How do you calculate the intrinsic viscosity of a polymer solution given only:

1) Time for a solution to go through a viscometer

2) Concentration

3) Viscometer constant

4) Density, viscosity, and time of water passing through a viscometer

I must calculate intrinsic viscosity and molar mass of cleaved and uncleaved PVOH solutions, but I am totally lost.

Let's say you are going to titrate a 200 ml solution of 0.5M KOH with a 0.1M solution of HNO3.

a) What is the initial pH?

b) Determine the pH when 300ml, 500ml, 975ml, 1000ml, 1005 ml, and 2000ml of the acid are added to the initial solution.

c) Sketch a rough titration curve.

3.36

On March 11, 2011, a massive earthquake and tsunami triggered a major disaster at Japan’s

Fukushima nuclear plant. A plume extending to the northwest of the site deposited significant amounts of iodine-131, cesium-134, and cesium-137 up to 30 miles away. Iodine-131 has an 8-day half-life and cesium-137 has a 3-year half-life. Determine how long it will take 99% of the iodine-131 and 99% of the cesium-

137 to naturally decay (you can learn about “U.S. Nuclear Power Safety One Year after Fukushima” by readin

g the report written by D. Lochbaum and E. Lyman, located on the web site of the Union of Concerned Scientists, http://www.ucsusa.org/publications/publications-nuclear-power.html)

How could solubility of an analyte impact its results in HPLC? How would the peak differ, for example? How would a more soluble molecule's peak differ from a less soluble one?

Also, what are the peak areas based on in HPLC? Why is one peak sharper and higher than another, for example? Does that relate to how well a molecule is retained by the stationary phase in the chromotography?

If you change the detection wavelength, how would the peak area of the same molecule change?

What does having a larger response factor mean in the internal standard method in HPLC? does it just relate just to the ratio of the two molecules?

write 3 paragraph on what you see could be the impact on the planet and society of this new approach to chemistry

Calculate the pH at 25°C of a 0.65 M aqueous solution of phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for phosphoric acid are 7.5 × 10−3, 6.25 × 10−8, and 4.8 × 10−13, respectively.)

Please show how you do the quadratic equation. I am struggling with this in particular. Thank you!

A tank of acetylene gas (C2H2) contains 52.0lb of the gas and is at a pressure of 511.2lb/in.2 .
Express the pressure of the gas in atmospheres. 760 mmHg= 14.696 lb/in.2.

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.
2Al(s)+3Cl2(g)→2AlCl3(s)

1) 7.7 g Al, 24.4 g Cl2

Express your answer using three significant figures.

2)0.230 g Al, 1.15 g Cl2

Express your answer using three significant figures.

How are Cu2+ and Bi3+ separated from Pb2+ and How can Bi3+ be separated from Cu2+?

Consider a titration involving 40.0 mL of 0.100 M ammonia , NH₃ (in an Erlenmeyer flask)with 0.100 M HCl (in a burette) to answer the next two questions.

NH₃ + HCl

A buffer solution is prepared by mixing 20.0 mL 0.45M HAc (acetic acid) with 35.0 mL 0.45M NaAc (sodium acetate)

(a) What is the amount of 4.0M HAc which must be added to this buffer solution to double [H3O+]?

(b) What is the amount of 2.0M HCl that must be added to decrease the pH by 0.50?

(c) How much NaOH(s) in g has to be added to the solution to raise the pH by 2.00?

The decomposition of Ethylene oxide, (CH2)2 O(g), at 652k is a 1st- order reaction with R=0.012 min^-1 and an activation energy of 218k J/mol (CH2)2 O(g) -----> CH4(g)+ CO (g)

Calculate a) the rate constant of reactin at 525k and b) the temperature at which the rate constant R=0.01min^-1 (universal gas constant R=8.314 J/mol^-1 k^-1)

Phosphine decomposes by the following reaction:

COCl_2(g) <---> CO_(g) + Cl_2(g) K_c = 8.3 x 10^-4

Calculate the concentration of each component when 2.55 g of phosphine decomposes in a 25.0mL flask.

An aqueous solution containing 5.99 g of lead(II) nitrate is added to an aqueous solution containing 5.04 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states.

balanced chemical equation:

Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq)Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq)

What is the limiting reactant?

The percent yield for the reaction is 83.2%. How many grams of the precipitate are formed?

How many grams of the excess reactant remain?

If the Ka of a monoprotic weak acid is 6.6×10−6, what is the pH of a 0.29 M solution of this acid?

The Ka of a monoprotic weak acid is 0.00604. What is the percent ionization of a 0.114 M solution of this acid?

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0154 M solution. The pH of the resulting solution is 2.38. Calculate the K_a for the acid.

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0186 M solution. The pH of the resulting solution is 2.60. Calculate the pKa for the acid.