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Considering the given equation where Keq = 0.016 2HI(g) ↔ H2(g) + I2(g) a container contains 0.60 M Hydrogen iodide, 0.038 M Hydrogen, and 0.15 M Iodine Initially at equilibrium. Determine the new equilibrium concentration of hydrogen, if the hydrogen concentration is raised by 0.299 M?
The absorbance of the unknown solution A=0.4862 +_ 0.0184 abs. units. Determine the un certainty in the concentration of the unknown.
Calcium fluoride CaF2 is an insoluble salt. The Ksp is 3.4 x 10^-11. Calculate the molar solubility of calcium fluoride.
If the molecular weight of a molecule is 180, how many grams would be required to make 100 milliliters of a 2 molar solution
The concentration of Mg2+ in a sample of water is 262 mmol/L At what pH will 99% of the Mg2+ be precipitated as Mg(OH)2? Ksp = 8.9 x 10-12
A certain shade of blue has a frequency of 7.12 × 1014 Hz. What is the energy of exactly one photon of this light
Adding a concentrated solution of NH4OH(aq) caused the precipitation of Cr+2 and Fe+3 as insoluble hydroxides. The Cu+2 remained in solution and forms the complex ion Cu(NH3)4+2. Which balanced molecular equations represent each of these reactions
What is the theoretical yield (in grams) of gold when 1.378 L of hydrogen gas (density = 0.0902 g/L) reacts with 20.14 g of gold(III) chloride in solution
A sugar water mixture contains 45.8g of sugar and 108.5 g of water. What is the percent by mass of sugar and the percent by mass of water in the solution?
How many grams of salicylic acid and of acetic anyhydride should she use? refer to the following reaction: 2 C7H6O3 + C4H603 -> 2 C9H8O4 + H20
Calculate the pH of the following solutions: 1.) 0.100 moles of HF and 0.120 moles of NaF in a 1.00 liter solution.--- 2.) a solution that has 0.10M NH4NO3 and 0.10 M NH3.--- 3.)0.100 moles of HF and 0.200 moles of NaCN in 1.00 liter solution.
The density of hydrogen gas in a flask is 0.147 g/L at 305 K. what is the pressure inside the flask? Calculate the density in G/L of CH4(g) at 75 Celsius and 2.1 atm (R= .08206 L*atm/mol*K).
Calculate the number of moles of ions present in 356 mL of 0.358 M calcium nitrate.
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