A 30.0 mL sample of 0.165 M propanoic acid (Ka = 1.3x10^-5) is titrated with 0.300 M KOH. Calculate the pH at 10 mL of added base.

Calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer solution that is 0.2604 M in CH3CH2NH2 and 0.2404 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Kb=5.6⋅10^−4).

A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.150 M NaOH, requiring 16.00 mL to reach the equivalence point. During the titration, the pH after adding 4.00 mL NaOH was 6.912. Calculate Ka for the weak acid.

How many moles of hydrofluoric acid, HF, must be added to 150 mL of 0.17 M sodium fluoride to give a buffer of pH 3.15? Ignore the volume change due to the addition of hydrofluoric acid. (Ka for HF is 6.8 × 10¬4.) mol

A 50.00-mL sample of 0.250 M HC2H3O2 was titrated with 0.125 M NaOH. What is the pH of the resulting solution after 45.0 mL of NaOH were added at 25°C?  Ka for HC2H3O2 is 1.8x10–5 at 25°C

A certain weak acid, HAHA, with a KaKaK_a value of 5.61×10−65.61×10−6, is titrated with NaOHNaOH. A solution is made by titrating 8.00 mmolmmol (millimoles) of HAHA and 1.00 mmolmmol of the strong base. What is the resulting pH?   More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 47.0 mL ?

An analytical chemist is titrating 137.2 mL of a 0.2100M solution of butanoic acid (HC3H,CO2) with a 0.5300 M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 28.68 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 == 11 G

A 1.30 L buffer solution consists of 0.313 M propanoic acid and 0.190 M sodium propanoate. Calculate the pH of the solution following the addition of 0.069 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The K₂ of propanoic acid is 1.34 × 10-5. pH =

A 25 mL sample of 0.150 M monoprotic organic acid is titrated with aqueous sodium hydroxide. After 9.87 mL of 0.150 M NaOH is added, what is the pH of the solution? The Ka of the acid is 3.93 * 10^-5.

A student titrated 30.00 mL of a weak base solution, 0.150 M CH₃NH₂ (Kb = 4.40 × 10⁻⁴), with 0.100 M HCl solution. Calculate the pH at the equivalence point.