A buffer solution was prepared by mixing 250.0 mL of 0.150 M HCH₂O (Ka = 1.8 x 104) with 100.0 mL of 0.200 M NaCH₂O. What would be the minimum mass (g) of NaOH (molar mass = 39.99 g/mol) to destroy this buffer?

Explain the role of a buffer, such as an antacid table or sodium bicarbonate, on the pH of a solution ( like blood)

For this question Find  the initial pH of 0.2000 L of buffer solution that is 0.165 M acetic acid and 0.145 M sodium acetate, and calculate the pH after the addition of 16.00 mL of 0.650 M potassium hydroxide.

A buffer solution contains 0.207 M CH3NH3Cl and 0.499 M CH3NH2 (methylamine). Determine the pH change when 0.101 mol HNO3 is added to 1.00 L of the buffer.

Determine the total buffer concentration ([HA] + [A-]) when 16.4 ml of 1.01 M acetic acid are mixed with 20.0 ml of 0.634 M sodium acetate and made to volume in a 200.0 ml volumetric flask.

A buffer solution contains 0.455 M KH,PO, and 0.295 M Na,HPO4. Determine the pH change when 0.091 mol KOH is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =

Calculate buffer pH after adding strong acid or strong base. Determine the pH change when 0.063 mol HBr is added to 1.00 L of a buffer solution that is 0.364 M in CH3COOH and 0.243 M in CH3COO pH after addition - pH before addition = pH change

2. Please help me answer all parts to this chemistry question:

Image

1. If 0.750 mole of HF is added to 450.0 ml of 0.250 M Ca(OH)2, is a buffer present?