A 1.00 L solution contains 19.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.86? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 19.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.86? Ka (HNO2) = 4.0 × 10–4.
Chapter9: Acids, Bases, And Salts
Section: Chapter Questions
Problem 9.116E
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A 1.00 L solution contains 19.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.86? Ka (HNO2) = 4.0 × 10–4.
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