please answer and explain

Determine what type of crystalline solid each example below represents.
Covalent Network Ionic Metallic Molecular  Argon, Ar
Covalent Network Ionic Metallic Molecular  Copper Nitrate, Cu(NO₃)₂
Covalent Network Ionic Metallic Molecular  Copper, Cu
Covalent Network Ionic Metallic Molecular  Quartz, SiO₂
Covalent Network Ionic Metallic Molecular  Sucrose, C₁₂H₂₂O₁₁
Covalent Network Ionic Metallic Molecular  KHg

Reaction is: Pb(NO3)2(aq) + 2KI(aq) ---> PbI2(s) + 2KNO3(aq) 2.0 ml of 0.250M Pb(NO3)2 and 7.0 ml of 0.250M KI

A) In your experiment, one of the reagents was limiting and the other was in excess. Therefore after the lead(II)iodide precipitated from the solution, there were spectator ions left in the solution, and also the unreacted excess reagent. Assuming complete precipitation of lead (II) iodide, calculate the concentrations of each type of ion (Pb2+, K+, NO3-, I-) present in the solution after the PbI2 precipitated out.

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.834 M and [Sn2 ] = 0.0190 M. Standard reduction potentials can be found here.

Provide a high level (cartoon or box model) description of how an ICP-MS and how an IC work.

A solution contains 0.018 mol each of I– , Br– , and Cl– . Use the Ksp values given below to determine how much AgCl(s) precipitates out when this solution is mixed with 200 mL of 0.24 M AgNO3.

A student left 40.0 mL of a bottle of 12.0 M HCl out overnight. The next morning, the bottle has only 35.7 mL of liquid left. Assuming that the volume change is only due to loss of water, what will be the molarity if the remaining solution is diluted to 150 mL? a)3.20 M b)2.86 M c)6.0 M d)12.0 M

Determine the mass of chloride (MW = 35.45 g/mol ) in grams present in 100 mL of a 0.187 M solution of aqueous FeCl3 (iron(III) chloride).

Limiting reactnt experiment

• What happens, if you will not stir the reaction mixture while heating on hot plate?
• What would be the effect, if you will add tap water instead of deionized water into the salt mixture?
• How will you identify the limiting reagent?
• What technique will you use to separate the un-reacted chemical from the reaction mixture?

Do emotional or pain-induced tears differ?

Is it possible to test tears and deduce if they are related to physical pain or emotion, if so what is the difference between the two?

what are the advantages of GC/Ms compared to GC with other detectors?

An aqueous solution of ___ will produce a neutral solution?

a. RbBr

b. LiNO₂

c. LiF

d NH4ClO₄

e. Rb₂CO₃

Rank these forces from weakest to strongest:

dispersion, dipole-dipole, H-bonds, dipole-induced dipole, ion-induced dipole, and ion-dipole.

Use the rules (in order) to assign oxidation numbers to each of the elements in the compounds below.

Solve an equilibrium problem (using an ICE table) to calculate the pH of each of the following solutions.

1.0.17M CH3NH2

.17M CH3NH3Cl

a mixture that is 0.17M in CH3NH2

and 0.17M in CH3NH3Cl

When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation

2AgNO3(aq)+CaCl2(aq)?2AgCl(s)+Ca(NO3)2(aq)

Part A

What mass of silver chloride can be produced from 1.35L of a 0.166M solution of silver nitrate?

Express your answer with the appropriate units.

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Part B

The reaction described in Part A required 3.38L of calcium chloride. What is the concentration of this calcium chloride solution?

Express your answer with the appropriate units.

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