A. You wish to prepare 198 grams of 10.3 % Na3PO4. How many grams will need of sodium phosphate and how many mL of water? Assume that the density of water is 1.00 g / ml.
B. If 20.5 grams of an aqueous solution of cobalt(II) sulfate, CoSO4, contains 2.84 grams of cobalt(II) sulfate, what is the percentage by mass of cobalt(II) sulfate in the solution?
C. An aqueous solution of lead nitrate, Pb(NO3)2, contains 8.74 grams of lead nitrate and 17.5 grams of water. What is the percentage by mass of lead nitrate in the solution?
D. An aqueous solution is 1.00% by mass ethanol, CH3CH2OH, and has a density of 0.996 g/mL. What is the molarity of ethanol in the solution?
E. An aqueous solution is 22.0% by mass silver nitrate, AgNO3, and has a density of 1.22 g/mL. What is the molarity of silver nitrate in the solution is?
F. An aqueous solution of 15.7 M ammonia, NH3, has a density of 0.892 g/mL. What is the percent by mass of NH3 in the solution?
Following is my Solution to the First full question i.e. Question: A)
The Answers are found to be the following:
- Grams of sodium phosphate (Na2PO4) = 20.39 gm
- Volume (mL) of Water (i.e. H2O) = 177.61 mL
The solution to the above results, are discussed/explained below: (i.e. in image format):
Correction: In the above solution at one "line" of the answer, Sodium Phosphate has been incorrectly mentioned as Na2PO4....
Correct representation of Sodium Phosphate is the following:
Sodium Phosphate is written as Na3PO4
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