4. A student has an unknown solution. She knows that the solution could be NaCl(aq), Mg(NO3)2(aq) or Ca(NO3)2. When a solution of silver nitrate was added to her unknown, there was no reaction. When a solution of sodium sulfate was added to her unknown, a white precipitate appeared. What is her solution? Explain your reasoning and write the molecular equation for the reaction that produced the precipitate.

In the laboratory you are given the task of separating Ca2+ and Co2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the lons. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Submit Answer Retry Entire Group Y or N Reagent Formula of Precipitate if YES 1. K₂S 2. M 3. NaOH NaBr 3 more group attempts remaining A solution contains 8.82x10-3 M lead acetate and 7.60x10-3 M barium nitrate. Solid potassium fluoride is added slowly to this mixture. What is the concentration of lead ion when barium ion begins to precipitate? [Pb2+] = A solution contains 5.18x103 M ammonium chloride and 1.47x10-2 M sodium sulfate. Solid lead acetate is added slowly to this mixture. What is the concentration of sulfate ion when chloride ion begins to precipitate? [sulfate] = M

In the laboratory you are given the task of separating Ag+ and Co2+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 NaOH   2. fill in the blank 3 Na2CO3   3. fill in the blank 5 NaI

In the laboratory you are given the task of separating Ba 2+ and Co2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. Na2CO3 2. K2SO4 3. NaI

You have a solution that is either CuCl2 (aq) or Cu(NO3)2 (aq).  You add some KOH (aq) and a solid precipitate is formed.  Does this test allow you to determine the contents of your solution?    If so, how?  If not, what other test could you perform that would give you the information that you need?  Please explain.

In the laboratory you are given the task of separating Ba²+ and Fe²+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. HBr 2. 3. K₂SO4 K₂CO3

In the laboratory you are given the task of separating Ba2+ and Zn2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 Na2CO3 2. fill in the blank 3 Na2SO4 3. fill in the blank NaBr

Use the solubility rules to determine if a precipitate forms in each of the following reactions. If so, then write the balanced chemical equation and the net ionic equation. IF NO PRECIPITATE FORMS THEN WRITE "NR" FOR NO REACTION

n the laboratory you are given the task of separating Ca2+ and Ag+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 K2SO4   2. fill in the blank 3 HBr   3. fill in the blank 5 Na2CO3

We now know the moles of hydroxide used in the titration. But, remember that, of the 100 mL of solution made from the ashes, only 20 mL were used for the titration. What is the total amount of hydroxide produced by the ashes? Volume HCl used: 5.44 mL Concentration HCl solution = 0.10 M 5.44 x 104 mol HCl used 5.44 x 104 mol OH in 20 mL solution X mol OH- resubmit total mol OH = 100 mL solution x Incorrect 5.44 x 104 mol 20 mL solution