For the chemical reaction, sodium hydroxide + copper (II) chloride = "robin's egg blue" precipitate, do the following: write the balanced molecular, balanced total ionic, and balanced net ionic equations; determine the Limiting Reactant (LR) for each chemical reaction, assuming that the concentration of each solution is 0.500M and the volume of each solution is 50.00mL; determine the theoretical yield of the product of interest; and, determine the actual yield of the product of interest if the percent yield was found to be 87.3%.
Give me some indication of what you know about this. This is a "keep you busy for the next hour" problem.
To answer your question and perform the necessary calculations, we will follow several steps. Here is a breakdown of how to get the answer:
Step 1: Write the Balanced Molecular Equation
First, you'll need to write the balanced molecular equation for the reaction.
The molecular equation for the reaction between sodium hydroxide (NaOH) and copper (II) chloride (CuCl2) is:
2 NaOH + CuCl2 -> Cu(OH)2 + 2 NaCl
This equation shows the reactants (NaOH and CuCl2) on the left side, and the products (Cu(OH)2 and NaCl) on the right side of the arrow.
Step 2: Write the Balanced Total Ionic Equation
Next, you'll need to write the balanced total ionic equation.
In the total ionic equation, all soluble ionic compounds are written as separate ions. Only compounds that are in the solid, liquid, or gas form are retained as formulas.
The total ionic equation for the reaction is:
2 Na+(aq) + 2 OH-(aq) + Cu2+(aq) + 2 Cl-(aq) -> Cu(OH)2(s) + 2 Na+(aq) + 2 Cl-(aq)
In this equation, the aqueous ions (Na+ and Cl-) are shown separately, while the solid Cu(OH)2 is shown as a formula.
Step 3: Write the Balanced Net Ionic Equation
To write the balanced net ionic equation, you'll need to remove the spectator ions, which are the ions that do not participate in the reaction. In this case, the spectator ions are Na+ and Cl-.
The net ionic equation for the reaction is:
2 OH-(aq) + Cu2+(aq) -> Cu(OH)2(s)
Here, only the ions that react are shown in the equation, which are 2 hydroxide ions (OH-) and 1 copper (II) ion (Cu2+).
Step 4: Determine the Limiting Reactant (LR)
To determine the limiting reactant, we need to compare the stoichiometry of the reactants based on the balanced molecular equation. The limiting reactant is the one that is completely consumed and determines the maximum amount of product that can be formed.
In this case, we have NaOH and CuCl2 as the reactants. You mentioned that the concentration of each solution is 0.500M and the volume of each solution is 50.00mL. To determine the moles of each reactant, we can use the formula:
moles = concentration * volume
For NaOH:
moles of NaOH = 0.500 M * 0.050 L = 0.025 moles
For CuCl2:
moles of CuCl2 = 0.500 M * 0.050 L = 0.025 moles
Comparing the stoichiometry of the balanced molecular equation, we can see that 2 moles of NaOH react with 1 mole of CuCl2. Since we have an equal number of moles for both reactants (0.025 moles), neither of them is in excess. Therefore, there is no limiting reactant in this case.
Step 5: Determine the Theoretical Yield
To determine the theoretical yield, we need to convert the moles of the limiting reactant (which is zero in this case) to moles of the product (Cu(OH)2), using the stoichiometry from the balanced molecular equation.
Since there is no limiting reactant, the theoretical yield cannot be determined. Theoretical yield is the maximum amount of product that can be formed based on stoichiometry and assuming 100% reaction efficiency.
Step 6: Determine the Actual Yield
To determine the actual yield of the product, we need to know the percent yield. You mentioned that the percent yield was found to be 87.3%. Percent yield is calculated using the formula:
percent yield = (actual yield / theoretical yield) * 100
In this case, the percent yield is given as 87.3%. Let's assume that the theoretical yield is "x" grams.
87.3 = (actual yield / x) * 100
Solving this equation for the actual yield, we get:
actual yield = (87.3/100) * x
Step 7: Calculate the Mass of the Actual Yield
To calculate the mass of the actual yield, we need to know the molar mass of the product Cu(OH)2.
Cu(OH)2 has a molar mass of approximately 97.56 g/mol.
Mass of the actual yield = (actual yield / 100) * molar mass of Cu(OH)2
Step 8: Calculate the Actual Yield
Using the mass of the actual yield and the given percent yield, we can calculate the actual yield.
actual yield = mass of the actual yield * percent yield / 100
By following these steps, you should be able to answer all the questions posed. I hope this explanation helps you understand the process.