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given that CO2 makes up .0355% of the atmosphere what is the maximum concentration fo CO2 in H2O. Using Henrys law C=kP where k for CO2 = 2*10^-3
On the previous problem set, you examined both radial wavefunctions and radial distribution functions. Do the two functions display radial nodes at the same places?
What is the total pressure in a 11.0 L flask 20.0°C, which contains 0.127 moles of H2 and 0.288 moles of N2
Hydrogenation of carbon double bonds C=C (i.e. adding a hydrogen on each carbon atom and thus reducing the double bond into a single bond: H-C-C-H) is a very common process in organic and polymer chemistry
what are the various parameters that can be changed performing MASCOT. how could them affects probability score, any one know about this
Suppose that 24 of each of the following substances is initially at 29.0. What is the final temperature of gold upon absorbing 2.30 of heat?
15.73 grams of a solution containing 8.43% acetic acid, HC2H3O2, is mixed with water and titrated with a 0.523 M solution of KOH. How many milliliters of the KOH solution are required to reach the equivalence point?
We recently did a lab/demo using the NMR to observe Na ions in sodium complexes in our Inorganic Class. I understand most of the post lab questions, but there are a few that still have me stumped.
What is the mass of 8.00 1022 molecules of tetraphosphorus decaoxide? (b) How many P atoms are present in this sample?
The precipitate SnO2·4H2O was removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 15.00 mL aliquot was buffered and titration of the lead, copper, and zinc required 35.78 mL 0.001500 M EDTA.
The theoretical value can be computed from the atomic weights of the atoms involved. How
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum-139.
65.50 mL of 0.161 M HF is titrated with 0.1200 M NaOH. What is the pH at the equivalence point? (Ka for HF is 6.8 x 10-4)
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