Calculate the pH of a buffer that was prepared by mixing 90 mL of a 0.01M aqueous hydrocyanic acid (HCN, Ka = 6.2 x 10-10) with 22 mL of 0.02 M aqueous potassium hydroxide (KOH)

You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa 4.20) and 0.240 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL

Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl   10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH   10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH   10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl   10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO

Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?