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You weigh out pure Calcium carbonate.... 0.1740 g a) Calculate how many whole drops (.05 mL/drop) of 6 M HCl are required to dissolve this. (I found this to be 11.59 drops or 12 full drops) How do you do part b? CaCO3 + 2HCl---> Ca2+ +2Cl- +H2O+CO2 please use 4 sig fig in all calculations b) What is the Ca concentration when this is dissolved and diluted to 100.00mL?
Draw the enantiomer of proline which would give rise to the absolute stereochemistry and draw a proposed catalytic cycle for the transformation and how does the catalyst activate the substrate
Does beta-D-fructose in its cyclic form have the same number of chiral carbons as beta-D-glucose?
A gas occupying a volume of 248 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume.
A voltaic cell is constructed with two Zn+2-Zn electrodes. The two cell compartments have [Zn+2]=5.00 M and [Zn+2]=1.00 x 10^-2 M, respectively. What is the standard emf of the cell?
The temperature is increased to 45 degree celcius then determine what is the pressure in the cylinder
What is the solubility of BaF2 (Ksp = 1.8x10-7) in pure water in grams per liter? The molecular weight of BaF2 is 175.
The volume of a manifold used to transfer gases is calibrated using Boyle's Law. A 0.251-dm3 flask at pressure of 697 Torr is attached and after system pumpdown,
If 42.3 L of PH3 forms when 85.1L of H2 (g) reacts with 167.6 (g) of P4 at STP. What is the percent yield.
At what temperature will a gas be at if you allow it to expand from an original 456 mL at 65 celcius to 3.4 L?
What would be the resulting molarity of a solution made by dissolving 21.9 grams of KCl in enough water to make an 869-milliliter solution?
what volume of a 0.37 M Mg(NO3)2 solution contains 87g of Mg(NO3)2.
In a high-altitude city, the normal atmospheric pressure is 607.1 torr. Use the Clausius-Clapeyron equation to estimate the boiling point of water in this city
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