Calculate the pH of a 1.00 L buffer solution containing 0.143 mol of acetic acid (HC₂H₂O₂) and 0.180 mol of sodium acetate (NaC₂H₂O₂). The Ka of acetic acid is 1.8 × 10-5. pH = Calculate the pH of the buffer solution after 0.0315 mol of HCl is added to the buffer. Assume the volume of the solution does not change. pH = Calculate the pH after 0.0315 mol of HCl is added to 1.00 L of pure water. pH =

You take a 1.50 moles of strong acid HCl and a 1.00 moles strong base NaCl and combine them with a total volume of 1.00 Liter. What is the pH of the solution? What is the [OH-] of the solution? What is the [Cl-] in the solution? What is the [Na+] in the solution?

Calculate the pH of a buffer solution prepared by dissolving 0.78 mole of sodium fluoride (NaF) and 1.0 mole of hydrofluoric acid (HF) in enough water to make 1.0 liter of solution. [Ka(HF) = 6.8 x 10-4]

A chemist titrates 70.0 mL of a 0.7708 M propionic acid (HC₂H,CO₂) solution with 0.4296M KOH solution at 25 °C. Calculate the pH at equivalence. The pk of propionic acid is 4.89. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = 0

1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH:COON has been found to be 4.76. What will be the pH of this solution after 0.1 mole/litre HCI has been added to the buffer? Assume that the volume is unchanged. Ka = 1.75 x 105 2. A litre of solution containing 0.1 mole of CH;COOH and 0.1 mole of CH;COON provides a buffer of pH 4.74. Calculate the pH of solution after the addition of 0.02 mole NaOH. Ka = 1.8 x 105.

Phosphoric acid is a triprotic acid (?a1=6.9×10^3Ka1=6.9×10^3, ?a2=6.2×10^8 Ka2=6.2×10−8, and ?a3=4.8×10^13Ka3=4.8×10^13). Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH2PO4(s) and 30.0 g of Na2HPO4(s) in water and then diluting to 1.00 L. pH=

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

a An analytical chemist is titrating 86.1 mL of a 1.100M solution of hydrazoic acid (HN3) with a 0.7600M solution of KOH. The p K of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 74.4 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.

A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 3.00 mL of a 2.00 M solution of sodium hydroxide is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5.   What is the pH of the solution after adding NaOH?