If you have 500 mL of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of the conjugate base do you need to make the buffer with a pH of 7.74 (assuming no change in volume)

5.90g of NaClO are needed

Explanation:

Assuming the weak acid is HClO pKa = 7.54

To solve this question we must use the H-H equation for acids:

pH = pKa + log [A-] / [HA]

Where pH is the pH we want = 7.74

pKa is pKa of the weak acid = 7.54

[A-] could be taken as the moles of the conjugate base (Moles NaClO) and [HA] moles weak acid = 0.500L * (0.10mol/L) = 0.0500 moles HClO

Replacing:

7.74 = 7.54 + log [NaClO] / [0.0500 moles]

0.20 = log [NaClO] / [0.0500 moles]

1.5849 = [NaClO] / [0.0500 moles]

Moles NaClO = 0.0792 moles

The mass is: -Molar mass NaClO = 74.44g/mol-

0.0792 moles * (74.44g / 1mol) =

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explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)