Problem on acid bases equilibria

Question

Assignment:

Question 1. The solvent cation in liquid ethanol, CH₃CH₂OH, is

a) CH₃CH₂O^-         b) H⁺     c) CH₃CH₂OH⁺     d) CH₃CH₂OH₂⁺     e) CH₃CH₂OH^-    

Question 2. Fill in the blanks.

a) The normality of 0.20M solution of H₂SO₄ ________________________

b) The following reaction is best classified as an Arrhenius, Bronsted or Lewis acid base reaction?   SiF₄  +  2F^-    ---→  SiF₆^2-       _________________

c) The conjugate base of H₂PO₃^-     _________________________

d) The conjugate acid of AsH₃          _________________________

Question 3. Identify the correct answer in each case.

a) The stronger acid, H₃SbO₃ or H₃AsO₃ ?    _____________________

b) The stronger base, GeH₄ or SiH₄ ?   ________________________

c) The stronger acid, H₂TeO₃ or H₂ TeO₄ ?  _______________________

d) The stronger base, Pd (OH)₂ or Sn (OH)₂ ?  _________________________

e) The stronger conjugate acid, the conjugate acid of Cl04- or the conjugate acid of MnO4-?  ____________________________

f) The amphiprotic species in the following equation 

H₂CO₃   ←--→  H+   +  HCO₃^-  _____________________

g) The conjugate base in the Bronsted  -  Lowry reaction 
HBr  +  NH₃  ←-→  NH₄⁺  +  Br-  _______________________

h) The Lewis base in the reaction 
Cu(NO₃)₂  +  4H2O  ←-→  Cu(H₂O)₄²⁺  +  2NO₃^-  ____________________

Question 4. In a 0.90M solution of the weak acid HA, the acid is 11% ionized.  What is the ionization constant, Ka, for the acid?  (Show work)

Question 5. Ka for HC₂H₃O₂ is 1.8 x 10-5.  To adjust the pH value of one liter of 0.020M acetic acid to pH  =  6.0, one must add how many grams of KC₂H₃O₂?  (Show work)

Question 6. Would the pH of a 0.1M solution of Cs₂SO₃ be less than, greater than, or equal to 7.0?  (Show work)

Question 7.  In the titration of HClO₄ with LiOH, 50.0mL of 0.35OM LiOH is added to 30.0mL of 0.400M HClO₄.  What is the pH at this point in the titration?  (Show work)

Question 8. What is the pH of a buffer made by mixing equal volumes of 0.10M NH₃ and 0.10M NH₄Cl?   Kb for NH₃  =  1.8 x 10^-5
(Show work)

Question 9. What is the pH after this same solution is made 0.020M in KOH?  (Show work)
 
Question 10. Below a pH of 4.8, an indicator, exists in the blue acid form, HIn.  At pH 4.8 about 10% of the indicator exists in the rose base form.  What is the ionization constant of this indicator?  (Show work)

Provide complete and step by step solution for the question and show calculations and use formulas.