You wish to prepare 223 grams of 21.1 % CrBr2. You will need grams of chromium(II)...
You wish to prepare 223 grams of 21.1 % CrBr2. You will need grams of chromium(II) bromide and mL of water. Assume that the density of water is 1.00 g / ml.
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You wish to prepare 223 grams of 21.1 % CrBr2. You will need
grams of chromium(II)...
You wish to prepare 239 grams of 27.4 % Co(NO3)2. You will need Assume that the...
You wish to prepare 239 grams of 27.4 % Co(NO3)2. You will need Assume that the density of water is 1.00 g /ml. grams of cobalt(II) nitrate and mL of water.
You wish to prepare 202 grams of 12.5% (w/w) . Assume that the density of water...
You wish to prepare 202 grams of 12.5% (w/w) . Assume that the density of water is 1.00 g/mL. QUESTION: You will need _________ grams of sodium iodide and _______ mL of water.
An aqueous solution is made by dissolving 22.3 grams of chromium(II) bromide in 479 grams of...
An aqueous solution is made by dissolving 22.3 grams of chromium(II) bromide in 479 grams of water. The molality of chromium(II) bromide in the solution is___ m.
The freezing point of water H2O is 0.00°C at 1 atmosphere. How many grams of chromium(II)...
The freezing point of water H2O is 0.00°C at 1 atmosphere. How many grams of chromium(II) bromide (211.8 g/mol), must be dissolved in 287.0 grams of water to reduce the freezing point by 0.450°C ? ____ g chromium(II) bromide.
A student wishes to prepare 250-mL of a 0.250 M chromium(II) iodide solution using solid chromium(II)...
A student wishes to prepare 250-mL of a 0.250 M chromium(II) iodide solution using solid chromium(II) iodide, a 250-mL volumetric flask, and deionized water. (a) How many grams of chromium(II) iodide must the student weigh out?
You wish to prepare 100.0 mL of a 325.0 ppm w/v sodium (MW = 22.9897 g/mol)...
You wish to prepare 100.0 mL of a 325.0 ppm w/v sodium (MW = 22.9897 g/mol) solution. How many grams of sodium dichromate dihydrate (Na2Cr2O7·2H2O, MW = 297.998 g/mol) are needed to prepare this solution? Assume the final solution has a density of 1.00 g/mL.
1)The mole fraction of chromium(II) sulfate, CrSO4, in an aqueous solution is 5.61×10-2 . The percent...
1)The mole fraction of chromium(II) sulfate, CrSO4, in an aqueous solution is 5.61×10-2 . The percent by mass of chromium(II) sulfate in the solution is %. 2) An aqueous solution is 40.0 % by mass hydrochloric acid, HCl, and has a density of 1.20 g/mL. The mole fraction of hydrochloric acid in the solution is . 3)An aqueous solution is 40.0 % by mass potassium bromide, KBr, and has a density of 1.37 g/mL. The mole fraction of potassium bromide in the...
1. You need to make an aqueous solution of 0.137 M chromium(II) iodide for an experiment...
1. You need to make an aqueous solution of 0.137 M chromium(II) iodide for an experiment in lab, using a 125 mL volumetric flask. How much solid chromium(II) iodide should you add? ________grams 2. How many milliliters of an aqueous solution of 0.172 M iron(II) acetate is needed to obtain 18.6 grams of the salt? ______mL
You wish to prepare 250.0250.0 mL of a 225.0225.0 ppm w/v Fe2+Fe2+ (MW=55.845 g/molMW=55.845 g/mol) solution....
You wish to prepare 250.0250.0 mL of a 225.0225.0 ppm w/v Fe2+Fe2+ (MW=55.845 g/molMW=55.845 g/mol) solution. How many grams of ferrous ammonium sulfate hexahydrate (Fe(NH4)2(SO4)2⋅6H2O(Fe(NH4)2(SO4)2⋅6H2O, MW=392.14 g/molMW=392.14 g/mol) are needed to prepare this solution? Assume the final solution has a density of 1.00 g/mL.
A student weighs out 3.68 g of CrBr2, transfers it to a 125. mL volumetric flask,...
A student weighs out 3.68 g of CrBr2, transfers it to a 125. mL volumetric flask, adds enough water to dissolve the solid and then adds water to the 125 mL mark on the neck of the flask. Calculate the concentration (in molarity units) of chromium(II) bromide in the resulting solution? _____ M Please show steps to solve!
You wish to prepare 239 grams of 27.4 % Co(NO3)2. You will need Assume that the density of water is 1.00 g /ml. grams of cobalt(II) nitrate and mL of water.
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