If you had 500.0 ml of a 0.10 M solution of HCLO, what mass of the corresponding Na+ (sodium salt) of the conjugate base would you need to make the buffer?
Use the Henderson-Hasselbalch equation.
I did ...I don't think am setting it up right.
also the answer says that it is 2.4 grams of the Naclo...
how do i set that up?
To find the mass of the corresponding sodium salt of the conjugate base required to make the buffer, we need to calculate the number of moles of the acid in the initial solution, and then use the stoichiometry of the reaction to determine the number of moles of the conjugate base.
1. First, calculate the number of moles of HCLO (the acid) in the initial solution.
Number of moles = Molarity × Volume (in liters)
Number of moles = 0.10 M × 0.500 L
2. Once you have the number of moles of HCLO, use the stoichiometry of the balanced equation to determine the number of moles of the conjugate base (sodium salt). In this case, sodium chloride (NaCl) is formed as the conjugate base of HCLO.
The balanced equation of HCLO and NaCl:
HCLO + NaOH = H2O + NaCl
From the equation, we see that 1 mole of HCLO reacts with 1 mole of NaCl. Therefore, the number of moles of NaCl will be the same as the number of moles of HCLO.
3. Convert moles of NaCl to grams by multiplying the number of moles by the molar mass of NaCl.
Molar mass of NaCl: 58.44 g/mol
Mass of NaCl = Number of moles × Molar mass
= moles of HCLO × Molar mass of NaCl
Now you have the mass of the corresponding sodium salt (NaCl) required to make the buffer.