Consider the reaction of 30.0 mL of 0.235 M BaI₂ with 20.0 mL of 0.315 M Na₃PO₄.  a.) Write and balance the chemical equation, including state of matter labels.  b.) Determine how much precipitate is formed if all the BaI2is used up. c.) Determine how much precipitate is formed in all the Na3PO4is used up. d.) How much precipitate is actually formed? e.) Emily did this experiment in the lab, and isolated 1.23 g of precipitate. What is the percent yield for this reaction?

You are in lab and ready to mix a beaker containing a solution of sodium cyanide with a beaker containing a solution of cobalt (III) acetate. You mix 45.0 mL of a 6.32 M solution of the sodium cyanide with an excess amount of cobalt (III) acetate. 1. Write out the balanced molecular reaction (including all physical states) for this reaction. 2. Calculate the amount of moles of sodium cyanide that was added into the mixture. 3. Calculate the minimum amount of moles of cobalt (III) acetate required to completely react the sodium cyanide. 4. Calculate the mass, in grams, of the solid produced from the reaction.

6. A sample of hydrochloric acid is standardized using sodium bicarbonate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bi- carbonate, NaHCO,. a. Iment b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. Calculate the mass percent concentration of hydrochloric acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL. c.

Write the formula for the precipitate (if any) from the reaction of CuNO3(aq) and (NH4)2S(aq). Write just the precipitate (not the whole reaction). Remember to include the state (i.e. (s) ). If no precipitate is formed, write NO REACTION. (already tried no reaction, did not work)

Silver iodide is a photosensitive material used in photography. One method of forming silver iodide is the reaction between potassium iodide and silver nitrate in solution. 5. Assume aqueous solutions of Potassium Iodide and Silver Nitrate are the starting substances (reactants) in the reaction. e. determine if a solid precipitate is formed in this reaction. If yes, state its chemical formula. f. If 1.75 g of potassium iodide and 3.21 g of silver nitrate are combined, then what is the limiting reactant? Theoretically what mass of the solid product could form from these amounts of reactants? g. What is the percent yield if 1.50 g of the solid product was actually obtained in lab? h. How many potassium atoms are in 0.986 g of potassium iodide? please answer all parts of question.

1. Weigh 0,500 g of NaCl-containing sample and treat with 25 mL of 0.1086 M AgNO3 solution. The remaining AgNO3 is titrated with 11.3 mL of 0.1010 M KSCN. How many g NaCl is found in the sample? find mass percentage of NaCl in the sample? (NaCl = 58.5 g / mol). 2. Arsenic in a 5.0 gram sample is converted to H3ASO4 by appropriate procedures. After the acid is neutralized and converted to AsO 4³ ion, 35.0 mL, 0.04952 M AgNO3 is added to precipitate Ag3ASO4(s) 3Ag+ AsO4³ Ag3ASO4(s) 8.88 mL of 0.1110 M KSCN was used to titrate excess Ag Ag +SCN→ AgSCN (s) Calculate the mass percentage of As2O3 in the sample? (As203: 198)

I only need help with the highlighted ones please :)

Which substances, when mixed together, will produce a precipitate? (All reactants are aqueous? a. NaF + CaCl2 b. NH4OH + K3PO4 c. Pb(NO3)2 + LiC2H3O2 d. CuBr2 + Na2SO4

5 volume of base ..

A 2.000g mixture containing only AgCl (MM = 143.32 g/mol) and AgBr (MM = 187.78 g/mol). It is quantitatively reduced to 1.300g silver metal Ag (MM = 107.87 g/mol). Calculate the percentage by mass of the AgCl and AgBr in the sample.