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Suppose you take a 35.00 mL sample of this acid solution. You then titrate it with a 0.1522 M sodium hydroxide solution. A volume of 29.25 mL of the sodium hydroxide was required to complete the titration. What is the concentration of this unknown hydrochloric acid solution?
A 1.630 g sample of naphthalene, C10H8(s), is completely burned in a bomb calorimeter assembly and a temperature increase of 8.44°C is noted.
using a gas sample of an ideal gas of .95 mol 3.00 atm and at 300 k expands from sixteen litres to twenty eight litres
Compute the activities and activity coefficients of both components in this solution on the Raoult's law basis. Explain the vapor pressures of the pure components at this temperature
Using a Table of Thermochemical Data, calculate ΔS for the following reaction. Is entropy increasing or decreasing? Is the system becoming more random or less random? Based on entropy changes only, would you predict the reaction to be spontaneous or ..
The following diagram represents a reaction shown going to completion. Letting A = red spheres and B = blue spheres, write a balanced equation for the reaction. Write the equilibrium- constant expression for the reaction.
How many grams of Na2CO3 are present in 29.7 mL of a 31.0% Na2CO3 solution. The density of the solution is 1.09 g/mL.
A piston has an external pressure of 13.00 atm. How much work has been done if the cylinder goes from a volume of 0.160 liters to 0.540 liters.
Write a balanced equation using the correct formulas and include conditions ( s, l, g, or aq) for each of the following reactions- Solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas:
What is the temperature of the gas in kelvins? Express your answer to three significant figures.
The viscosities are 1.00 × 10-3 kg m-1 s-1, and 2.2 ×10-4 kg m-1 s-1, respectively.
Enough of a monoprotic acid is dissolved in water to produce a 0.0194 M solution. The pH of the resulting solution is 6.26. Calculate the Ka for the acid.
Write the net ionic equations for & the reactions occurring for each cation in the group.
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