Net Ionic Equations Select the NET-IONIC equation from the list (A - ), for each of the suggested reactions, in aqueous medium. | Aqueous solutions of AGNO3 and NazCro4 mix to form a precipitate. | Aqueous solutions of AGNO3 and KCI mix to form a precipitate. | Aqueous solutions of SrCl2 and NazSO4 mix to form a precipitate. A. 2AGNO3 + NazCrO4 → 2NANO3 + Ag2CrO4 В. AGNO3 + KCI H AgCl + KNO3 C. SrCl2 + NazSO4 – SrS04 + 2NACI | D. 2Ag* + CrO42 – Ag2CrO4 E. Nat + CI - NaCI F. 2Ag* + 2NO3 + 2Na* + Croq2- → Ag2CrO4 + 2NaNO3 Sr2+ + so,2 SrS04 G. Н. NO3 + K* + KNO3 I. Ag+ + Cl AGCI J. none of the above

Net Ionic Equations Select the NET-IONIC equation from the list (A - ), for each of the suggested reactions, in aqueous medium. | Aqueous solutions of AGNO3 and NazCro4 mix to form a precipitate. | Aqueous solutions of AGNO3 and KCI mix to form a precipitate. | Aqueous solutions of SrCl2 and NazSO4 mix to form a precipitate. A. 2AGNO3 + NazCrO4 → 2NANO3 + Ag2CrO4 В. AGNO3 + KCI H AgCl + KNO3 C. SrCl2 + NazSO4 – SrS04 + 2NACI | D. 2Ag* + CrO42 – Ag2CrO4 E. Nat + CI - NaCI F. 2Ag* + 2NO3 + 2Na* + Croq2- → Ag2CrO4 + 2NaNO3 Sr2+ + so,2 SrS04 G. Н. NO3 + K* + KNO3 I. Ag+ + Cl AGCI J. none of the above

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. Drag the appropriate reactions to their respective bins. Precipitate MnBr2 + Na2SO3 No precipitate Ba(NO3)2 + KOH HNO3 + CuSO4 Hg(NO3)2 + Na3PO4 Reset Help
How do you do these Double displacement Reactions.
34 excess silver nitrate is added to 100.0 mL of a solution containing barium ions to produce 1.84 g of AgCl precipitate molar mass equals 143.32 g•mol^-1. What is the molar concentration of the silver iron in the original solution?
You have three soultions: Na2CO3, BaCl2 and KNO3. You also have four reagents, HCl, CaCl2, NaOH, and H2SO4, that can help you identify all three solutions. Which one of these reagents can you use to be able to identify and label all three solutions? Explain your reasoning. Include any net ionic equations for precipitation reacions.
Use the precipitation interactive to answer the questions. Select the color of the solid that forms when Ni(NO3)2Ni(NO3)2 solution is added to K2SK2S solution. white green black yellow Complete the net ionic equation for the reaction. Cation ++ Anion ⟶⟶ Precipitate
What does the notation Į mean? The species is negligible in the reaction. The species is dissolved in water. The species also participates in the reaction below the one in which the Į notation appears. The species precipitates (it is an insoluble solid).
CTO:2. Use solubility rules to determine the solubility of the following compounds: insol compound sol compound sol MgCl, Li₂SO4 KF CaSO4 AgBr K₂CO3 BaCl, Zn(NO3)2 AI(NO3)3 Pb(NO3)2 Hg(OAc)2 Pbl₂ CaS NaOAc CTO:3 insol compound sol ZnCO3 Cu(OH)2 NH₂OH Ni3(PO4)2 AIPO4 Na3PO4 AgNO3 insol
You have aqueous solutions of Ag* and PO43- that have equal concentrations. You mix them according to the following table: Test Tube # Number of drops Ag Number of drops PO4³- 01 0 4 2 1 3 3 9 2 t 8 3 6 4 Assuming the product of the reaction is insoluble, which test tube will contain the most. precipitate? 8 5 9 3
9 and 14
2. Write the balanced net ionic equation, including the phases, for the given reaction. A solution of Ba(OH), and a solution of H,S0, are mixed. Water and a precipitate of BaSO . balanced net ionic equation:
Using solubility rules, predict the solubility in water of the following ionic compounds. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. PbS- AgNO3- Na2CO3- CaI2-
Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. If no reaction occurs leave all boxes blank and click on "Submit". Use H* for hydronium ion. Write a net ionic equation for the reaction that occurs when potassium sulfite (aq) and excess hydrochloric acid (aq) are combined. Note: Sulfites follow the same solubility trends as sulfates. +