How many milliters of 1.80M HCl are required to react with 30.0 grams of calcium hydroxide according to the given equation:
CA(OH)2(s) + 2HCl(aq)> CaCl2(aq) + 2H2O(l)
moles Ca(OH)2 = M x L = ??
Using the coefficients in the balanced equation, convert moles Ca(OH)2 to moles HCl. (It will be 2 x moles Ca(OH)2).
Then M HCl = moles HCl/L HCl
Solve for L HCl and convert to mL.
To determine the number of milliliters of 1.80M HCl required to react with 30.0 grams of calcium hydroxide (Ca(OH)2), we need to use the molar ratio from the balanced equation.
The molar mass of Ca(OH)2 is calculated as follows:
Ca: 40.08 g/mol
O: 16.00 g/mol (2 atoms)
H: 1.01 g/mol (2 atoms)
Total = 40.08 + (16.00 * 2) + (1.01 * 2) = 74.16 g/mol
Therefore, 1 mole of Ca(OH)2 weighs 74.16 grams.
To find the number of moles of Ca(OH)2 in 30.0 grams, we divide the mass by the molar mass:
30.0 g / 74.16 g/mol = 0.405 moles of Ca(OH)2
According to the balanced equation, 2 moles of HCl are required to react with 1 mole of Ca(OH)2. Therefore, we need twice the number of moles of HCl.
0.405 moles of Ca(OH)2 * 2 moles of HCl / 1 mole of Ca(OH)2 = 0.810 moles of HCl
Now we can find the volume of 1.80M HCl solution required to supply 0.810 moles of HCl. The concentration of HCl is given as 1.80 moles per liter (1.80M).
Using the formula: moles = volume (in liters) * concentration (in moles per liter)
0.810 moles = volume * 1.80 M
Rearranging the equation to solve for the volume:
volume = 0.810 moles / 1.80 M
volume = 0.450 liters
Finally, we need to convert the volume from liters to milliliters:
0.450 liters * 1000 mL/liter = 450 mL
Therefore, 450 milliliters of 1.80M HCl are required to react with 30.0 grams of calcium hydroxide.
To find out the amount of HCl required to react with 30.0 grams of calcium hydroxide (Ca(OH)2), we need to use stoichiometry and the balanced equation.
Step 1: Calculate the molar mass of Ca(OH)2.
The molar mass of Ca(OH)2 can be calculated by adding up the masses of one calcium atom (40.08 g/mol), two oxygen atoms (16.00 g/mol each), and two hydrogen atoms (1.01 g/mol each).
Molar mass of Ca(OH)2 = (40.08 g/mol) + 2(16.00 g/mol) + 2(1.01 g/mol) = 74.10 g/mol
Step 2: Convert the mass of Ca(OH)2 to moles.
To convert the mass of Ca(OH)2 to moles, divide the given mass by the molar mass.
30.0 g Ca(OH)2 × (1 mol Ca(OH)2/74.10 g Ca(OH)2) = 0.405 mol Ca(OH)2
Step 3: Use the stoichiometry of the balanced equation to determine the moles of HCl required.
From the balanced equation, we can see that each mole of Ca(OH)2 reacts with 2 moles of HCl. Therefore, the moles of HCl required will be twice the moles of Ca(OH)2.
0.405 mol Ca(OH)2 × 2 mol HCl/1 mol Ca(OH)2 = 0.810 mol HCl
Step 4: Calculate the volume of the HCl solution required.
To determine the volume of the HCl solution required, we need to use the given concentration of HCl (1.80 M). The molarity (M) is defined as moles of solute divided by liters of solution.
Molarity (M) = moles of solute/volume of solution (in liters)
Therefore, rearranging the equation: volume of solution (in liters) = moles of solute/Molarity
Volume of solution (in liters) = 0.810 mol HCl/1.80 M = 0.45 L
Step 5: Convert liters to milliliters.
Finally, we can convert the volume from liters to milliliters by multiplying by 1000.
0.45 L × 1000 mL/L = 450 mL
So, 450 milliliters of the 1.80 M HCl solution are required to react with 30.0 grams of calcium hydroxide.