# How many grams of copper (II) chloride should be added to 1.50 Liters of water if a 2.235 M solution is desired?

By signing up, you agree to our Terms of Service and Privacy Policy

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.

By signing up, you agree to our Terms of Service and Privacy Policy

- Why are nitrates always soluble?
- What percentage of water vapor is found in the air?
- What is the freezing point of an aqueous solution containing #"40.0 g"# of ethylene glycol in #"60.0 g"# of water? #K_f = 1.86^@"C/m"# and #K_b = 0.512^@ "C/m"# for water.
- 0.040mol of (NH4)2Ni(SO4)2•6H2O is dissolved in water to give 200cm3 of aqueous solution. What is the concentration, in mol dm–3, of ammonium ions?
- What is an example of a solvation practice problem?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7