Concentration of formamide at equilibrium
If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00M and 2.00M, respectively, what will the concentration of HCONH2 be at equilibrium?
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1. Find the pH of a solution that has a concentration of hydrochloric acid equal to 0.001 M. 2. Find the normal pH of rainfall (not acid rain). Would a rain sample with a pH of 5.0 be considered "acid rain"
What is the balanced ionic and net ionic equation for each: 1.MgCO3 + HBR 2.CH3CO2H + NH4OH 3.AgNO3 + AlCl3 4.BaF2 + H2SO4
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, 14.0
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.100 M HClO(aq) with 0.100 M KOH(aq). The ionization constant for HClO can be found here.
When a sample of HI(g) (0.1192 mol/L) is placed in 110.0 L reaction vessel at 968.0 K and allowed to come to equilibrium the mixture contains 0.02028 mol/L of H2(g). What concentration (mol/L) of HI(g) reacted? 2HI(g) = H2(g)+I2(g)
An antacid tablet containing magnesium hydroxide instead of calcium carbonate was dissolved in 10 mL of 0.2893 M HCL. 10 mL of this solutions was tritated to endpoint with 25.20 mL of 0.1007 M NaOH. How much magnesium hydroxide was in the antacid
Each component contains different metals and minerals. The pebbles and shells can easily be separated from the sand. Which term or terms could be used to describe this sample of sand?
The pressure increases from 1.10 atm to 3.06 atm, and the volume of the sample changes from 2.67 L to 4.57 L. To what temperature, in oC, was the methane heated?
What is the molar concentration of sodium ions in a solution in which 75.02 g of sodium sulfate and 102.75 g of sodium phosphate were completely dissolved in 500.00 mL of water and brought to a final solution volume of 750.00 mL?
A swan can float on a lake with only 33% of its volume below the surface. What is the average density of the swan
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