Chromium ion concentration for saturated solution

Question

Assignment:

Q1.What is the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH₃CO₂H and 0.100 M NaCH₃CO₂? The Ka for acetic acid is 1.8 x 10 ^-5.

Q2. What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄ 2- and the Ka₂= 6.2 x 10 ^-8.

Q3. Calculate the molar solubility of thallium chloride in 0.20M NaCl at 25 degrees Celcius. Ksp for TICl is 1.7 x 10 ^-4.

Q4. What volume of 0.500 M HNO₃ is needed to titrate 60.00 mL of 0.500 M Ca(OH)₂ to the equivalence point?

Q5. What is the chromium ion concentration for a saturated solution of Cr(OH)₃ if the Ksp for Cr(OH)₃ is 6.7 x 10 ^-31?

Q6. What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? Ksp for Mg(OH)₂ is 5.6 x 10^-12.

Q7. What is the pH of a solution made by mixing 15.00mL of 0.10M acetic acid with 15.00mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka=1.8 x 10^-5 for CH₃CO₂H.

Q8. Formic acid (HCO₂H, Ka=1.8 x 10 raised to the -4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00mL of the formic acid solution requires 49.80mL of 0.0567 M NaOH to reach the equivalence point?

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