Consider the reaction. 2 NaCl(aq)+Ba(OH), (aq) → BaCl, + 2 N2OH Identify the precipitate, or lack thereof, for the reaction. O no precipitate O BaCl, O NAOH

Excess Na2SO4(aq) is added to a 4.41×102 mL sample of industrial waste containing Ba2+ ions. If 55.5 g of BaSO4(s) are precipitated from the reaction, what was the molar concentration of Ba2+ in the original sample?

A student combined CuCl2 (aq) and Na (s). The student observed a color change, thus a reaction occurred. Write the balanced molecular equation for this reaction showing coefficients and phase labels. Write the complete ionic equation for this reaction. Write the net ionic equation for this reaction. Assign oxidation numbers to the reactants and products in the net ionic equation. Which reactant, CuCl2 (aq) or Na (s), got oxidized? Which reactant, CuCl2 (aq) or Na (s), got reduced? Which reactant, CuCl2 (aq) or Na (s), is the oxidizing agent? Which reactant, CuCl2 (aq) or  Na (s), is the reducing agent?

9 mL of a 1.25 M solution of CaCl2(aq) is reacted with 125.0 mL of 0.17M  solution of Na3PO4(aq) Given the reaction : 2Na3PO4(aq) + 3CaCl2(aq) → Ca3(PO4)2 (s)+6NaCl(aq) Determine the mass of the precipitate Ca3(PO4)2 formed Determine the concentration in mol/L of NaCl in the solution after the reaction has occurred Determine the concentration in mol/L of Na3PO4 in the solution after the reaction has occurred Determine the concentration in mol/L of CaCl2 in the solution after the reaction has occurred

1-A 15.0 mL solution of Sr(OH)₂ is neutralized with 35.6 mL of 0.350 M HCl. What is the concentration of the original Sr(OH)₂ solution? 2-If 15.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq) 3-You add 475 mL of water to 40.0 mL of 0.550 M MgCl₂ solution. Assuming the volumes are additive, what is the MgCl₂ concentration in the diluted solution?

A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. Write the balanced molecular equation for the reaction. Write the net ionic equation for the reaction. How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).

In the laboratory you are given the task of separating Ca2+ and Fe2+ 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 lons, give the formula of the precipitate. If it cannot, type "No" Y or N 1. 12. 3 Reagent Formula of Precipitate if YES ка K₂SO4 Na CO

While working in a lab, Ronan reacts 50.0 mL of 0.320 mol/L Na2CO3 (aq) with 85.0 mL of 0.210 mol/L AlCl3 (aq). Calculate the mass of Al2(CO3)3 precipitate that forms when the reaction is complete 3 Na2CO3 (aq) + 2 AlCl3 (aq) → Al2(CO3)3 (↓) + 6 NaCl (aq)

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

A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.