How many milliliters of 3.0 M NaOH are required to react with 0.50g of Cu2+ to form Cu(OH)2?
To determine the number of milliliters of 3.0 M NaOH required, we need to first calculate the number of moles of Cu2+ and then use the stoichiometry of the reaction to determine the moles of NaOH required. Finally, we can convert the moles of NaOH to milliliters using the molarity.
Here are the step-by-step calculations:
Step 1: Calculate the moles of Cu2+
Given:
Mass of Cu2+ = 0.50g
We need to determine the number of moles of Cu2+. To do this, we divide the mass of Cu2+ by its molar mass.
Molar mass of Cu2+ = atomic mass of Cu x 2
Molar mass of Cu = 63.55 g/mol
Molar mass of Cu2+ = 2 x 63.55 g/mol = 127.1 g/mol
Number of moles of Cu2+ = Mass of Cu2+ / Molar mass of Cu2+
Number of moles of Cu2+ = 0.50g / 127.1 g/mol
Step 2: Use the balanced equation to determine the moles of NaOH required
The balanced equation for the reaction is:
Cu2+ + 2OH- -> Cu(OH)2
From the balanced equation, we see that 1 mole of Cu2+ reacts with 2 moles of OH-. Therefore, the moles of NaOH required will be the same as the moles of Cu2+.
Moles of NaOH required = Number of moles of Cu2+
Step 3: Convert moles of NaOH to milliliters using the molarity
Given:
Molarity of NaOH = 3.0 M
To convert moles of NaOH to milliliters, we can use the formula:
Moles of solute = Molarity x Volume (in liters)
Volume (in liters) = Moles of solute / Molarity
Volume (in liters) = Moles of NaOH / Molarity
Volume (in milliliters) = Volume (in liters) x 1000
Volume (in milliliters) = (Moles of NaOH / Molarity) x 1000
Step 4: Substitute the values into the equation and calculate
Moles of NaOH = Number of moles of Cu2+ (from step 1)
Volume (in milliliters) = (Number of moles of Cu2+ / Molarity of NaOH) x 1000
Now, you can substitute the values into the equation and calculate the volume of NaOH required.
To determine the number of milliliters of 3.0 M NaOH required to react with 0.50 g of Cu2+ to form Cu(OH)2, we need to use stoichiometry and the equation for the reaction.
The balanced equation for the reaction between NaOH and Cu2+ is:
2NaOH + Cu2+ -> Cu(OH)2 + 2Na+
In this reaction, we see that 2 moles of NaOH react with 1 mole of Cu2+ to produce 1 mole of Cu(OH)2.
Step 1: Calculate the moles of Cu2+
To determine the number of moles of Cu2+ in 0.50 g, we need to divide the given mass by the molar mass of Cu2+. The molar mass of Cu2+ is the sum of the atomic masses of copper (Cu) and twice the atomic mass of oxygen (O).
Molar mass of Cu2+ = 63.55 g/mol + 2 * 16.00 g/mol = 95.55 g/mol
Moles of Cu2+ = mass of Cu2+ / molar mass of Cu2+
= 0.50 g / 95.55 g/mol
Step 2: Use stoichiometry to determine the moles of NaOH required
From the balanced equation, we know that 2 moles of NaOH react with 1 mole of Cu2+. Therefore, the moles of NaOH required can be calculated as follows:
Moles of NaOH = 2 * moles of Cu2+
Step 3: Calculate the volume of 3.0 M NaOH
The concentration of NaOH is given as 3.0 M, which means there are 3.0 moles of NaOH in 1 liter (1000 mL) of solution.
Using the formula:
Moles = Concentration (M) * Volume (L)
we can rearrange it to solve for volume:
Volume (L) = Moles / Concentration (M)
Since we want the volume in milliliters (mL), we can convert the final result to mL by multiplying the volume in liters by 1000.
Volume (mL) = Volume (L) * 1000
Step 4: Substitute the values and calculate the answer
Substitute the moles of NaOH obtained from step 2 into the formula to calculate the volume of 3.0 M NaOH required.
Volume (L) = (2 * moles of Cu2+) / 3.0 M
Volume (mL) = Volume (L) * 1000
By following these steps and plugging in the appropriate values, you'll be able to calculate the number of milliliters of 3.0 M NaOH required to react with 0.50 g of Cu2+.