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Consider the titration of 20 mL of 0.3 M formic acid, HCOOH, Ka = 1.78 x 10−4.  What is the pH of the solution after adding 20 mL of 0.25 M NaOH?

Consider the titration of 50.0 mL of 0.15 M HClO4 with KOH.   What is the pH after 40.0 mL of 0.25 M KOH has been added?

A solution prepared in the lab contains 3.5 × 10⁻3 M Sr²⁺ and 0.0030 M F⁻. Will a precipitate of SrF2 form in this solution? Hint:  Ksp of SrF₂ is 4.3 × 10⁻⁹

Which of the following titrations would produce a solution with an acidic pH at the equivalence point?

What happens when a small amount of HCl is added to a buffer solution containing NH₃ and NH₄Cl?

A 1.00 L buffer solution is made with 0.500 mol of ammonia (NH₃) and 0.600 mol of ammonium chloride (NH₄Cl).The pKa of NH₄⁺ is 9.25. What is the pH of the solution after the addition of 0.100 mol of HCl. Hint:  Assume no change in volume upon addition of HCl

A solution contains 2.0 × 10⁻³ M Pb²⁺ and 1.2 × 10⁻³ M I⁻.  Will a precipitate of PbI₂ form in this solution? Hint:  Ksp of PbI₂ = 8.5 × 10⁻⁹

A solution prepared in the lab contains 3.5 × 10⁻⁴ M Sr²⁺ and 0.0010 M F⁻. Will a precipitate of SrF2 form in this solution? Hint:  Ksp of SrF₂ is 4.3 × 10⁻⁹

What is the molar solubility (in M) of magnesium hydroxide (Mg(OH)₂) in water? Hint: Ksp of Mg(OH)₂ = 1.5 × 10⁻11

According to the additional assigned reading What does CPS stand for and what is its purpose?