A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 MNaOH solution. Calculate the pH after the following volumes of base have been adde

Part A

35.5 mL

Express your answer using two decimal places

Part B

50.0 mL

Express your answer using two decimal places

A 10.0 mL solution of 0.030 M AgNO3 was titrated with 0.015 M NaBr in the cell. S.C.E. || titration solution | Ag(s) Find the cell voltage for 0.4, 10.0, 20.0, and 27.0 mL of titrant. (The Ksp of AgBr = 5.0 ✕ 10−13.) 0.4 V 10.0 V 20.0 V 27.0 V

A solution is prepared by dissolving 32.5 g of a nonvolatile solute in 200 g of water. The vapor pressure above the solution is 21.85 Torr and the vapor pressure of pure water is 23.76 Torr at this temperature. What is the molecular weight of the solute?

You are asked by your new boss to prepare 750 ml of a 0.5M pH 8.4 tris- (hydroxymethyl) amminomethane (Tris) buffer. The Tris base is provided in the solid form (mol. wt. 121.1 g/mole, pKa 8.1). You are also supplied with solutions of 0.5 M HCl and 0.5M NaOH. Explain how you would prepare this buffer.

Liquid enters a valve at Tin and exits at Tout, Pout = 1 atm. Determine Tin and Tout to vaporize 20% of the feed if the liquid is 1/3 benzene and 2/3 toluene.

Which of the following two reactions would have an equilibrium constant more favorable to the right? Explain your answer.

The followings are related to the ‘’Synthesis of Nickel Nanowires’’ which are broken down into 4 related questions.

a ) Draw a schematic diagram of the synthesis of nickel nanowires by electrodeposition. Identify the anode and the cathode in the experimental setup.

b) What are the corresponding half-reactions occurring at the anode and at the cathode?

c) What determines the final dimensions of the nanowires?

d) How are the nanowires separated from the template?

Note: Please answer clearly and at a professional level!

Be able to calculate the amount of solute when given the ppm or ppb concentrations and the amount of solution or solvent.

Be able to calculate the molarity of a solution when given the mass or moles of solute and the volume of solution.

Be able to calculate the amount of solute (mass or moles) when given the molarity of solution and the volume of solution.

Be able to calculate the volume of solution when given the molarity of solution and the amount solute (mass or moles).

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).