A litre of solution containing 0.1 mole of CH3COOH and 0.1 mole of CH3COONa provides a buffer of pH 4.74. Calculate the pH of solution after the addition of 0.02 mole NaOH. Ka = 1.8 × 10– 5.

An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH, with a 0.5300M 2 solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 42.4 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = | ?

Calculate the pH of a 1.07 M solution of a weak acid, AH, for instance CH3COOH, and 0.62 M of a salt derived by its conjugate base, ANa, like CH3COONa. The acid dissociation constant, Ka , is 2.27e-6. What is the pH if 38 mL of 0.149 M of a strong acid, like HCl, is added to 100 mL of the buffer solution? What if a strong base, like NaOH, is added with the same ammount instead ?   pH      ← please insert your values   Add acid     = _______   Add base     = _________

A buffer is made by adding 0.300 mol HC:H:Oz and 0.300 mol NaC:H»O2 to enough water to make 1.00 L of solution. Ka for acetic acid is 1.8 × 105. 3. Calculate the pH after 5.0 ml of 4.0 M NaOH is added. 4. Calculate the pH after 5.0 mL of 4.0 M HCl is added.

An analytical chemist is titrating 213.4 mL of a 0.3200M solution of butanoic acid (HC,H,CO,) with a 0.6400M solution of NaOH. The p K of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 115.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0

An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ||

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.

Calculate the pH of a buffered solution that is 0.100 M in C6H5COOH (Ka = 6.4 x 10–5) and 0.100 M in C6H5COONa

45.0 mL of a buffer solution contains 0.20 M CH₂COOH and 0.25 M CH₂COONa. What is the pH of the mixture after 18.0 mL of 0.45 M HCI is added to this buffer solution? Ka of CH₂COOH = 1.8 x 105.

Calculate the pH of a buffer prepared by dissolving 0.80 moles acetic acid (CH3COOH) and 0.40 moles of sodium acetate (CH3COONa) in enough water to make 1500 mL of buffer solution. The pKa for acetic acid is 4.74