18. What is the pH at the equivalence point when a 30.0 mL sample of 0.100 M aqueous formic acid (HCO;H) is titrated with 0.200 M aqueous potassium hydroxide? (K. of HCO;H = 1.8 x 104) a. 8.28 b. 10.26 c. 5.72 d. 2.46 e. None of these
18. What is the pH at the equivalence point when a 30.0 mL sample of 0.100 M aqueous formic acid (HCO;H) is titrated with 0.200 M aqueous potassium hydroxide? (K. of HCO;H = 1.8 x 104) a. 8.28 b. 10.26 c. 5.72 d. 2.46 e. None of these
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![18. What is the pH at the equivalence point when a 30.0 mL sample of 0.100 M aqueous
formic acid (HCO2H) is titrated with 0.200 M aqueous potassium hydroxide? (K. of HCO,H =
1.8 x 104)
a. 8.28
b. 10.26
C. 5.72
d. 2.46
e. None of these
19. What is the molar solubility of solid iron(III) hydroxide, Fe(OH)3, in a solution that is
buffered to a pH of 2.50 at 25 °C? The Kap of Fe(OH)s is 6.3 x 10-38 at 25 °C.
a. 6.9 x 10-28 mol/L
b. 1.3 x 10-13 mol/L
c. 2.0 x 10 mol/L
d. 2.0 x 10-28 mol/L
e. 5.0 x 10 mol/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc9404307-c815-4f92-bb95-dfbb13e42d62%2F63e4c471-0acc-4a8e-850e-70b8f1b180aa%2Fhqjrn1b_processed.png&w=3840&q=75)
Transcribed Image Text:18. What is the pH at the equivalence point when a 30.0 mL sample of 0.100 M aqueous
formic acid (HCO2H) is titrated with 0.200 M aqueous potassium hydroxide? (K. of HCO,H =
1.8 x 104)
a. 8.28
b. 10.26
C. 5.72
d. 2.46
e. None of these
19. What is the molar solubility of solid iron(III) hydroxide, Fe(OH)3, in a solution that is
buffered to a pH of 2.50 at 25 °C? The Kap of Fe(OH)s is 6.3 x 10-38 at 25 °C.
a. 6.9 x 10-28 mol/L
b. 1.3 x 10-13 mol/L
c. 2.0 x 10 mol/L
d. 2.0 x 10-28 mol/L
e. 5.0 x 10 mol/L
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Step 1 Write the balanced chemical equation.
VIEWStep 2 Calculate the volume of potassium hydroxide required to reach equivalnce point
VIEWStep 3 Calculate the concentration of species remain at equivalence point
VIEWStep 4 Set up the equilibrium chart
VIEWStep 5 Calculate the Kb and set up the equation for Kb .
VIEWStep 6 Calculate pH
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