You have 75.0 mL of 0.11 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka value of HA?

What is the pH of an aqueous solution made by mixing 300 mL of 0.10M hydrofluoric acid (pKa= 3.18) with 200 mL of 0.10M potassium hydroxide?

25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka of acetic acid is 1.8x10-5. What is the pH of the solution after adding NaOH?

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.

Given: A certain weak acid,HA with a Ka value of 5.61 •10-6 is tutorage's with NaOH.  part A: a solution is made by titration 7.00mmol of HA and 3.00 mmol of the strong base. What is the resulting pH? Part B: more strong base is added until the equivalence point is reached. What is the pH of this addition at the equivalence point if the total volume is 34mL?

Calculate the pH of a buffer solution that is 0.200 M in HCN and 0.120 M in NaCN.  The Ka of HCN is 4.90 x 10-10.

A patient presents itself to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 6.8 ×10-8 M    and bicarbonate ion (HCO3-)  2.325 ×10-7 M                                                                              Ka = 4.3 × 10-7                  H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?

TUTOR Analysis of a Weak Acid-Strong Base Titration Curve Determine the pH during the titration of 63.3 mL of 0.465 M formic acid (K₂ = 1.8×10) by 0.465 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 95.0 mL of KOH

When a strong base is added to buffer it will react to become neutralized. Determine the pH after 0.15 mol of OH- is added to a buffer consisting of 2.0 mol of HA and 1.0 mol of A-. (Ka = 5.8 x 10-10) HA + OH- → A- + H2O

Calculate the pH of a buffer solution that is 0.200 M in HCN and 0.120 M in NaCN. The Ka of HCN is 4.90 x 10-10.