Solution Test Review W Full Answers0 
Solution Review
Complete all questions in this package. Be careful to use correct significant figures and units for any calculation problems. For all chemical equations use phase subscripts.
Concentration
1. Calculate the concentration of the solution formed when 23.61 g of sodium phosphate is dissolved in 475.0 cm3 of water.
2. What volume of water is needed to dissolve 85.8 g of silver nitrate to make a 2.650 M solution?
3. What mass of magnesium sulphate is needed to make 1500 mL of a 2.45 M MgSO4 solution?
4. Calculate the concentration of the solution formed when 59.78 g of ammonium hydroxide is dissolved in 856.0 cm3 of water.
5. What volume of water is needed to dissolve 150.8 g of lithium borate to make a 9.46 M solution?
6. What mass of mercury (II) iodide is needed to make 1350 mL of a 3.17 M HgI2 solution?
7. How many moles of (NH4)2CO3 are contained in 2.40 L of a 0.899 M solution?
Dilutions
1. A 350.0 mL solution is diluted to 1.965 L. At this dilution, it has a concentration of 0.97 M. What was the original concentration?
2. Calculate the resulting concentration when 460.0 mL of 6.58 M ammonium phosphate solution has 650.0 cm3 of water added to it.
3. What volume of water is needed to dilute 275.0 mL of 7.95 M AlCl3 solution to a concentration of 0.820 M?
4. A 10.00 mL solution is diluted to 680.0 mL. Calculate the original concentration if it now has [ ] = 0.055 M?
Ion Concentration Calculations
1. What is the concentration of each ion in a 10.5 M sodium silicate solution?
2. What is the concentration of each ion in the solution formed when 94.5 g of nickel (III) sulphate is dissolved into 850.0 mL of water?
3. If 3.78 L of 0.960 M calcium fluoride solution is added to 6.36 L of 0.550 M ammonium fluoride solution, what is the resulting concentration of each ion?
4. What is the concentration of each ion in the solution formed when 94.78 g of iron
Complete all questions in this package. Be careful to use correct significant figures and units for any calculation problems. For all chemical equations use phase subscripts.
Concentration
1. Calculate the concentration of the solution formed when 23.61 g of sodium phosphate is dissolved in 475.0 cm3 of water.
2. What volume of water is needed to dissolve 85.8 g of silver nitrate to make a 2.650 M solution?
3. What mass of magnesium sulphate is needed to make 1500 mL of a 2.45 M MgSO4 solution?
4. Calculate the concentration of the solution formed when 59.78 g of ammonium hydroxide is dissolved in 856.0 cm3 of water.
5. What volume of water is needed to dissolve 150.8 g of lithium borate to make a 9.46 M solution?
6. What mass of mercury (II) iodide is needed to make 1350 mL of a 3.17 M HgI2 solution?
7. How many moles of (NH4)2CO3 are contained in 2.40 L of a 0.899 M solution?
Dilutions
1. A 350.0 mL solution is diluted to 1.965 L. At this dilution, it has a concentration of 0.97 M. What was the original concentration?
2. Calculate the resulting concentration when 460.0 mL of 6.58 M ammonium phosphate solution has 650.0 cm3 of water added to it.
3. What volume of water is needed to dilute 275.0 mL of 7.95 M AlCl3 solution to a concentration of 0.820 M?
4. A 10.00 mL solution is diluted to 680.0 mL. Calculate the original concentration if it now has [ ] = 0.055 M?
Ion Concentration Calculations
1. What is the concentration of each ion in a 10.5 M sodium silicate solution?
2. What is the concentration of each ion in the solution formed when 94.5 g of nickel (III) sulphate is dissolved into 850.0 mL of water?
3. If 3.78 L of 0.960 M calcium fluoride solution is added to 6.36 L of 0.550 M ammonium fluoride solution, what is the resulting concentration of each ion?
4. What is the concentration of each ion in the solution formed when 94.78 g of iron