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A rod 8.6 cm long is uniformly charged and has a total charge of -26.1 μC Determine the magnitude of the electric field along the axis of the rod at a point 40.8268 cm from the center of the rod. The Coulomb constant is 8.98755 × 109 N · m2/C2.
A mixture is made by combining 1.39 lb of salt and 5.07 lb of water. What is the percentage of salt (by mass) in this mixture?
Determine the concentration of each of the individual ions in a 0.600 M NiCl3 solution
Assuming that the density of the solution is 1.0 g/mL, find the molarity of the hydrogen ion in the solution. The molar mass of HCl is 36.5 g/mol
For the neutralization reaction involving HNO3 and Ca(OH)2, how many liters of 1.55 M HNO3 are needed to react with 45.8 mL of a 4.66 M Ca(OH)2 solution.
It is found that 4.68e-06 g of Nd2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Nd2(CO3)3
Initially a container contains 0.46 M HI and no product. What is the equilibrium concentration of H2
What is the pH of a solution prepared by titration 100.0 mL of 0.100 M Acetic Acid (CH3COOH) with 20.0 mL of 0.250 M NaOH
For the equilibrium H2(g)+ CO2(g) H2O(g)+CO(g) Kc=3.18 at 1106K. If each of the four species was initially present at a concentration of 3.000M.
An unknown acid has a molar mass of 90. g/mol and a mass composition of, 40%-C, 6.7%-H, and 53.3% -O. What is the molecular formula of the acid
Will a precipitate of magnesium flouride form when 200.0 milliliter of 1.9x10^-3mol/Litre MgClsubnumber2 solution is added to 300.0 milliliter of 1.4x10^-2mol/Litre NaFsolution?
What would be the best indicator for the titration of 0.20 M CH3COOH titrated with 0.2 M NaOH? (Ka for acetic acid = 1.8 X 10-5) The pH ranges for the color change of some common acid base indicators are given below
A 1.80 g sample of a large boimolecule was dissolved in 18.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C. Calculate the molar mass of the biomolecule.
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