. 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
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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 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate the concentration of HNO2 and its conjugate base in a 0.025 M HNO2 Solution. Please please show all work!
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.
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
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?