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briefly discuss the errors tahat occur in the above titration and the change in the colour of the indicators.

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What is the molality of a solution by dissolving 2 moles of NaOH in 10kg of water?

10kg of water contains 10l of water. So morality is 0.2mildm-3.


How many cups are in 40 mL?

40 metric cups is 10L


What is the final volume if 10L of methane reacts with 20L of Oxygen at 100c and two atmospheres?

The reaction between methane and oxygen to form carbon dioxide and water is balanced as follows: CH4 + 2O2 -> CO2 + 2H2O. Using the ideal gas law, we can calculate the final volume by determining the number of moles of methane and oxygen reacting and then finding the volume of the products formed at the same conditions of temperature and pressure.


How many moles of gas are present in a 10L container when 3.84atm of pressure is exerted at 35 Celsius?

Assuming that gas being used is an ideal gas, the gas law equation PV=nRT can be used. P=Pressure (atm) V=Volume (Liters) n=Moles R=0.08206 (a gas constant) T=Temperature (Kelvin) In this problem we know that there is a 10L container with 3.84atm of pressure at 35 C. So P=3.84atm, V=10L, and R=0.08206. To calculate T, you need to convert from Celsius (C) to Kelvin (K). Using the formula K=273+C, you should get T=308K. Now you know all of the variables you can work the problem out. Solve the equation for moles(n) by dividing each side by R and T: (PV/RT)=n Plug in your numbers and solve with a calculator: n=(3.84)(10)/(0.08206)(308) =(38.4)/(25.27448) =1.5193190918 Leaving us a rounded answer of 1.52n in the container


What volume is needed to store .80 moles of helium gas at 204.6 kpa and 300 kelvin?

First let's convert 204.6kPa to atm: 204.6 / 101.3 = 2.02atm. Now, use PV = nRT: (2.02)(V) = (0.80)(0.0821)(300), solve for V to get 9.75L, so a 10L container would work just fine.