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)
HC2H3O2 + NaOH ==> NaC2H3O2 + H2O
mols acetic acid = M x L = ?
Using the coefficients in the balanced equation, convert mols aceit acid to mols NaOH. You can see the ratio is 1:1.
Then M NaOH= mols NaOH/L NaOH.You know M and mols, solve for L and convert to mL.
2.
KHP + NaOH ==> NaKP + H2O
mols KHP = grams/molar mass
Using ther coefficients in the balanced equation, convert mols KHP to mols NaOH. Again, note the ratio is 1:1 for KHP to NaOH.
Then M = mols/L. You know mols NaOH and L NaOH, solve for M.
To calculate the number of mL of a NaOH solution required to neutralize a given volume of acetic acid solution, you need to use the concept of stoichiometry. Here's how you can solve the first question:
1) Write the balanced chemical equation:
NaOH(aq) + CH3COOH(aq) -> H2O(l) + CH3COONa(aq)
This equation tells you that for every 1 mole of NaOH, 1 mole of CH3COOH is required to react and produce 1 mole of water and 1 mole of CH3COONa.
2) Convert the given volume of acetic acid solution to moles:
0.15 M means that there are 0.15 moles of CH3COOH in 1 liter of solution. So, in 25.0 mL (0.025 L) of the solution, there would be:
0.15 mol/L x 0.025 L = 0.00375 moles of CH3COOH
3) Use the stoichiometry from the balanced equation to determine the moles of NaOH required:
From the balanced equation, we know that the ratio of NaOH to CH3COOH is 1:1. Therefore, we need 0.00375 moles of NaOH.
4) Convert moles of NaOH to volume (mL) of the NaOH solution:
0.095 M means that there are 0.095 moles of NaOH in 1 liter of solution. So, to convert moles to milliliters for a 0.095 M solution:
0.095 mol/L x (volume in L) = 0.00375 moles
Volume in L = 0.00375 moles / 0.095 mol/L = 0.039 L
Since 1 L is equal to 1000 mL, the volume in mL would be:
0.039 L x 1000 mL/L = 39 mL
Therefore, 39 mL of the 0.095 M NaOH solution is required to neutralize 25.0 mL of the 0.15 M acetic acid solution.
Now, let's solve the second question:
To calculate the molarity of the NaOH solution, you need to determine the number of moles of NaOH and the volume of the solution used to neutralize the KHP.
1) Write the balanced chemical equation:
NaOH(aq) + KHC8H4O4(aq) -> H2O(l) + KNaC8H4O4(aq)
This equation tells you that for every 1 mole of NaOH, 1 mole of KHC8H4O4 is required to react and produce 1 mole of water and 1 mole of KNaC8H4O4.
2) Convert the weight of KHP to moles:
The molar mass of KHP (KHC8H4O4) is needed to convert grams to moles. From the given mass of 0.50 g, we have:
0.50 g KHP x (1 mol KHP/204.22 g KHP) = 0.00245 moles of KHP
3) Use the stoichiometry from the balanced equation to determine the moles of NaOH:
From the balanced equation, we know that the ratio of NaOH to KHP is 1:1. Therefore, we need 0.00245 moles of NaOH.
4) Convert the volume of NaOH solution used to moles:
22.0 mL x (1 L/1000 mL) = 0.0220 L
5) Calculate the molarity of NaOH:
Molarity (M) = moles/volume in liters
Molarity = 0.00245 moles / 0.0220 L = 0.111 M
Therefore, the molarity of the sodium hydroxide solution is 0.111 M.