What are the identities of the precipitate in each of the following reactions:
A) AgNO3 (aq) + KI (aq) ------> Ag (s) + KNO3 (aq)
B) Pb(NO3)2 (aq) + 2KI (aq) ------> PbI2 (s) + 2KNO3 (aq)
C) Na3PO4 (aq) + 3Ca(NO3)2 (aq) ------> Ca3(PO4)2 (s) + 6NaNO3 (g)
D) MgSO4 (aq) + BaCl2 (aq) ------> BaSO4 (s) + MgCl2 (aq)
E) COCl2 (aq) + Ca(OH)2 (aq) ------> CaCl2 (aq) + Co(OH)2 (s)
What are the identities of the precipitate in each of the following reactions: A) AgNO3 (aq)...
Consider the balanced equation of KI reacting with Pb(NO3)2 to form a precipitate. 2KI(aq)+Pb(NO3)2(aq)⟶PbI2(s)+2KNO3(aq) What mass of PbI2 can be formed by adding 0.413 L of a 0.140 M solution of KI to a solution of excess Pb(NO3)2?
Determine whether each of the following equations for precipitation reactions is correct. If not, write the correct equation. If no reaction occurs, choose NO REACTION. Ba(NO3)2(aq)+(NH4)2SO4(aq)→BaSO4(s)+2NH4NO3(aq)Ba(NO3)2(aq)+(NH4)2SO4(aq)→BaSO4(s)+2NH4NO3(aq) correct incorrect no reaction BaS(aq)+2KCl(aq)→BaCl2(s)+K2S(aq)BaS(aq)+2KCl(aq)→BaCl2(s)+K2S(aq) correct incorrect no reaction 2KI(aq)+Pb(NO3)2(aq)→PbI2(s)+2KNO3(aq)2KI(aq)+Pb(NO3)2(aq)→PbI2(s)+2KNO3(aq) correct incorrect no reaction Pb(NO3)2(aq)+2LiCl(aq)→2LiNO3(s)+PbCl2(aq)Pb(NO3)2(aq)+2LiCl(aq)→2LiNO3(s)+PbCl2(aq) correct incorrect no reaction
2KI (aq) + Pb(NO3)2 (aq) + PbI, (s) + 2KNO3 (aq). How much 0.7 M KI solution in liters will completely precipitate the Pb2+ in 2.1 L of 0.18 M Pb(NO3), solution? Do not include units in your answer and round to two significant figures. Druiden bela
For each of the following precipitation reactions, calculate how many grams of the first reactant are necessary to completely react with 18.0 g of the second reactant. a. 2KI(aq)+Pb(NO3)2(aq)→PbI2(s)+2KNO3(aq) b. Na2CO3(aq)+CuCl2(aq)→CuCO3(s)+2NaCl(aq) c. K2SO4(aq)+Sr(NO3)2(aq)→SrSO4(s)+2KNO3(aq)
A solution containing 1.25 g of KI is combined with a solution containing 2.42 g of Pb(NO3)2. What mass of PbI2 would result using the following equation? 2KI(aq) + Pb(NO3)2(aq) = 2 KNO3(aq) + PbI2(s).
Potassium iodide reacts with lead (ii) nitrate in the following precipitation reaction: 2KI (aq) + Pb(NO3)2 (aq)---> 2KNO3 (aq) + PbI2 (s) What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all the lead in 155.0 mL of a 0.122 M lead (ii) nitrate solution?
1. Na2CO3(aq) + Ni(NO3)2(aq) 2. NaCl(aq) + AgNO3(aq) 3. Na2CO3(aq) + HCl(aq) Select Select precipitate gas hot test tube cool test tube color change NR 4. NaOH(aq) + HCl(aq) 5. Kl(aq) + Pb(NO3)2(aq) Select Select 6. Na2CO3(aq) + CaCl2(aq) 7. BaCl2(aq) + H2SO4(aq) 8. CuSO4(aq) + NaOH(aq) 9. Zn(s) + H2SO4(aq) 10. Zn(s) + CuSO4(aq) 11. Ni(NO3)2(aq) + NaOH(aq) 12. NaOH(aq) + FeCl3(aq) Select Select Select Select 13. Mg(s) + HCl(aq) Select
For each of the following chemical equations, fill in the missing information, AgNO3(aq) + NaCl(aq) AgCI NaNO31 AgNO3(aq) + Cu(NO3)2(aq) AgNO3| ) + Cu(NO3)2 AgNO3(aq) + Na3PO4(20) Ag3P NaNO3 NaCl(aq) + Cu(NO3)2(aq) NaNO34 + CuCl2 NaCl(aq) + Na3PO4(a) NagPO, + NaCl Cu(NO3)2(aqt Na3PO4(29) Cuz(PO4)2
Consider the net ionic equation: 3Ca+2 (aq) + 2PO4-3 (aq) → Ca3(PO4)2 (s) Which of the following unbalanced chemical equations could give rise to this net ionic equation? A. CaCl2 + Na3PO4 → Ca3(PO4)2 + H2O B. CaC2 + H3PO4 → Ca3(PO4)2 + C2H2 C. Both of the above reactions. D. None of the above reactions
The test for sulfate used in lab may give a false positive. Even though there is no sulfate, the precipitate may form. However, the test for phosphate does not give a false positive. Explain why the test for phosphate does NOT give a false positive, whereas the sulfate test may give a false positive. Sulfate tests: Na2SO4(aq) + BaCl2(aq) --> BaSO4(S)2NaCl(aq) ---True positive 2Na3PO4(aq) + 3BaCl2(aq) --> Ba3(PO4)2(S) + 6NaCl(aq) ---False positive Phosphate tests: 2Na3PO4(aq) + 3Mg(NO3)2(aq) --> Mg3(PO4)2(S) +...