A 0.75 g sample of X2CO3 is dissolved in water and 80 mL of 0.20 M CaCl2 solution is added.
This is the balanced equation I have created.
X2CO3(aq) + CaCl2(aq) → CaCO3(s) + 2 XCl(aq)
Based on the ratio in your balanced equation, how many moles of X2CO3 must have reacted? How many moles of CO32- is this?
I don't know how to start.
I know that the moles of each compound is the coefficient.
mols CaCl2 = M x L = ?
mols X2CO3 = mols CaCl2 from the 1:1 ratio.
mols (CO3)^2- = mols X2CO3 = mols CaCl2.
To find the number of moles of X2CO3 that reacted, we can use the molarity (M) and volume (V) of the CaCl2 solution added.
First, we need to convert the volume of the CaCl2 solution from milliliters (mL) to liters (L):
80 mL = 80/1000 L = 0.08 L
Now, we can use the equation:
Moles (X2CO3) = Molarity (CaCl2) × Volume (CaCl2 in liters)
Given:
Molarity (CaCl2) = 0.20 M
Volume (CaCl2) = 0.08 L
Moles (X2CO3) = (0.20 M) × (0.08 L)
Moles (X2CO3) = 0.016 mol
According to the balanced equation:
1 mole of X2CO3 reacts to form 1 mole of CO32-
Therefore, the number of moles of CO32- formed is also 0.016 mol.
To find the number of moles of X2CO3 that reacted, we can use the balanced equation you provided.
1 mole of X2CO3 reacts with 1 mole of CaCO3. Therefore, the moles of X2CO3 that reacted is the same as the moles of CaCO3 formed.
We can calculate the number of moles of CaCO3 formed using the given information:
Mass of X2CO3 = 0.75 g
Molar mass of X2CO3 = [you need to provide the molar mass]
Using the formula:
Moles of X2CO3 = Mass of X2CO3 / Molar mass of X2CO3
Next, we need to determine the number of moles of CO32- formed. From the balanced equation, we see that 1 mole of X2CO3 produces 1 mole of CO32-. Since X2CO3 is a 2:1 ratio with CO32-, the number of moles of CO32- is half the number of moles of X2CO3.
Number of moles of CO32- = Moles of X2CO3 / 2
Hope this helps!