What mass (g) of KHP is required to neutralize 10.00 mL of 0.1092 M NaOH?
mols NaOH = M x L
mols NaOH = mols KHP
mols KHP = grams/molar mass. You know mols and molar mass, solve for grams.
1.889g thanks Dr. Bob :)
I don't get 1.889 g KHP.
mol NaOH = 0.01 x 0.1092 =0.001092
mols KHP = 0.0001092.
mols KHP = grams KHP/molar mass KHP or
g KHP = mols KHP x molar mass KHP
= 0.0001092 x 204.22 = about 0.2230 g KHP.
To determine the mass of KHP required to neutralize the given volume and concentration of NaOH, we can use the concept of stoichiometry.
Here's how you can approach the problem step-by-step:
Step 1: Write the balanced chemical equation between NaOH and KHP:
NaOH + KHC8H4O4 (KHP) → H2O + KNaC8H4O4
Step 2: Determine the molar ratio between NaOH and KHP:
According to the balanced equation, the stoichiometric ratio between NaOH and KHP is 1:1. This means that 1 mole of NaOH reacts with 1 mole of KHP.
Step 3: Calculate the number of moles of NaOH:
To determine the number of moles of NaOH, we can use the formula:
moles = concentration × volume
moles = 0.1092 M × 10.00 mL
Note: Since the concentration is given in M (moles per liter) and the volume is given in milliliters, it's important to make sure the units are consistent. To do this, convert the volume from milliliters to liters by dividing by 1000.
Step 4: Convert the moles of NaOH to moles of KHP:
Since the stoichiometric ratio between NaOH and KHP is 1:1, the number of moles of NaOH is also equal to the number of moles of KHP required to neutralize it.
Step 5: Convert the moles of KHP to mass:
To calculate the mass of KHP, you need to multiply the number of moles of KHP by its molar mass. The molar mass of KHP (potassium hydrogen phthalate) is 204.23 g/mol.
mass = moles × molar mass of KHP
By following these steps, you can solve the problem and find the mass of KHP required to neutralize 10.00 mL of 0.1092 M NaOH.