What ratio of NaCN to HCN is needed to prepare a pH 10.20 buffer? (Ka of HCN is 4.9 x 10-¹⁰)

How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 4.20? (Ka for HF is 6.8 × 10⁻⁴)

What is the pH of a buffer solution that is 0.214 M in ammonia and 0.390 M in ammonium chloride (NH4CI)? The Kü of ammonia is 1.8 x 10-5. (Two decimal places)

What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.120 mol of CH₃NH₃I?

What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.00 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)

A certain indicator, HA, has a K value of 2.0 x 10. The protonated form of the indicator is blue and the ionized form is red. What is the pK, of the indicator? pK = What is the color of this indicator in solution with pH = 3? about us careers privacy policy terms of use contact us help 949 PM XI 风下 3/10/202 edts f12 inse ho 立

What is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10-5) when 100.0 mL of a 0.0.75 M HCl solution is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ?Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.

What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.10 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)

You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M NH4Cl solution, what concentration of NH3 l will you need to also start with? (Kb for NH3 is 1.8x10-5)

Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL  after 0.158 g of NaOH was added? [Ka= 1.56 ×10-5] Report your answer with three decimals. Enter numbers only; do not enter units.