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 |
Determine whether each of the following equations for precipitation reactions is correct. If not, write the...
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. Correct the incorrect reaction Pb(NO3)2(aq)+2LiCl(aq)→2LiNO3(s)+PbCl2(aq)
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)
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)
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?
QUESTION 1 Which of the following is an example of a precipitation reaction? 2 Na (s) + Cl2 (g) → 2 NaCl (s) a. b. 12 (9) ► 12 (5) c. NaOH (aq) + HCl (aq) – NaCl(aq) + H20 (1) Pb(NO3)2 (aq) + 2KI (aq) – 2KNO3(aq) + PbI2 (s) d. LECTION Chek Chek Sue and submit to s u bmit Click Savel Anders to save all answer
You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) + 2KNO3 (aq) You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) +...
Identify the following solution reaction as acid-base / redox / precipitation reaction: 2NH4Cl(aq) + Pb(NO3)2 (aq) --> PbCl2(s) + 2NH4NO3(aq)
determine the limiting reactant express your answer ss a chemical formual A 27.0 mL sample of a 1.88 M potassium chloride solution is mixed with 15.0 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq) + Pb(NO3)2(aq) + PbCl2 (s) + 2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the limiting reactant, the theoretical yield, and the percent yield.
A 29.3-mL sample of a 1.22 M potassium chloride solution is mixed with 14.5 mL of a 0.860 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.46 g. Determine the limiting reactant, the theoretical yield, and the percent yield.
You mix a 25.0 mL sample of a 1.20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 2KNO3 (aq) You collect and dry the solid PbCl2 and find that it has a mass of 3.45 g. Determine the limiting reactant, and the percent yield? How many grams of excess reactant will remain when the reaction is complete?