A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H,S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H,S 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. Definitely present Definitely absent Possibly present Answer Bank Bi3+ Cu2+ Ni2+ Lit Ag+ Sn2+ Pb2+ A13+ Ba2+ Zn2+ Hg?+ Mg²+ Hg3*

What you expect to observe on mixing 6M NH3 with HCl. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?

A 23.1 mL sample of 0.382 M ethylamine, C,H;NH,, is titrated with 0.297 M hydrobromic acid. The pH before the addition of any hydrobromic acid is

A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.500 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. pKa of HNO2 is 3.40 Ka of HNO2 is 4.0E-4 m.w. of HNO2 is 47.01 g/mol pH of the buffer solution is 3.30, so now Calculate the pH of the buffer solution after the addition of 5.00 ml of 2.50 M Ba(OH)₂.

2. Identify those salts that are more soluble in acid than in neutral solution. Explain why. ZNCO3 Ni(OH)2 Agl AIPO4 PbCl2 Hg2Br2 CuS

A 25.00-mL sample of H2C2O4 solution required 43.88 mL of 0.1891 M NaOH solution to titrate it to the equivalence point. Calculate the molarity of the H2C2O4 solution. Use the formula below but remember that there are two H+ molecules in H2C2O4.

A 25.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1372 MM KOHKOH solution. A volume of 40.22 mLmL of KOHKOH was required to reach the equivalence point.

20.4 mL of 0.142 M solution of nitric acid is titrated with 0.192 M NaOH solution.  What is the pH at the equivalence point?

Some contact lens solutions use boric acid buffers to resist pH change. Over what pH range does boricacid have good buffering capacity? Explain. Please help

4. A buffer is prepared containing 1.00 M acetic acid and 1.00 M sodium acetate. What is its pH?