A researcher wants to make a buffer of pH 4.60 using nitrous acid (Ka = 4.0 x 10^-4) and sodium nitrite.
a. Determine the approximate ratio of the two buffer compoents that she should use to get the desired pH.
b. Evaluate the researcher's decison to use the nitrous acid/nitrite buffering system.
A researcher wants to make a buffer of pH 4.60 using nitrous acid (Ka = 4.0...
2. (5 pts) A researcher wants to make a buffer of pH 4.60 using nitrous acid (K = 4.0 x 10-4) and sodium nitrite. a) Determine the approximate ratio of the two buffer components that she should use to get the desired pH. b) Evaluate the researcher's decision to use the nitrous acid/nitrite buffering system.
. The Ka of nitrous acid is 4.0 × 10−4. What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M nitrous acid and 45.0 mL of 1.25 M sodium nitrite? The answer is 3.45 Please show the solution. Thank you.
The nitrous acid/sodium nitrite conjugate pair has been chosen to prepare a buffer solution. What should the concentration ratio of NO2-/HNO2 be if the desired pH of this buffer is 4.00? (Ka of HNO2 = 4.27 x 10-4)
What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2) and 1.242 grams of sodium Nitrite (NaNO2), in 250ml of solution?(Ka of Nitrous acid = 4.5X10-4)
What is the pH of a buffer that is 0.95 M nitrous acid and 0.35 M sodium nitrite? (Ka = 4.5x10-4) OA. 3.23 OB. 4.24 OC. 2.91 OD. 3.78
A 1.00 L solution contains 22.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.96? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 23.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.36? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 15.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.66? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 20.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.56? Ka (HNO2) = 4.0 × 10–4.
An environmental researcher needs a carbonate buffer at pH 10.0 to study the effects of acid rain. How many grams of sodium carbonate must be added to 1.50 L of 0.200 M sodium bicarbonate to make a buffer if the Ka for sodium bicarbonate is 4.7x10-11?