1)Calculate the number of mL of a 0.095 M NaOH solution required to neutralize 25.0 mL of 0.15 M acetic acid solution
2) Calculate the molarity of a sodium hydroxide solution if 22.0 mL of the sodium hydroxide is required to neutralize 0.50 g of KHP.
NaOH(aq)+ KHC8H4O4 -> H2O(l) + KNaC8H4O4(aq)
To solve these problems, we will use the concept of stoichiometry, which is the relationship between the quantities of reactants and products in a chemical reaction.
1) To calculate the number of mL of a NaOH solution required to neutralize the acetic acid solution, you need to use the balanced chemical equation and the concept of stoichiometry.
The balanced chemical equation for the reaction of NaOH and acetic acid is:
CH3COOH + NaOH -> CH3COONa + H2O
From the balanced equation, we can see that the stoichiometric ratio between NaOH and CH3COOH is 1:1. This means that one mole of NaOH reacts with one mole of CH3COOH.
First, let's calculate the number of moles of CH3COOH in 25.0 mL of the acetic acid solution:
moles CH3COOH = (volume in L) x (molarity)
moles CH3COOH = 0.025 L x 0.15 mol/L = 0.00375 mol
Since the stoichiometric ratio between NaOH and CH3COOH is 1:1, the number of moles of NaOH required to neutralize the acetic acid is also 0.00375 mol.
Now, let's calculate the volume of the NaOH solution using the molarity:
volume NaOH (in L) = (moles NaOH) / (molarity)
volume NaOH (in L) = 0.00375 mol / 0.095 mol/L = 0.03947 L
Finally, convert the volume from liters to milliliters:
volume NaOH (in mL) = 0.03947 L x 1000 mL/L = 39.47 mL
Therefore, 39.47 mL of the 0.095 M NaOH solution is required to neutralize 25.0 mL of the 0.15 M acetic acid solution.
2) To calculate the molarity of the sodium hydroxide (NaOH) solution, we will use the concept of stoichiometry and the information given in the problem.
From the balanced chemical equation, we can see that the stoichiometric ratio between NaOH and KHC8H4O4 (KHP) is 1:1. This means that one mole of NaOH reacts with one mole of KHP.
First, let's calculate the number of moles of KHP in 0.50 g:
moles KHP = (mass in grams) / (molar mass)
moles KHP = 0.50 g / (molar mass of KHP)
The molar mass of KHP (KHC8H4O4) can be calculated by adding up the atomic masses of each element in the compound, which are:
K (39.10 g/mol)
H (1.01 g/mol) x 4
C (12.01 g/mol) x 8
O (16.00 g/mol) x 4
molar mass of KHP = (39.10 g/mol) + (1.01 g/mol x 4) + (12.01 g/mol x 8) + (16.00 g/mol x 4)
Now, divide the mass of KHP by the molar mass to get the number of moles:
moles KHP = 0.50 g / (molar mass of KHP)
Next, because the stoichiometric ratio between NaOH and KHP is 1:1, the number of moles of NaOH required to neutralize KHP is equal to the number of moles of KHP.
Now, let's calculate the molarity of NaOH using the volume and number of moles:
Molarity of NaOH (in mol/L) = (moles NaOH) / (volume in L)
Molarity of NaOH (in mol/L) = moles NaOH / (22.0 mL x 0.001 L/mL)
Finally, divide moles NaOH by the volume in liters:
Molarity of NaOH (in mol/L) = moles NaOH / (22.0 mL x 0.001 L/mL)
Follow these steps to calculate the molarity of the sodium hydroxide solution.