## pH Reactions

- A solution is prepared by mixing 50 mL of 0.1 M NH
_{3}with 50 mL of 0.1 M NH_{4}Cl.- Calculate the pH of this solution.
- 10 mL of 0.1 M HCl is now added to this solution. Write an equation for the reaction that occurs and then calculate the pH of the solution after the HCl has been added.
- Calculate the pH of a 0.1 M HCl solution.

- 5.9 g of trimethyl amine [ (CH
_{3})_{3}N ] is added to enough water to make 1.0 L of solution. 50.0 mL of this solution is placed in an Erlenmeyer flask and is then titrated with 0.100 M HCl.- Calculate the pH of the solution in the Erlenmeyer flask before the titration is started.
- Calculate the pH of the solution at the midpoint of the titration.
- Calculate the pH of the solution at the equivalence point.
- What indicator would you choose for the titration?

- Carefully explain why a solution of aluminum nitrate is acidic. Be sure to use equations.
- Complete the following equations and tell whether K>1 or K<1 or K=1.
- BaCl
_{2}+ Na_{2}CO_{3}→ - CaCl
_{2}+ Fe(NO_{3})_{2}→ - CH
_{3}COOH + SO_{4}^{-2}→ - H
_{2}SO_{3}+ NH_{3}→ - H
_{2}O + H_{3}O^{+}→ - ZnCO
_{3}+ Cd(NO_{3})_{2}→

- BaCl
- Show how the hydrogen carbonate ion can act as both an acid and a base in water by writing appropriate equations using full electron-dot formulas.
- Consider ortho-fluoro aniline (o-FC
_{6}H_{4}NH_{2}).- Give an electron-dot formula for this compound and indicate with an arrow which atoms can accept a proton. Circle the atom that actually does accept a proton from water.
- Determine whether o-FC
_{6}H_{4}NH_{2}is a stronger or weaker base than aniline itself (C_{6}H_{5}NH_{2}) and explain why this is the case. - Calculate the pH of a 0.1 M solution of o-FC
_{6}H_{4}NH_{2}. - Draw the structural formula of the conjugate acid of o-FC
_{6}H_{4}NH_{2}. - Calculate the pH of a 0.010 M solution of the conjugate acid of o-FC
_{6}H_{4}NH_{2}.

- Determine whether each of the following 1 M solutions is acidic, basic, or neutral.
- NaHS
- NaBr
- NH
_{4}Ac (remember Ac = acetate) - KNO
_{2} - KHSO
_{3} - NaH
_{2}PO_{4}

- 6.00 g acetic acid and 10.00 g sodium acetate are dissolved in enough water to make 1 L of solution.
- What is the pH of the solution?
- If 5 mL of 0.1 M HCl are added to the solution, what is the new pH?
- If instead 5 mL of 1.0 M KOH are added to the original solution, what is the new pH?

- Calculate the pH at the beginning, at the midpoint, and at the equaivalence point for the titration also choose an indicator:
- of 50 mL of 0.1M HCl with 0.1 M NaOH
- of 50 mL of 0.1 M CF
_{3}COOH with 0.1 M NaOH - 50 mL of 0.1 M triethylamine with 0.1 M HCl

- Complete the equation for each of the following reactions and determine the equilibrium constant (that is, give a numerical value) for each reaction:
- SO
_{3}^{-2}+ H_{2}O → - NH
_{3}+ H_{3}O^{+}→

- SO