React NaCl(aq) with AgNO_3(aq) to produce NaNO_3(aq) and AgCl(s). What are the spectator ions? What is the net ionic equation?
What is a precipitate?
Why do you need a stir bar in the calorimeter?

React NaCl(aq) with AgNO_3(aq) to produce NaNO_3(aq) and AgCl(s). What are the spectator ions? What is...
consider the equation NaCl(aq)+AgNO3(aq)>AgCl(s)+NaNO3(aq) identify the spectator ions in the equation
Identify the spectator ions in the following molecular equation. LiCl(aq) + AgNO3(aq) → AgCl(s) + LiNO3(aq)
2. When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) + AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO, reacts with excess NaCl? a. 1.55 g b. 2.62 c. 4.17 g d.6.20 g
Consider the reaction. AgNO3(aq) + NaCl(aq) - NaNO, (aq) + AgCl(s) What is the total ionic equation for this reaction? NO3(aq) + Nat(aq) Na+ (aq) + NO3(aq) O Ag+ (aq) + NO3(aq) + Na+ (aq) + CI+ (aq) - Na+ (aq) + NO3(aq) O Ag+ (aq) + NO3(aq) + Na+ (aq) + CH(aq) Na+ (aq) + NO3(aq) + AgCl(s) O Ag+(s) + NO3(aq) + Na+ (aq) + CF (S) - Na+ (aq) + NO3(aq) + AgCl(s) O Ag+ (aq) +...
2. Write the net ionic equation for the following. Which ions are spectator ions? (NH4)2CO3(aq) + Cu(NO3)2(aq) → CuC03(s) + 2 NH4NOg(aq)
Separate the following balanced chemical equation into its total ionic equation. AgNO3(aq)+NaCl(aq) ---> NaNO3(aq)+AgCl(s) __ (aq) + __ (aq) + __ (aq) + __ (aq) --> __ (aq) + __ (aq) + __ (s)
NaCl (aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) Note: All of the aqueous species in the above reaction exists as ions in solution: NaCl(aq) exists as Na+ and Cl- AgNO3 exists as Ag+ and NO3- NaNO3 exists as Na+ and NO3- AgCl(s) is a white solid 1) A solution contains 2.00 grams of Sodium Chloride. How many grams of AgNO3 must be added to the solution to completely react with Sodium Chloride according to the reaction above? List equipment and materials...
Identify the spectator ions in the following complete ionic equation. 2K+(aq)+S2−(aq)+Pb2+(aq)+2NO−3(aq)→PbS(s)+2K+(aq)+2NO−3(aq) Express your answers as ions separated by a comma.
CaCl2 reacts with AgNO3 in aqueous solutions to produce a precipitate of AgCl that can be filtered and weighed. The balanced equation for the reaction is: CaCl2 (aq) + 2 AgNO3 (aq) → 2 AgCl (s) + Ca(NO3)2 (aq) Suppose you have a mixture that contains CaCl2, plus other compounds that do not react with AgNO3. If 0.2918 g of the mixture yields 0.4462 g of AgCl, what is the percentage of CaCl2 in the mixture? Molar masses: CaCl2 110.98...
2Na+(aq)+2OH−(aq)+Zn2+(aq)+2NO3−(aq) → Zn(OH)2(s)+2Na+(aq)+2NO3−(aq) The complete ionic equation you determined in Part C is shown above for your convenience. The net ionic equation only depicts the chemical species that participate in the reaction, and that is the formation of a solid between one type of cation and one type of anion in this precipitation reaction. Recall that any of the ions that do not participate in the reaction are spectator ions, and spectator ions are excluded from the net ionic equation....