17.46) Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl.
Calculate the Molar concentration of the lactate ion C3H5O3- , in the resulting solution In the final solution, 0.50 M HC3H5O3 (100 mL / 200 mL) = 0.25 M HC3H5O3 0.10 M HCl (100 mL / 200 mL) = 0.050 M H+ HC3H5O3 (aq) H+ (aq) + C3H5O3- (aq)
b) 80 Ml of 0.1 M HCl (aq) mixed with 50 mL of 0.1 M NaOH (aq). c) 50 Ml of 0.1 M HC2H3O2 (aq) mixed with 50 mL of 0.1 M NaOH (aq). d) 50 Ml of 0.1 M HC2H3O2 (aq) mixed with 80 mL of 0.1 M NaOH (aq).
Will a precipitate of calcium sulfate (Ksp = 2.4 x 10-5) form when 50.0 mL of 0.00150 M calcium chloride and 25.0 mL of 0.0100 M sodium sulfate are mixed? Why or why not? 5. Complex-Ion Equilibria.
Find [H+] in a solution prepared by dissolving 1.50 g of Ca(OH)2 in 600 mL of water and diluting the solution to a final volume of 800 mL. 4. Find the pH when 45.0 mL of 0.250 M NaOH (aq) is added to 35.0 mL of 0.200M HCl (aq). 5.
498204 Strong Acid, Strong base Titration Calculate the pH of the solution when 0.1 M sodium hydroxide (NaOH) is titrated with a 25.0 mL hydrochloric acid (HCl) at the following stages of the titration.
The equilibrium is represented by the equation below MgF2(s) ---> Mg2+ (aq) + 2F- (aq) A) write the expression for the solubility product , Ksp , and calculate its value at 18C B) predict whether a precipitate of MgF2 will form when 100.0
of HCOOH. 5- Ammonia, NH 3 , is a weak base with a K b value of 1.8×10 −5 .What is the percent ionization of ammonia at this concentration?
248368 Preparing a Buffer Solution Calculate the mass (g) of pure Na3AsO4 (s) and volume (mL) of 1.50 M HCl that are required to make 100.0 mL of a buffer solution at a pH of 6.80 and an H2AsO4-(aq) concentration of 0.100 M.
[HOCL ] Hypochlorous acid , HOCl , is a weak acid in water with the above Ka A) write a chemical equation showing how HOCl behaves as an acid in water B) calculate the pH of a 0.175 M solution of HOCl C) write the net ionic equation for