A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H2S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H2S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Answer Choices: Cd2+, Ni2+,Cr3+,Bi3+,Ag+,Ca2+,Mg2+,Pb2+,Hg22+,Mn2+,Sn2+,Li+,Hg2+

10.00 mL of 0.200 M formic acid is titrated with 0.100 M sodium hydroxide. Write a balanced equation for the reaction of the acid and base indicated. Determine the volume of titrant added at the equivalence point. SHOW ALL WORK! Determine the pH of the solution at the equivalence point (HINT: Consider the products of the reaction. One of the products should be a salt having an ion which will undergo hydrolysis.Determine the concentration of this ion, and write an equation showing the reaction of the ion with water. Then, use an inital, change, final chart in order to work the problem. Using the pH at the equivalence point as a guide, sketch an approximate titration curve for the titration described in the option

A solution is made by combining 10.0 mL of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. Calculate the pH of the solution.

2. After dissolving the KHP with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 sec and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared! a) What happened? b) What can the student do to correct for this erTor and salvage this trial? How should the data sheet be modified to reflect this correction? 3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red! a) What happened? b) What can the student do to correct for this error and salvage this trial? How should the data sheet…