3. Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25? For the best choice, calculate the ratio of the conjugate base to the acid required to attain the desired pH.
Chlorous acid pKa = 1.95
Nitrous acid pKa = 3.34
Formic acid pKa = 3.74
Hypochlorous acid pKa = 7.54
3. Which acid would you choose to combine with its sodium salt to make a solution...
Question 2: A) Calculate the pH of the buffer that results from mixing 56.1 mL of a 0.406 M solution of HCHO2 and 11.9 mL of a 0.606 M solution of NaCHO2. The Ka value for HCHO2 is 1.8×10−4 B) Calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 300.0 mL of a buffer solution that is 0.225 M in HCHO2 and 0.280 M in KCHO2 C) Calculate the initial pH and the final pH...
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 2.06 (assuming no change in volume)? chlorous acid (HClO2HClO2), pKa=1.95 I get 2.89g. Not correct.
If you have 500.0 mL of a 0.30 M solution of the acid, what mass of the corresponding sodium salt of the conjugate base do you need to make the buffer? Hypochlorous acid (HClO) = 7.54 pKa
If you have 500 mL of a 0.10 MM 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 3.14 (assuming no change in volume)? nitrous acid (HNO2), pKa=3.34 Express the mass to two significant figures and include the appropriate units.
A solution buffered at pH 3.90 is needed for a reaction. Would formic acid (HCOOH = HA) and its salt, sodium formate, NaHCO2 = NaA), make a good choice for this buffer? If so, what ratio of moles of A- and HA is needed? Use the Henderson Hasselbalch Equation. Ka formic acid = 1.8 x 10-4
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 7.35 (assuming no change in volume)? Express the mass to two significant figures and include the appropriate units. Acid is HCLO Pka = 7.54
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
You wish to make a buffer solution at a pH 9.56 with the weak acid HCN (Ka = 6.9 x 10-10 ) and its salt, NaCN..What ratio of the concentration of conjugate base to the acid: ([A- ]:[HA]) is required to attain the desired pH? a. [A- ] is 2.5 × that of [HA] b. [A- ] is 5 × that of [HA] c. [A- ] is 1 × that of [HA] d. [A- ] is ½ × that of...
The pKa is 7.54. Acid is HClO. Part B 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 7.68 (assuming no change in volume)? Express the mass to two significant figures and include the appropriate units. TI MÅ ? 0 2 Units m= | Value m =
You combine 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4 what is the pH of the solution? With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4. You add 8g sodium hydroxide to this solution, what is the new pH? With the same initial solution of 0.75 moles formate and 0.85 moles...