKb1=4 and...
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Given a diprotic acid, H2A, with two ionization constants of Ka1 = 3.5× 10–4 and Ka2...
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6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2?
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
<Post-Lecture Ch 17 Exercise 17.78 19 of 19 R. Review l Constants l Periodic Table Part A 19.0-mL sample of 0.123 M diprotic acid (H A) solution is itrated with 0.1012 MKOH, The acid ionization constants for At what added volurne of base does the first equivalence point occur? the acid are Ka 5.2 x 10-5 and K3.4 x 10-10 V- mL Submit Requesl Answer Part B At what added volume of base does the second equivalence point occur? mL...
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od luck! Question 15 4 pts A 20.0 mL sample of 0.115M H2SO3 is titrated with...
od luck! Question 15 4 pts A 20.0 mL sample of 0.115M H2SO3 is titrated with 0.1014 M KOH. At what volume (of added base) does the second equivalence point occur at? 50.0 mL 40.0 mL 22.7 ml 45.4 mL 20.0 mL Previous Next
Review I Constants I Periodic Table 20.0-mL sample of 0.123 M diprotic acid (H2 A) solution is titrated with 0.1021 M KOH. The acid ionization constants for the acid are Part A Ka1 5.2 x 10 and Ka, =3.4 x 10-10. At what added volume of base does the first equivalence point occur? η ΑΣφ V= 21.7 mL Previous Answers Request Answer Submit X Incorrect; Try Again; 14 attempts remaining Part B At what added volume of base does the...
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6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
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od luck! Question 15 4 pts A 20.0 mL sample of 0.115M H2SO3 is titrated with 0.1014 M KOH. At what volume (of added base) does the second equivalence point occur at? 50.0 mL 40.0 mL 22.7 ml 45.4 mL 20.0 mL Previous Next
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> So what were the Pka and PKa2 values for??
miguelangelseguragiraldo Sat, Nov 13, 2021 11:34 AM