Titration of 25.0 mL of an unknown concentration H2SO4 solution requires 43.6 mL of 0.0985 M NaOH solution.  What is the concentration of the H2SO4 solution (in M)?  To receive full credit (2 pts for answer and 2 pts for showing work), submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL

What is the pH of a solution with a H+ hydrogen ion concentration of 2.44x 10-5 M?

Balance the chemical equation given below, and determine the number of milliliters of 0.150 M phosphoric acid required to neutralize 45.00 mL of 0.0850 M magnesium hydroxide.   ________ Mg(OH)2(aq) + ________ H3PO4(aq) → ________ Mg3(PO4)2(s) + ________ H2O(l) To receive full credit (2 pts for answer and 2 pts for showing work), submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL

The half-life decreases with time for the reaction aA =>bB , which is: 

How can you find the oxidation number of an ion?

Which of the following is a balanced molecular equation describing the titration of a weak acid with a strong base? 

The half-life increases with time for the reaction aA =>bB, which is: 

What is an equivalence point in titration weak base with the strong acid?

 In a redox reaction, what is oxidation?

What volume in liters of 0.125 M H2SO4 is required to neutralize a solution prepared by dissolving 12.5 g of KOH in 250 mL of water?      To receive full credit (2 pts for answer and 2 pts for showing work), submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL