Barium sulfate (BaSO₄) is known for its very low solubility in water, with a solubility product (Ksp) indicating that only about 0.0002 grams can dissolve in 1 liter of water at room temperature. Therefore, to dissolve 1 gram of barium sulfate, an impractically large volume of water—approximately 5,000 liters—would be needed. This highlights the compound's nature as a sparingly soluble salt.
To find the molarity of the barium hydroxide solution, first calculate the number of moles of hydrochloric acid used in the titration. Then use the stoichiometry of the reaction to determine the number of moles of barium hydroxide present. Finally, divide the moles of barium hydroxide by the volume of the solution in liters to get the molarity.
26.8125 g
At standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. To find the number of moles of ammonia gas (NH₃) required to fill a volume of 50 liters, you can use the formula: moles = volume (liters) / volume per mole (liters/mole). Therefore, the calculation is 50 liters / 22.4 liters/mole = approximately 2.24 moles of NH₃ are needed.
1 litre = 1000 millilitres. You now have all the information required to work out, for yourself, the answer to this and similar questions.
For an awake 70 kg male, it's about 5 liters per min. If you're asleep it can fall to about 4 liters per min.
Balanced equation first. BaCl2 + Na2SO4 -> 2NaCl + BaSO4 22.6 ml BaCl2 = 0.0226 liters 54.6 ml Na2SO4 = 0.0546 liters 0.160 M BaCl2 = moles BaCl2/0.0226 liters = 0.00362 moles BaCl2 0.055 M Na2SO4 = moles Na2SO4/0.0546 liters = 0.0030 moles Na2SO4 The ratio of BaCl2 to Na2SO4 is one to one, so either mole count wull drive this reaction. Use 0.0003 moles Na2SO4 0.0030 moles Na2SO4 (1 mole BaSO4/1 mole Na2SO4)(233.37 grams/1 mole BaSO4) = 0.700 grams of BaCO4 produced
Amount of sodium sulfate required = 0.683 x 350/100 = 0.239The formula mass of sodium sulfate, Na2SO4 is 2(23.0) + 32.1 + 4(16.0) = 142.1 Therefore mass of sodium sulfate required = 0.239 x 142.1 = 34.0g Approximately 34 grams of sodium sulfate would be needed.
0.125 Molar solution! Molarity = moles of solute/Liters of solution Algebraically manipulated, Moles of copper sulfate = 2.50 Liters * 0.125 M = 0.313 moles copper sulfate needed ===========================
To find the molarity of the barium hydroxide solution, first calculate the number of moles of hydrochloric acid used in the titration. Then use the stoichiometry of the reaction to determine the number of moles of barium hydroxide present. Finally, divide the moles of barium hydroxide by the volume of the solution in liters to get the molarity.
You in a cult ? ... This question is suss -_-
First, calculate the number of moles of barium chloride using its molar mass. Then, convert the volume from milliliters to liters. Finally, divide the number of moles by the volume in liters to find the molarity of the solution.
To determine the mass of ammonium sulfate needed to make a 0.5 M solution: Calculate the molar mass of ammonium sulfate (NH4)2SO4. Use the formula: Mass (g) = Molarity (M) x Volume (L) x Molar mass (g/mol). Plug in the values: Molarity = 0.5 M, Volume = 0.5 L, and Molar mass of (NH4)2SO4. Calculate to find the mass of ammonium sulfate required.
39.25 liters.
That depends on the model of the transformer. I have seen transformers that required 7500 liters and some that needed 2,5 liters.
Ba(NO3)2 Molarity = moles of solute/Liters of solution ( 100 ml = 0.100 liters ) 0.10 M Ba(NO3)2 = moles Ba(NO3)2/0.100 liters = 0.01 moles Ba(NO3)2 (261.32 grams/1 mole Ba(NO3)2) = 2.6 grams of Ba(NO3)2 needs to be put into that 100 milliliters of solution.
Required for what? Required to do what? Required by whom? Required by what authority? What are you trying to figure out? This could be a drinking water quality question for the municipal water authority, or a chemistry question [how much can you dissolve], or a whole number of other possibilities. Also, so you mean Magnesium metal [Mg] or Magnesium Chloride [MgCl2]? To go along with the Potassium Chloride [KCl].
To find the molarity of the solution, first calculate the number of moles of lithium sulfate in 734g. Then, divide the moles by the volume of solution in liters to get the molarity. Remember to convert grams to moles using the molar mass of lithium sulfate (Li2SO4).