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How can you downplay your authority over others in presenting a command?

REMINDER:  For review purposes, make quick notes of terms and facts, using pen and paper only. You do not have time to write full questions and answers. If you attempt to take pictures of the screen and/or do screen captures, it will cause you to have no grade for the quiz and a grade reduction on Test 4. REMINDER 2:  This, along with notes you make from reading and from the PowerPoint is your only review for Test 4. This quiz and review is designed to help you have review materials from these chapters. Reminder 3:  The following provide some answers following some questions, but not all. Answer ‘True’ and move forward.

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

Consider the titration of 20 mL of 0.30 M butanoic acid, HC4H7O2, Ka = 1.5 x 10−5.  What is the pH of the solution after adding 20 mL of 0.25 M NaOH?

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