Calculating A sample of barium nitrate is placed into a jar containing water
A 68.4-g sample of potassium chloride was added to 200.0 g of water at 20 ºC. Is the solution saturated, unsaturated, or supersaturated? Use the graph to help answer the questionSubstance Solubility Substance SolubiliBarium- Hydroxide 3.89 Potassium- Chloride 34.2Barium-Nitrate 9.02 Sodium- Chloride 35.9Calcium-Hydroxide 0.173 Sucrose 203.9Thank You!!! :)
A 13.50 g sample of Au is heated, then placed in a beaker containing 60.00 g water. The temperature of water increases from 19.00 ºC to 20.00 ºC. What is the initial temperature of the gold sample? Cs (Au) = 0.1300 J/gºC; Cs (H2O) = 4.184 J/gºC
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
1) A student added 56.4 grams of barium nitrate to 894 grams of water. The resulting solution had a density of 1.12 g/ml. What is the weight perfect, molarity, and molarity of the solution? 2) A student evaporated 545 ml of a .523M sodium chloride solution down to a volume of 275 ml. What is the molarity of this final solution?
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2CO3. If the mass of the BaCO3 precipitate formed is 0.7578 g, what is the percent by mass of Ba in the original unknown compound?
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A jar of tea is placed in sunlight until it reaches an equilibrium temperature of 32.6 ◦C . In an attempt to cool the liquid, which has a mass of 189 g , 98.8 g of ice at 0.0 ◦C is added. At the time at which the temperature of the tea is 28.6 ◦C , find the mass of the remaining ice in the jar. The specific heat of water is 4186 J/kg · ◦ C . Assume the...
When a 5.12-g sample of solid sodium nitrate dissolves in 31.1 g
of water in a coffee-cup calorimeter (see above figure) the
temperature falls from 25.00 oC to 16.37 oC.
Calculate H in kJ/mol NaNO3 for the solution
process.
NaNO3(s)
Na+(aq) + NO3-(aq)
The specific heat of water is 4.18 J/g-K.
We were unable to transcribe this imageWe were unable to transcribe this imagethermometer stirrer coffee cups containing reaction mixture When a 5.12-g sample of solid sodium nitrate dissolves in...
Calculating molarity using solute moles (please show
work)
A chemist prepares a solution of barium chlorate (Ba(CIOby measuring out 12.1 umol of barium chlorate into a 350. ml. volumetric flask and filling the flask to the mark with water Calculate the concentration in mmol/L of the chemist's barium chlorate solution. Round your answer to 3 significant digits. mmol
A student was given a solid containing a mixture of nitrate salts. The sample completely dissolved in water, and upon addition of dilute HCI, no precipitate formed. The pH was lowered to about 1 and HS was bubbled through the solution. No precipitate formed. The pH was adjusted to 8 and HS was again bubbled in. This time, a precipitate formed, Which compounds might have been present in the unknown? Zn(NO), Fe(NO), Ca(NO), AgNO, Sn(NO) NaNO, Bi(NO), CH(NO), Which salts...