I did an experiment were I added some water and KHP into a beaker and phenophalene [sp?]. It was a titration lab. We slowly added calciuum hydroxide into the beaker and waited till the solution turned into a faint pink. The question is asking me to find the number of mols of calcium hydroxide used to neutralize the KHP. Can I just convert the number of mL of calcium hydroxide I used into grams. I was thinking that 1 mL = 1 gram. And then after just find the molar mass and divide.
You don't need to do that.
moles = M x L or
millimiles = M x mL.
Just remember that you probably will be asked for the moles KHP and to do that you must convert from moles Ca(OH)2 to moles KHP with the equation,
2KHP + Ca(OH)2 ==> 2H2O + CaK2P2
So obviously, moles KHP = 2 x moles Ca(OH)2
but M is in grams/mol.d When I said M I meant molar mass not molarity.
I repeat. If you want moles, it is M x L.
True, M is molarity and since M = moles/L, then M x L = moles.
I assume you have the molarity of the Ca(OH)2. And of course you may convert mL Ca(OH)2 to grams but chemicals react by moles and not grams. By the way, that CaK2P2 I wrote would better be written as K2P + CaP.
We weren't given the molarity of Ca(OH)2, that's why I don't understand how to do the question.
Were you given grams? Then grams/molar mass = moles Ca(OH)2. Then moles/L = M.
You don't have enough information so far to convert mL into grams. And you may not assume that 1 mL 1 gram unless that was the actual mass Ca(OH)2 used. You may have done the experiment to determine the molarity of the Ca(OH)2 in which case you would need the mass of the KHP used. If that's the case, mass KHP/molar mass KHP moles. Then 1/2 that is moles Ca(OH)2. Then M Ca(OH)2 = moles/L in the titration.
To find the number of moles of calcium hydroxide used to neutralize the KHP, you cannot simply convert the volume of calcium hydroxide used into grams.
Here's how you can approach the problem step by step:
Step 1: Balanced Chemical Equation
Start by writing the balanced chemical equation for the reaction between calcium hydroxide (Ca(OH)2) and potassium hydrogen phthalate (KHP). The balanced equation is as follows:
Ca(OH)2 + KHP → H2O + CaK(C8H4O4)2
This equation tells us that one mole of calcium hydroxide reacts with one mole of KHP.
Step 2: Determine the Concentration of Calcium Hydroxide
Next, you need to determine the concentration of the calcium hydroxide solution you used in the titration. The concentration is typically provided in units of moles per liter (M).
Step 3: Calculate the Volume of Calcium Hydroxide Used
Using the balanced equation and the stoichiometry of the reaction, you can relate the volume of calcium hydroxide used (in liters) with the number of moles of KHP neutralized.
Step 4: Convert the Volume of Calcium Hydroxide to Moles
Now, convert the volume of calcium hydroxide used to moles by multiplying it by the concentration of the calcium hydroxide solution, which is given in moles per liter.
Step 5: Determine the Molar Mass of Calcium Hydroxide
To find the number of grams of calcium hydroxide used, you need to know the molar mass of calcium hydroxide. The molar mass is calculated by adding up the atomic masses of each element present in the compound.
Step 6: Calculate the Number of Moles of Calcium Hydroxide
Divide the mass of calcium hydroxide used (in grams) by the molar mass of calcium hydroxide to calculate the number of moles used.
By following these steps, you will be able to accurately calculate the number of moles of calcium hydroxide used to neutralize the KHP in your titration lab.