Calculate the pH of a solution that is made by combining 55 mL of 0.060 M hydrofluoric acid with 125 mL of 0.120  sodium fluoride.

Buffer 2 will be 150 mL of 0.15 M Tris-HCl buffer with a pH of 8.5 Write out the chemical equation for this buffer. Identify which species is the conjugate acid and conjugate base.

The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 3.50? mass= Based on this information, what volume of acid should the student measure to make the buffer solution? volume = g ml.

A chemist titrates 210.0 mL of a 0.4409M hypochlorous acid (HCIO) solution with 0.7835M NaOH solution at 25 °C. Calculate the pH at equivalence. The pK, of hypochlorous acid is 7.50. 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 NAOH solution added. pH = ] ?

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH 4Cl with 200.0 mL of 0.32 M NH 3. The K b for NH 3 is 1.8 × 10 -5.     10.55     9.14     9.58     12.42     4.74

A 2.00 L solution contains 0.545 M NH3 and 0.641 M NH4A.  (The Kb of NH3 is 1.86⋅10−51.86⋅10-5). What is the pH of this solution?   What is the pH of this solution after 0.121 mol of HCl are added to the solution?   What is the pH of this solution after 0.242 mol of HCl are added to the solution?

Classify the following solutions as one of these types AND calculate the pH: strong acid, strong base, weak acid, weak base, buffer, neutral salt. a) 0.040 M NaF (Ka for HF = 7.2 x 10-4) b) 10 M HClO4 c) A solution made by mixing 10.0 mL of 0.072 M NaOH with 15.0 mL of 0.100 M acetic acid (pKa for acetic acid = 4.75) d) 0.453 M NaCl

A solution is prepared that is initially 0.45M in pyridine (CÂHÂN), a weak base, and 0.50M in pyridinium bromide (C5H₁NHBr). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [où¯]. You can leave out the symbol for molarity. initial change final [C,H,N] [C₂H₂NH*] [OH-] 0 0 0 0 DO X Ar

Calculate the pH of the solution that results following addition of 30 mL of 1 M NaOH to 40 mL of 1 M NH4Cl.

An analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M solution of HNO3 . The pKb of ammonia is 4.74 . Calculate the pH of the base solution after the chemist has added 31.6mL of the HNO3 solution to it.   Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.   Round your answer to 2 decimal places.