Choose a reagent that will separate the cations in the following pair: Mn2+ and Fe³+ NaOH, 1M NaOCI and 6M NH3 6M Acetic acid 6M HNO3 NaOH

NH3(aq)+H2O⇄NH4+(aq) + OH-(aq) What happens to this equlibria in regards to Le Chateliers principle when HCL was added? This caused the indicator and solution to turn from pink to clear.

Determin the pOH for a 1650 mL solution of 3.00 g of Mg(OH)2

Calculate the pH of a titration between 15.0 mL of 0.10 M HCl and 8.0 mL of 0.20 M NaOH at 25°C.

What is the hydronium ion concentration of a 0.500 M acetic acid solution with Ka=1.8x10^-5?

Write net ionic equations to explain the acidity or basicity of the various salts listed in question 60.  A) FeCl3 B) BaI2 C) NH4NO2 D) Na2HPO4 E) K3PO4

8.)

What is the concentration of hypochorite ion if 20.00 mL of bleach requires 32 mL of 0.500 M HCl to reach the equivalence point?

In an acid base titration between Carbonic acid and Sodium hydroxide, which of the following salts is not formed? Na2CO3 NaHCO3 NaH2CO3

What is the pH of an aqueous solution containing 75.0 mL of a 0.15M HNO2 solution and 45.0 mL of a .25M KNO2? What is the pH of this solution after 10.0 mL of a 0.20M solution of KOH is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)?