Two acids are mixed in solution: 0.20 M of HBr and 1.50 M of HBRO (Ka = 2.3 x 10-9). What is the resulting pH?

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 solution is prepared that contains 25.0 mL pyridine, C5H5N, d = 0.978 g/ml and 27.6 g pyridinium hydrochloride, C5H5N • HCl. The volume of the aqueous solution is 250. mL. What is the pH of this buffer solution? (K₁ C5H5N = 1.5 × 10 %) A) 4.68 B) 5.17 C) 5.29 D) 8.82 E) 8.71 ||

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

A buffer solution is prepared by dissolving 0.10 mol of acetic acid and 0.10 mol of sodium acetate in 1 L of solution. A 10-mL portion of 1 M HCl is then added to the solution. How much does the addition change the pH of the buffer? [Ka (CH3COOH) = 1.8 x 10-5]

The pKa of the weak acid HA is 4.49. If 0.17 mL of a 1.00 M solution of hydrochloric acid are added to a solution made by mixing 20.00 mL of 0.100 M HA and 10.00 mL of 0.100 M NaOH, what is the pH of the solution after the acid is added?

A buffer solution is prepared by dissolving  1.700 g of ammonium chloride (NH4Cl) into 100.00 mL of a  0.170 M solution of ammonia (NH3). The Kb of ammonia is 1.8 x 10−5.  What is the pH of the solution?

We have 500.0 mL of a buffer solution that is 0.697 M in NH3 and 0.380 M in NH4Cl. We add 500.0 mL of a solution 0.202 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?

b) What is th 1 с E 10. If a 50.0-mL sample of 0.250 M NaCN is titrated by 0.250 M HCI (strong acid), what is the pH of the solution at the equivalence point? Ka of Hydrocyanic Acid (HCN) at 25 °C is 6.2 x10-10. Hydrocyanic acid ce reacts with water to produce hydronium and cyanate.

A buffer solution is 0.463 M in H3PO4 and 0.210 M in KH₂PO4. If K₁1 for H3PO4 is 7.5 × 10-³, what is the pH of this buffer solution? pH =