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3. Which of the following represents the balanced equation for the reaction described in #2?

3. Which of the following represents the balanced equation for the reaction described in #2? *

a. 2HCl + NaOH = 2H2O + NaCl
b. HCl + NaOH = Na2O + OHCl
c. 2HCl + 2NaOH = 2H2O + 2NaCl
d. HCl + NaOH = H2O + NaCl


4. What is the pH of the solution after the titration is completed? *

a. 0.947
b. 4.00
c. 6.17
d. 7.00


5. If solution A was titrated with 0.80M Ba(OH)2, what volume would be required? *

a. 1.77mL
b. 3.53mL
c. 7.06mL
d. 25.0mL


6. Which of the following represents the balanced equation for the reaction described in #5? *

a. HCl + Ba(OH)2 = BaCl2 + H2O
b. 2HCl + Ba(OH)2 = 2BaCl + H2O
c. HCl + Ba(OH)2 = BaH2 + OHCl
d. 2HCl + Ba(OH)2 = BaCl2 + 2H2O


Use the following for #7 - 8
HS- + NH4+ = H2S + NH3


7. What is the Bronsted-Lowry acid? *

a. HS-
b. NH4+
c. H2S
d. NH3


8. What is the Bronsted-Lowry base? *

a. HS-
b. NH4+
c. H2S
d. NH3


9. In a reaction which would be the conjugate acid for HTe-? *

a. Te2-
b. H2Te
c. HTe-
d. H3Te+


10. What is the pH of a 6.2 x 10-3M H2SO4 solution? *

a. 3.21
b. 2.21
c. 11.79
d. 10.79


11. What is the pOH of a solution with a pH of 12.75? *

a. 2.25
b. 1.25
c. 12.75
d. 14


12. What is the [OH] of a solution with pOH equal to 4.8? *

a. 6.31x10-10
b. 6.31x10-9
c. 1.58x10-4
d. 1.58x10-5


Solution B - Use for #13-15
10.00mL of 0.222M KOH is added to a flask


13. How many milliliters of a 2.5M HCl solution is required to neutralize Solution B? *

a. 0.889mL
b. 112mL
c. 10.0mL
d. Not enough information


14. Which of the following represents the balanced equation for the reaction explained above? *

a. 2HCl + KOH = 2H2O + KCl2
b. HCl + KOH = H2O + KCl
c. HCl + KOH = K2O + OHCl
d. 2HCl + 2KOH = 2H2O + 2KCl


15. What is the pH of the solution after the titration is completed? *

a. 14.00
b. 10.00
c. 8.00

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