One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chande anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. ml. sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl₂(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂), (aq) The chemist adds 52.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitats. He finds he has collected 2.7 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Round your answer to 2 sighficant digits. mg X G C

Solid nickel(II) acetate is slowly added to 75.0 mL of a 0.0349 M potassium hydroxide solution. The concentration of nickel ion required to just initiate precipitation is  M.

The solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp.       See Periodic Table If only 0.238 g of Ca(OH)2 dissolves in enough water to give 0.243 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?

[References] Use the References to access important values if needed for this question. The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+(aq) + 21(aq) PbI2(s) A student finds that 16.64 mL of 0.5820 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? Submit Answer Try Another Version 1 item attempt remaining ot ot pt pt pt Previous Next ail 6,290 10 15 MAY étv W X 280

A 1.00 gram sample of anhydrous cerium sulfate was dissolved in water. Barium nitrate solution was then added until no further precipitation occurred. The precipitate was filtered from the solution then dried and was found to weigh 1.41 g. Determine the formula of the cerium sulfate. Encom calt is hydrated

b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.

4. Using the solublity chart we can see that compound is soluble KNO3 PBCI Ca(OH)2 Agl

Mercury as an amalgam with copper, silver, and tin is used fro fillings in teeth and in the production of chlorine. Soluble mercury compounds can be toxic and must be removed from wastewater. Aqueous mercury (II) nitrate is a toxic compound formed in wastewater and must be removed. To remove this compound, an aqueous sodium sulfide (Na2S) solution is added to wastewater to form a solid mercury (II) sulfide  (HgS) precipitate and aqueous sodium nitrate in solution. From the analysis, 0.051 L of 0.010 M mercury (II) nitrate was reacted with 0.020 L of 0.10 M sodium sulfide. Write a balance equation for this chemical reaction. Determine the limiting reactant. How many grams of mercury (II) sulfide form? How many grams of excess reactant remain after the reaction is finished?

If 30.0 g of LiOH is added to 0.650 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction?    a) Write a balanced equation. Identify a precipitate. Include states of matter.  b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up.  c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up.  d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.

Some compounds are soluble in water and some compounds are insoluble in water. For each compound below determine if the compound if soluble or insoluble in water. * Soluble Insoluble Mg(NO:): Agcl LIOH Mg:(PO.):