A solution of potassium permanganate is standardized using pure As2O3as the primary standard (upon addition of water, As2O3is converted to H3AsO3). A sample of As2O3weighing 0.2248 g requires 44.22 mL of potassium permanganate solution for titration. Calculate the molarity of the potassium permanganate.                                  5H3AsO3 + 2MnO4-+ 6H+→2Mn2++ 5H3AsO4+ 3H2O

Solubility of AgCl is 0.0000123 M. What is the solubility product, Ksp for AgCl?

The initial in the unknown analysis is the addition of 6. M HCl. This results in the formation of a precipitate. The solid precipitate is separate from the liquid solution. The solution could potentially contain K+, Ca2+, and Al3+. Next, 3M NH3 is added to the solution to separate the Al3+. This is a result of the fact that the Al3+ forms the hydroxide, Al(OH)3. But Ca2+ also forms the hydroxide, Ca(OH)2. Why does the Ca(OH)2 not separate out with the Al(OH)3?

Which statement explains why the pH at the stoichiometric point in the titration of a weak acid with a strong base is NOT 7.00 (at 25 °C)? O Strong base still is present at the stoichiometric point. O A basic salt is the primary species present at the stoichiometric point. O At the stoichiometric point, a buffer is present. A neutral salt is the primary species present at the stoichiometric point. An acidic salt is the primary species present at the stoichiometric point.

it took 32.47 mL of 0.123M NaOH to reach the endpoint when titrating a sample containg 0.2372g of unkown tripotic acid. What is the molar mass of the acid?

An unknown solution is titrated with a strong titrant. The pH at the equivalence point is 5.7. What was the unknown solute? O A weak base O A weak acid O A strong base O A strong acid

R456

Calculate the amount of precipitate when excess CO2 is bbbled through a solution containing 0.205 mol of Ba(OH)2 according to the equation:  Ba(OH)2 + CO2 --> BaCO3 (MM=197.4g) +H2O (MM=18.02)

Please answer questions 3a&b based on the information in question 2.

To determine buffer capacity, 40.0mL of solution are titrated with 0.13M NaOH. How many moles of acid were added? initial V- 2.21mL final V- 20.86mL initial pH- 4.32 final pH- 5.61