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Calculate the pH of the solute in an aqueous solution of 0.372 M (CH3)3N(aq) if the Kb is 6.5 Ã- 10âˆ'5.
What is the percentage protonation of the solute?
what volume will it occupy? Assume constant pressure. Note the temperatures are given in two different units. Be sure to change each to deg K first.
At a certain temperature and pressure 2.8 L of N2 reacts with 4.2 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure.
How many liters of softened water, containing a sodium concentration of 5.8×10^-2% sodium by mass, have to be consumed to exceed the FDA recommendation (less than 2.4 g sodium per day)? (Assume a water density of 1.0 g/mL.)
Calculating the equilibrium constant (Keq) for the given reactions - Determine the Keq for the following reactions
How many moles of each ion are in each solution? (a) 2 mol of potassium perchlorate dissolved in water K+ mol ClO4- mol (b) 255 g of magnesium acetate dissolved in water Mg2+ mol C2H3O2- mol
The rate constant for a certain reaction is = 5.70×10-3 s^-1. If the initial reactant concentration was 0.650 M, what will the concentration be after 14.0 minutes.
What is the concentration of chromium ion present in a 0.01976 M solution of potassium hydroxide in contact with a large excess
There is 12.0 g CCl3F in a 1.1 L container at 856 torr and 300 K. What is the mass of the liquid left over?
write the chem equation for the reaction which occurs when solutions of potassium sulfide and iron (II) chloride are mixed.
Determine the final temperature of the mixture. (Use 1g/mL as the density of water)
My dilemma is that I'm unsure on how to find the actual limiting reactant, and what information I should use. There's too much given; but from my introspection, we only need 1-Octene and the Pt catalyst
In a first order decomposition in which the rate constant is 0.0181 sec-1, how long will it take (in seconds) until 0.484 mol/L of the compound is left, if there was 0.548 mol/L at the start?
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