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What is the concentration of nitrate ions in 40.0 mL of a 0.25 M solution of copper(II) nitrate (Cu(NO_3)_2)?
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6. Chemical Quantities & Aqueous Reactions
Molarity
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What is the mass in grams of EDTA (molar mass = 292 g/mol) required to prepare 500 mL of a 0.01 M EDTA solution?
A
2.92 g
B
1.46 g
C
0.146 g
D
0.292 g
Guida verificata passo dopo passo1
Identify the given information: volume of solution (V) = 500 mL, molarity (M) = 0.01 M, and molar mass (MM) of EDTA = 292 g/mol.
Convert the volume from milliliters to liters because molarity is expressed in moles per liter: \(V (L) = \frac{500}{1000} = 0.5\) L.
Calculate the number of moles of EDTA needed using the molarity formula: \(\text{moles} = M \times V = 0.01 \times 0.5\).
Convert moles of EDTA to mass in grams using the molar mass: \(\text{mass} = \text{moles} \times MM = (0.01 \times 0.5) \times 292\) g.
The result from the previous step gives the mass of EDTA required to prepare 500 mL of a 0.01 M solution.
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