QUESTION 1 Which of the following is an example of a precipitation reaction? 2 Na (s)...
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
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)
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?
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?
Which of the following reactions could be considered a "precipitation" reaction? NaOH(aq) + HCl(aq) + NaCl(aq) + H2O(1) 2H2O(1) + 2H2(g) + O2(g) + 2Nal(aq) + Pb(NO3)2(aq) + 2NaNO3(aq) + Pbl2(s) 2C2H6(g) + 702(g) + 4CO2(g) + 6H2O(1) None of these
1. A 75.0-mL sample of 0.200 M Lead(II) nitrate, Pb(NO3)2, is reacted with 75.0 mL of 0.450 M KI solution and the following precipitation reaction occurs. Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) (a) Determine the limiting reactant. (b) How many grams of PbI2 will be formed if the yield is 100%? (c) What is the percent yield if 6.45 g of PbI2 were obtained? (2) K2Cr2O7(aq) + FeCl2(aq) → CrCl3(aq) + Fe(NO3)3(aq) (a) Determine the net ionic reactions and...
Which balanced chemical equation could represent the following result of a precipitation reaction? 0 0 0 400: Select one: • A. K2C1O4(aq) + 2AgNO3(aq) + Ag2 CrO4(s) + 2KNO3(aq) O B. MgSO4(aq) + 2AgNO3(aq) - Ag2SO4(s) + Mg(NO3)2(aq) O C. MgCl2(aq) + 2AgC2H302(aq) + 2AgCl(s) + Mg(C2H302)2(aq) O D. 2K3PO4(aq) + 3Cr2(SO4)3(aq) -- CrPO4(s) + 6KCl(aq) O E. K2S(aq) + Pb(NO3)2(aq) -- PbS(s) + 2KNO3(aq)
reaction MgI,(aq) + Pb(NO3)2(aq) + Mg(NO3), (aq) + Pb17 () Na(s) + Br, (1) NaBr, (s) type of reaction (check all that apply) combination precipitation single replacement combustion double replacement acid-base decomposition combination precipitation single replacement combustion double replacement acid-base decomposition combination precipitation single replacement combustion double replacement acid-base decomposition combination precipitation single replacement combustion double replacement acid-base decomposition CH, CH, OH (1) + 30 (8) ► 2002 (8) + 3H,0 (8) H Br(aq) + NaOH(aq) NaBr(aq) + H, 0(1)
Which of the following is not a precipitation reaction? a. Na2SO4 + CaCl2 --> CaSO4 + NaCl b. MgCl2 + AgNO3 --> Mg(NO3)2 + AgCl c. NaOH + HCl --> NaCl + H2O d. NaCl + AgC2H3O2 --> NaC2H3O2 + AgCl
QUESTION 7 Which of the following is the net ionic reaction between hydrochloric acid and aqueous sodium hydroxide NaOH(aq) + HCl(aq) - NaCl(aq) + H20 (1) H(aq) + OH (aq) - H20 (1) Na* (aq) +Cr (aq) - NaCl (aq) b. c. NaOH (aq) + HCl(aq) - NaCl (aq) + H20 (1) Na" (aq) - OH(aq) - NaOH(aq) CSP and Suhtel it