What is the pH of a buffer prepared by adding 5.80g of sodium nitrite to 150 mL of 0.15M nitrous acid( KA

pH = 3.73

Explanation:

Let's apply the Hendersson Hasselbah equation

pH = pKa + log [salt / acid]

HNO₂ → pKa = 3.16

Concentration of salt and acid must be M

Let's determine molarity of salt

5.80 g . 1 mol /68.99 g = 0.0840 moles of sodium nitrite

0.0840 mol / 0.150L of solution = 0.56 M

pH = 3.16 + log (0.56/0.15)

pH = 3.73

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d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong