A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Calculate the pH of the solution upon addition of 47.2 mL of 1.00 M HCl to the original buffer. Express your answer using two decimal places.

A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. The ka of ammonia is 5.68 X 10-10.  The pKa of ammonia is 9.25.  These questions are challenging so this is very similar to the one online but the answers will be a little different.    What is the initial pH of the solution?     A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 15.0 mL of HCl is added?      Calculate the pH at the equivalence point.         Calculate the pHat one-half equivalence point.       A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 38.0 mL of HCl has been added?

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

You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF.  Find 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.

A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.

An analytical chemist is titrating 75.3 mL of a 0.2100M solution of cyanic acid (HCNO) with a 0.8800M solution of NaOH. The p K of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 20.9 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

Calculate the pH for each of the cases in the titration of 35.0 mL of 0.170 M LiOH(aq) with 0.170 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCI: after addition of 21.5 mL HC1: after addition of 45.5 mL HCl: after addition of 13.5 mL HCl: after addition of 35.0 mL HCl: after addition of 50.0 mL HC1: []

A 10.0mL solution of 0.720 M NH3 is titrated with a 0.240 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00mL, 10.0mL, 30.0mL, and 40.0mL. Be sure your answer has the correct number of significant digits. 0.00 mL added, pH = 10.0 mL added, pH = 30.0 mL added, pH = 40.0 mL added, pH =

An analytical chemist is titrating 103.5 mL of a 0.3300M solution of acetic acid (HCH₂CO₂) with a 0.3600M solution of KOH. The p K of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 22.84 mL of the KOH solution to it. a 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 = Ś 000 18 Ar

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 =