Please indicate for every reactions where equal amounts of chemicals (all in aqueous solutions) are mixed...

Question

Question

science chemistry

Answer 1

Answer #1

(i) AgNO₃(aq) + KI(aq) → AgI(s) + KNO₃(aq)

ppt will form

(ii) Pb( NO3)₂ (aq) + 2KI(aq) → PbI₂ (s) + 2KNO₃(aq)

ppt will form

(iii) No reaction

(iv) Na3PO4 (aq) + Ca(NO3)2 (aq) => Ca3(PO4)2 (s) + NaNO3 (aq)

ppt will form

(v) MgSO4(aq) + BaCl2(aq) --> BaSO4(s) + MgCl2(aq)

ppt will form

(vi) Ca(NO3)2 (s) + 2 NH4Cl (s) ---> 2 N2O (g) + CaCl2 (s) + 4 H2O (g)

ppt will form

(vii) CoCl2 (aq) + Ca (OH)2 (aq) -> Co(OH)2 (s) + CaCl2 (aq)

ppt will form

Your one thumbs up will help me lot. Thanks!

Add a comment

Answer 2

Similar Homework Help Questions

Consider a solution containing lead ions (Pb^2+). Which of those same fourteen solutions would cause a...

Consider a solution containing lead ions (Pb^2+). Which of those same fourteen solutions would cause a precipitate to form when mixed with this lead ion solution? Use the fourteen solutions below. AICIE N Hg BaCl2 CuSO4 FeCl3 HCI Pb(NO3)2 HNO3 KI AgNO3 Na co NaOH Na3PO4 H2SO4
What are the identities of the precipitate in each of the following reactions: A) AgNO3 (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)
Use the solubility table to answer the following. You do not need to mix any chemicals....

Use the solubility table to answer the following. You do not need to mix any chemicals. 1. Circle the following compounds if they will not dissolve completely or will form ppt in H a CaSO4 (s) Cu(IO3)2(s) AgNO3(s) Baco3 (s) Pb(NO3)2(s) Al(OH)3(s) 2. circle all of the following solutions that will form a precipitate with addition of Mg(IO3)2 aq) Ba (NO3)2(aq) Pb (NO3)2(aq) K2CO3 (aq) CuCl2(aq) NH40H (aq) ZnSO4(aq) 3. Circle all of the following solutions that will not form...

please help me find the cation and anion nominal concentrations for columns 4 and 5. the...

please help me find the cation and anion nominal concentrations for columns 4 and 5. the original solutions used as sources of ions are all 0.20 M. I'd appreciate if you showed the process as well as the answers. thank you! no equilibrium constant was given. It says the dilution equation must be used to determine the the nominal concentrations. Solutions Mixed Cation Anion Solution Solution Concentrations [Cation] [Anion] AgNO3 NaCI 0.10 0.10 AgNO3 KI AgNO3 Na2SO4 BaCl2 NaCl 0.10...
PLEASE DO ALL 3. Calculate the number of moles of precipitate that would be produced when...

PLEASE DO ALL 3. Calculate the number of moles of precipitate that would be produced when two solutions were mixed. a 1.0 mL 0.10 M Pb(NO3)2 and 5.0 ml, 0.10 M KI b. 2.0 ml 0.10 M Pb(NO3)2 and 4.0 mL, 0.10 M KI c. 3.0 mL 0.10 M Pb(NO3)2 and 3.0 mL, 0.10 M KI d. 4.0 mL 0.10 M Pb(NO3)2 and 2.0 mL, 0.10 M KI e. 5.0 mL 0.10 M Pb(NO3)2 and 1.0 mL, 0.10 M KI
Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions...

Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. nitric acid, HNO3, and calcium hydroxide, Ca(OH)2 B. lead (II) nitrate, Pb(NO3)2, and potassium iodide, KI

Compare the solubility of lead chloride in each of the following aqueous solutions: Clear All 0.10...

Compare the solubility of lead chloride in each of the following aqueous solutions: Clear All 0.10 M Pb(NO3)2 More soluble than in pure water. 0.10 M NH4Cl Similar solubility as in pure water. 0.10 M NaNO3 Less soluble than in pure water. 0.10 M NH CH3COO
(1) For the following pairs of aqueous solutions: (1) KOH(aq) & Ag(NO3)2 (aq) (2) Ba(OH)2 (aq)...

(1) For the following pairs of aqueous solutions: (1) KOH(aq) & Ag(NO3)2 (aq) (2) Ba(OH)2 (aq) & Pb(NO3)2(aq) Do the following: (a) Determine if a precipitate forms when the two solutions are mixed. (b) If a precipitate forms write down its molecular formula. (C) Write the net ionic equation for the precipitation reactions. (2) For the acid-base neutralization reactions below. (1) HCI + LiOH (2) HNO, + Ca(OH), Write down the: (a) Molecular equation (b) Net ionic equation (3) Compute...
please, I need assistance with this Laboratory Report on the periodic table. Part A 1. Place...

please, I need assistance with this Laboratory Report on the periodic table. Part A 1. Place 9 clean small test tubes in a test tube rack. The test tubes should be clean but do not have to be dry because aqueous solutions will be used. 2. To cach test tube add 5 drops of the solution (0.1 M) indicated in the data table. 3. Next add 5 drops of silver nitrate (0.5 M) to each of the 9 test tubes....

15. The mixing of which pair of reactants will result in a precipitation reaction? CsI(aq)...

15. The mixing of which pair of reactants will result in a precipitation reaction? CsI(aq) + NaOH(aq) HCl(aq) + Ca(OH)2(aq) K2SO4(aq) + Hg2(NO3)2(aq) NaNO3(aq) + NH4Cl(aq) 16. Which of the following is a precipitation reaction? Zn(s) + 2 AgNO3(aq) 2 Ag(s) + Zn(NO3)2(aq) NaCl(aq) + LiI(aq) NaI(aq) + LiCl(aq) 2 KI(aq) + Hg2(NO3)2(aq) Hg2I2(s) + 2 KNO3(aq) HI(aq) + NaOH(aq) NaI(aq) + H2O(l) None of these are precipitation reactions. 17. Which...