How many grams of copper (II) chloride should be added to 1.50 Liters of water if a 2.235 M solution is desired?
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To determine how many grams of copper (II) chloride should be added to 1.50 liters of water to make a 2.235 M solution, you first need to calculate the number of moles of copper (II) chloride required.
Use the formula: moles = molarity × volume (in liters)
Given: Molarity (M) = 2.235 M Volume (in liters) = 1.50 L
Calculate moles of copper (II) chloride needed: moles = 2.235 M × 1.50 L
Once you have the moles, you can use the molar mass of copper (II) chloride to convert moles to grams.
The molar mass of copper (II) chloride (CuCl2) is: Copper (Cu): 1 atom × 63.55 g/mol = 63.55 g/mol Chlorine (Cl): 2 atoms × 35.45 g/mol = 70.90 g/mol Total molar mass = 63.55 g/mol + 70.90 g/mol = 134.45 g/mol
Now, multiply the number of moles by the molar mass: grams = moles × molar mass
Calculate the grams of copper (II) chloride needed.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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