What is thhe pH of 500mL of solution containing 0.0124 grams of Ca(OH)2?
0.0124/121.64= 1.02 x 10^-4g/mol
1.02 x 10^-4/ .5= 2.04 x 10^-4
2.04 x 10^-4*2=4.08x 10^-4
-log(4.08 x 10^-4)= 3.39
14-3.39=10.61
thank you so much!!!!!!
How many moles do you have?
moles = grams/molar mass.
Solve for moles and plug into
M = moles/L
Note that you have 2 OH^- for each Ca(OH)2; therefore, multiply the molarity by 2 to find concn OH, then pOH = -log(OH) and convert to pH.
Well, Ca(OH)2 is a base, so it's quite basic of it to hang around with such a crowd. Now, to calculate the pH, we need to know the concentration of hydroxide ions (OH-) in the solution. But don't worry, I've got this under control!
The molar mass of Ca(OH)2 is approximately 74.1 g/mol. With 0.0124 grams of Ca(OH)2, we can find the number of moles by dividing that by the molar mass.
0.0124 g / 74.1 g/mol = 0.000167 moles
Since Ca(OH)2 dissociates to produce two moles of OH- ions for every mole of Ca(OH)2, we can multiply the number of moles by 2 to find the number of moles of OH- ions.
0.000167 moles * 2 = 0.000334 moles of OH- ions
Now, the concentration of OH- ions can be found by dividing the number of moles by the volume of the solution in liters.
500 mL = 0.5 L
Concentration of OH- ions = 0.000334 moles / 0.5 L = 0.000668 M
Finally, pH is related to the concentration of H+ ions in the solution. Since this is a basic solution, we can approximate the pH using the pOH formula:
pOH = -log[OH-] = -log(0.000668) ≈ 3.175
And since pH + pOH = 14, we can calculate the pH:
pH = 14 - 3.175 ≈ 10.825
So, the pH of the solution is approximately 10.825. It's quite basic, just like my sense of humor!
To find the pH of a solution containing Ca(OH)2, we first need to determine the concentration of hydroxide ions (OH-) in the solution.
Step 1: Calculate the number of moles of Ca(OH)2.
Given that the mass of Ca(OH)2 is 0.0124 grams, we need to convert it to moles. The molar mass of Ca(OH)2 is approximately 74.093 grams/mol.
Number of moles of Ca(OH)2 = mass of Ca(OH)2 / molar mass of Ca(OH)2
Number of moles of Ca(OH)2 = 0.0124 g / 74.093 g/mol
Step 2: Calculate the concentration of hydroxide ions (OH-).
Since Ca(OH)2 dissociates in water to produce two moles of OH- for every mole of Ca(OH)2, we can multiply the number of moles of Ca(OH)2 by 2 to get the number of moles of OH-.
Number of moles of OH- = 2 * number of moles of Ca(OH)2
Step 3: Calculate the concentration of OH- in moles per liter (Molarity).
The volume of the solution is given as 500 mL, which can be converted to liters by dividing it by 1000.
Volume of solution = 500 mL / 1000 = 0.5 L
Concentration of OH- (Molarity) = Number of moles of OH- / Volume of solution
Step 4: Calculate the pOH of the solution.
pOH is defined as the negative logarithm (base 10) of the hydroxide ion concentration (OH-).
pOH = -log10(concentration of OH-)
Step 5: Calculate the pH of the solution.
pH is defined as 14 minus the pOH.
pH = 14 - pOH
Now, let's perform the calculations:
Step 1: Number of moles of Ca(OH)2 = 0.0124 g / 74.093 g/mol = 0.000167 moles
Step 2: Number of moles of OH- = 2 * 0.000167 moles = 0.000334 moles
Step 3: Concentration of OH- (Molarity) = 0.000334 moles / 0.5 L ≈ 0.000668 M
Step 4: pOH = -log10(0.000668) ≈ 3.175
Step 5: pH = 14 - 3.175 ≈ 10.825
Therefore, the pH of the solution containing 500 mL of solution and 0.0124 grams of Ca(OH)2 is approximately 10.825.
To determine the pH of a solution containing Ca(OH)2, we need to understand that this compound is a strong base that dissociates completely in water. When it dissolves, it releases hydroxide ions (OH-) into the solution.
First, let's calculate the amount of hydroxide ions (OH-) produced by 0.0124 grams of Ca(OH)2.
The molar mass of Ca(OH)2 is calculated as follows:
(1 atom of Calcium x atomic mass of Calcium) + (2 atoms of Oxygen x atomic mass of Oxygen) + (2 atoms of Hydrogen x atomic mass of Hydrogen)
= (1 x 40.08 g/mol) + (2 x 16.00 g/mol) + (2 x 1.01 g/mol)
= 40.08 g/mol + 32.00 g/mol + 2.02 g/mol
= 74.10 g/mol
Now, let's calculate the number of moles of Ca(OH)2:
Number of moles = Mass / molar mass
= 0.0124 g / 74.10 g/mol
= 0.000167 mol
Since Ca(OH)2 has a 1:2 ratio of calcium ions (Ca2+) to hydroxide ions (OH-), the number of moles of hydroxide ions produced is twice the number of moles of Ca(OH)2.
Number of moles of OH- ions = 2 x 0.000167 mol
= 0.000334 mol
Next, let's calculate the concentration of hydroxide ions in the solution. The concentration is the number of moles divided by the volume of the solution.
Concentration (molarity) = Number of moles / Volume
= 0.000334 mol / 0.5 L
= 0.000668 mol/L
Finally, let's calculate the pOH (negative logarithm of the hydroxide ion concentration) and then convert it to pH.
pOH = -log[H+]
pOH = -log(0.000668)
pOH ≈ 3.176
pH = 14 - pOH
pH = 14 - 3.176
pH ≈ 10.824
So, the pH of the solution is approximately 10.824.