How many mL of 0.225M HCl would be required to titrate 6.00 grams of KOH?
To determine the amount of HCl required to titrate 6.00 grams of KOH, we need to use the stoichiometric ratio between HCl and KOH.
The balanced chemical equation for the reaction between HCl and KOH is:
HCl + KOH → KCl + H2O
From the balanced equation, we see that the ratio between HCl and KOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of KOH.
Step 1: Calculate the molar mass of KOH.
K (39.10 g/mol) + O (16.00 g/mol) + H (1.01 g/mol) = 56.11 g/mol
Step 2: Convert the given mass of KOH to moles.
6.00 g KOH × (1 mol KOH / 56.11 g KOH) = 0.107 mol KOH
Step 3: Since the reaction is 1:1, the moles of HCl required would also be 0.107 mol.
Step 4: Calculate the volume of 0.225M HCl solution needed using the molarity and the moles of HCl derived in step 3.
volume (L) = moles / molarity
volume (L) = 0.107 mol / 0.225 mol/L
volume (L) = 0.476 L
Step 5: Convert the volume from liters to milliliters.
volume (mL) = 0.476 L × 1000 mL/L
volume (mL) = 476 mL
Therefore, 476 mL of 0.225M HCl would be required to titrate 6.00 grams of KOH.
To calculate the volume of HCl required to titrate a certain amount of KOH, we need to use the concept of stoichiometry and the balanced chemical equation for the reaction between HCl and KOH.
The balanced chemical equation for the reaction is:
HCl + KOH → KCl + H2O
From the balanced equation, we can see that the ratio of HCl to KOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of KOH.
Step 1: Convert the mass of KOH to moles.
To do this, we need to know the molar mass of KOH, which consists of potassium (K), oxygen (O), and hydrogen (H). The molar mass of KOH is calculated by adding up the atomic masses of each element:
(1 x molar mass of K) + (1 x molar mass of O) + (1 x molar mass of H)
The atomic masses for K, O, and H are found on the periodic table. Adding them up will give us the molar mass of KOH.
Step 2: Find the number of moles of HCl required to react with the calculated moles of KOH.
Since the balanced equation tells us that the ratio of HCl to KOH is 1:1, the number of moles of HCl required will be equal to the number of moles of KOH.
Step 3: Calculate the volume of HCl using the molarity of the HCl solution.
The formula to calculate the volume of a solution is:
Volume (in liters) = moles / molarity
In this case, we have the number of moles of HCl from step 2, and we are given the molarity of the HCl solution (0.225 M). We can use this information to calculate the volume of HCl in liters.
Step 4: Convert the volume from liters to milliliters.
Since the question asks for the volume in milliliters, we need to convert the volume from liters to milliliters. There are 1000 milliliters in one liter, so we can multiply the calculated volume by 1000 to convert it to milliliters.
By following these steps, we can calculate the volume of the 0.225 M HCl solution required to titrate 6.00 grams of KOH.
KOH + HCl ==> KCl + H2O
moles KOH = grams/molar mass. Solve for moles.
moles HCl = moles KOH because the equation is 1:1.
moles HCl = M x L. Solve for L.