An aqueous solution contains 0.26 M NaCHO2 and 0.40 M HCHO2. What is the pH of the solution? HCHO₂ has K₂ = 1.8 x 10-4.

4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid used to prepare buffers for biological samples through combination with strong bases. How many mL of 0.626 M KOH should be added to 5.00g of MOBS (pKa=7.48 and formula mass is 223.29 g/mol) to give a pH of 7.40

Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3).  (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

A buffer, consisting of H₂PO4 and HPO42, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the buffer ingredients are 6.50 g of NaH2PO4 and 8.00 g of Na2HPO4 per 355 mL of solution? The Ka of H₂PO4 is 6.20 x 10-8.

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?

Calculate the pH of a buffer solution prepared by dissolving 0.400 mol of cyanic acid (HCNO) and 0.800 mol of sodium cyanate (NACNO ) in enough water to make 1.00 L of solution. The Ka of HCNO at 25° C is 2.00 x 10-4

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.

A solution is prepared that is initially 0.13M in acetic acid (HCH3CO₂) and 0.24M in potassium acetate (KCH3CO₂). 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 initial change final [HCH,CO₂] 0 [H₂0]. You can leave out the M symbol for molarity. [cH,co,] 0 L [H₂O] 0 0 0 plo X G

A solution contains 0.295 M potassium hypochlorite and 0.299 M hypochlorous acid (Ka The pH of this solution is = 3.50 × 10-8).

An analytical chemist is titrating 146.0 mL of a 1.200 M solution of benzoic acid (HC6H5CO₂) with a 0.6900 M solution of NaOH. The pK of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 46.25 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 ×