A solution contains CO32- and OH". Separation of these two anions by selective precipitation is accomplished by first adding Ba(NO3)2 solution, then filtering and finally adding to the filtrate (what is passed through the filter) a solution of CATIONS High Solubility (aq) Low Solubility (s) NH4NO3. TINO 3. Sr(NO3)2. NaNO3. Cl, Br, I Halides Pb(NO3)2 Most Ag+, Pb²+, Tl+, Hg₂2+, Hg, Cu 52. Solubility Table Group 1, NH₁, Group 2 Most ANIONS OH Group 1, NHƯ, Sri Ba²+, Tl Most SO₂² Most Ag, Pb²+, Ca²+, Ba²+, Sr²+, Raz CO3², PO₂¹ SO3² All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Group 1, NH4 C₂H30₂ NO3 Most All Most Ag+ None

A solution contains 9.92×103 M ammonium carbonate and 9.27x103 M sodium hydroxide. Solid iron(II) acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of iron(II) ion when this precipitation first begins? [Fe?*] =[ M

At a certain temperature, chlorine gas and carbon monoxide react to form carbonyl chloride: Cl2(g) + 2 CO(g) 2 coC(g). When 3.0 x 10-3 M Cl2 is mixed with 0.030 M CO and 9.0 x 10-3 M COCI, the concentration of ccl decreases. Which statement below is true? а. Кс 100 c. Kc = 30 d. Kç > 30 e. Kç = 100 f. Kç < 100 Your answer is incorrect. The correct answer is: Kc < 30

A solution contains 1.45x10-2 M sodium carbonate and 9.94x10-3 M ammonium sulfide. Solid copper(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu²+] = M

Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is  M.

11c.

1. A solution of HCIO, was standardized by dissolving 0.3745 g of primary standard grade HgO in the solution of KBr. The liberated OH required 37.79 mL of the acid to be neutralized. Calculate the molarity of HCIO.. HgOs) + 4Br + H,0 > HgBr. + 20H

Step 1 Lead(II) ions of Lead(II) nitrate reacts with chloride ion of NaCl to form a PbCl2 precipitate. Pb2+(aq) + 2Cl-(aq) →PbCl2(s) arrow_forward Step 2 The precipitate of PbCl2 starts forming when the reaction quotient (Q=[Pb2+][Cl-]2) is greater than the solubility product of PbCl2. The solubility product of PbCl2  is Ksp=1.17×10-5 To find the concentration of chloride ion that starts the precipitation of PbCl2, equate Q to solubility product and solve for the concentration of Chloride ion. [Pb2+][Cl-]2 =1.17×10-5 [Cl-]2 =1.17×10-5[Pb2+] [Cl-] =1.17×10-5[Pb2+] [Pb2+] = concentration of lead(II) nitrate solution [Cl-] =1.17×10-51.0×10-2=3.4205×10-2 M   arrow_forward Step 3 The mass of NaCl needed to start the precipitation of PbCl2 is calculated below. mass of NaCl =[Cl-]×Volume of solution ×Molar mass of NaCl mass of NaCl =3.4205×10-2 M×800 mL ×58.44 gmol mass of NaCl =3.4205×10-2 molL×800 ×10-3 L ×58.44 gmol mass of NaCl =159915.216×10-5 g =1.599 g =1.6

Solid potassium hydroxide is slowly added to 150 mL of a 0.0614 M silver acetate solution. The concentration of hydroxide ion required to just initiate precipitation is ______ M.

A solution is prepared by adding 150.0 mL of a 0.0100 M Mg(NO3)2 solution to 250.0 mL of a 0.100 M NaF solution. Will anything precipitate from this solution and, if so, what is the precipitate?   a. No, nothing will precipitate.   b. Yes, MgF 2   c. There is not enough information to answer this question.   d. Yes, Mg(NO 3 ) 2   e. Yes, NaNO 3