If 0.694 grams of pure KHP are needed to exactly neutralize 30.5 mL of a calcium hydroxide solution, what is the concentration (in molarity) of the base solution?
2KHP + Ca(OH)2 ==> 2H2O + Ca(PK)2
moles KHP = grams/molar mass
Convert moles KHP to moles Ca(OH)2 (multiply by 2).
M Ca(OH)2 = moles Ca(OH)2/L Ca(OH)2.
To find the concentration of the calcium hydroxide solution, we need to use the concept of molarity. Molarity is defined as the number of moles of solute per liter of solution.
In this case, the solute is the calcium hydroxide (Ca(OH)2) and the solution is the calcium hydroxide solution.
First, we need to calculate the number of moles of KHP used to neutralize the solution.
The molar mass of KHP (potassium hydrogen phthalate) is approximately 204.23 g/mol.
Given that 0.694 grams of KHP is used, we can calculate the number of moles of KHP:
moles of KHP = mass of KHP / molar mass of KHP
moles of KHP = 0.694 g / 204.23 g/mol
Now, we need to calculate the number of moles of calcium hydroxide (Ca(OH)2) present in the solution.
From the balanced chemical equation for the reaction, we know that the stoichiometric ratio between KHP and Ca(OH)2 is 1:2. This means 1 mole of KHP reacts with 2 moles of Ca(OH)2.
So, moles of Ca(OH)2 = 2 * moles of KHP
Next, calculate the volume of the calcium hydroxide solution in liters:
volume of solution (L) = 30.5 mL / 1000 mL/L
Finally, we can find the concentration of the calcium hydroxide solution:
concentration (molarity) = moles of Ca(OH)2 / volume of solution (L)
By plugging in the values, you can calculate the concentration (in molarity) of the base solution.