od luck! Question 15 4 pts A 20.0 mL sample of 0.115M H2SO3 is titrated with...
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?
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...
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
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?
A.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 5.00 mL of 0.0960 M KOH. What is the solution pH to the nearest hundredths place? pKa1 = 6.35 and pKa2 = 10.33. B.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 0.0960 M KOH. How many mL of titrant are required to reach the first equivalence point? C. )A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated...
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with 0.200 M KOH. Calculate: a. the pH after adding 10.00 mL of KOH b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of KOH d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of KOH
1. To a flask is added 20.0 mL of 0.200 M NaHC.O. It is then titrated it with 0.100 M NaOH. Calculate the PM or the solution in the flask (a) before any base is added (bl at the quarter equivalence point, the half-equivalence point, (d) the equivalence point, and (e) at a point past the equivalence point. (20 pts.) MIVI = Mr. Ve
1. A 30.00 mL sample of 0.400 M HNO3 is titrated with 0.600 M KOH. What is the balanced neutralization chemical reaction? What volume of base (in mL) must be added to reach the equivalence point? Is the pH of the equivalence point acidic, basic, or neutral?
A 40.0 mL sample of a mixture of HCl and H3PO4 was titrated with 0.100 MNaOH. The first equivalence point was reached after 88.0 mL of base, and the second equivalence point was reached after 126.4 mL of base.
ration 46. A 30.0-ml sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: OmL, 5 mL, 10 mL, equivalence point, one-half equivalence point. 20 mL, 25 mL. Use your calculations to make a sketch of the titration curve. ed by