Silver nitrate solution reacts with calcium chloride solution according to the equation: AgNO3 + CaCl2 → Ca(NO3)2 + AgCI Suppose we mix together a solution containing 12.6 g AGNO3 and 8.4 g CaCl2.

Write the balanced NET ionic equation for the reaction when aqueous BaCl₂ and aqueous (NH₄)₂SO₄ are mixed in solution to form aqueous NH₄Cl and solid BaSO₄.

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, provide the net ionic equation. KI+ Pb(NO3)2

3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.

Classify each chemical reaction: reaction CH, OCH (1) +30₂(g) → 2CO₂ (g) + 3H₂O(g) HI (aq)+ NaOH (aq) → Nal (aq) + + H₂O(1) Mgl, (aq) + Pb(NO₂)₂ (aq) → Mg(NO3)₂(aq) + Pbl₂(s) 2 Mg(s) + F₂ (g) → 2MgF (s) - type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X O precipitation combustion acid-base O precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base S

Lead ions can be precipitated from solution with KC1 according to the following reaction: Pb²+ (aq) + 2 KCl(aq) → PbCl₂(s) + 2 K+ (aq) When 28.8 g KCl is added to a solution containing 25.5 g Pb²+, a PbCl₂ precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.6 g. Part A Determine the limiting reactant. KCI Pb²+ Submit Part B m = Determine the theoretical yield of PbCl₂. Submit Part C Request Answer ΨΕ ΑΣΦ Submit Request Answer Determine the percent yield for the reaction. ΨΕ ΑΣΦ Request Answer BE ? ? % g

Classify each chemical reaction: Ba (CIO,),(s) → BaCl,(s) + 30, (8) KOH(aq) + HBrO (aq) 1 reaction CuSO4 (aq) + Zn CrO4 (aq) K BrO (aq) + H₂O (1) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) ZnSO4 (aq) + Cu Cro(s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base

In the laboratory you are given the task of separating Ba2+ and Cu2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. K₂SO4 2.0 3. Na₂CO3 HCI

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. → NaCl(aq) + H₂O(1) X 0-0 Ś

Classifying Reactions and Balancing Chemical Equations Part A: For each of the chemical reactions that are listed below, balance the chemical equation and then state the type of chemical reaction. 1. - Cu (s) + O₂(g) → CuO (s) Reaction type: 2.H₂O ()→→O₂ (g) + H₂ (B) Reaction type: 3. Fe (s) + H₂O () Fe₂O3 (s) + H₂(g) Reaction type: 5. 4.H₂S (aq) + AsCl3 (aq) →→As2S3 (s) + HCl(aq) Reaction type: CaCO3 (s) → CO₂(g) + Reaction type: 6. C4H10O (g) + O₂(g) →→CO₂(g) + H₂O (c) Reaction type: 7. S8 (s) + Fe (s)→ FeS (s) Reaction type: CaO (s) 8. H₂SO4 (aq) +Al (s) →→Al2(SO4)3 (aq) + H₂(g) Reaction type: 9. H3PO4 (aq) + NH,OH (aq) Reaction type: (NH4)3PO4 (aq) + stei HOH (c) 2017-