An aqueous solution of volume 2.30 L is prepared from 0.15 mol of KF and 0.25 mol of HF. The pH of the solution is (Ka HF = 6.8 x 10-4)
A. 11.06
B. 1.97
C. 3.38
D. 12.03
E. 2.95
An aqueous solution of volume 2.30 L is prepared from 0.15 mol of KF and 0.25...
Calculate the pH of a 1.0-L aqueous solution containing 0.40 mol of HF and 0.10 mol of HCl. (Ka for HF = 6.8 x 10?4) 0.40 1.0 0.016 2.6 1.4 x 10?3
Calculate the pH of a buffer solution prepared by dissolving 1.79 mol of HF and 2.26 mol of NaF in water to make a total volume of 1.25 L of solution. The Ka of HF is 6.8*10^-4. A) 3.57 B) 3.47 C) 3.27 D) 3.37 E) 3.68 Please let me know what answer is correct and how to work it. Thank You!
Consider a solution which is 0.10 M in HF and 0.15 M in KF. If 0.10 moles of NaOH is added to the solution, which of the following is true? The Ka for HF is 3.5 x 10-4 (at 25ºC) Group of answer choices The pH of the solution will not change. The buffer capacity of the solution will be exhausted. The pH of the solution will decrease. The Ka of HF will decrease.
Part B: A 50.0 mL volume of 0.15 mol L−1 HBr is titrated with 0.25 mol L−1 KOH. Calculate the pH after the addition of 14.0 mL of KOH. Express your answer numerically. Part C: A 75.0 mL volume of 0.200 mol L−1 NH3 (Kb=1.8×10−5) is titrated with 0.500 mol L−1 HNO3. Calculate the pH after the addition of 28.0 mL of HNO3. Express your answer numerically. Part D: A 52.0 mL volume of 0.350 mol L−1 CH3COOH (Ka=1.8×10−5) is...
Calculate the pH of a solution that is 0.25 M KF and 0.20 M HF. (Given: Ka (HF)-6.8x 10-4) O A. 3.26 O B. 3.36 O C. 3.46 D. 10.45 E. 10.64
calculate ph 7. A buffer solution prepared by adding 0.25 mol NaAc and 0.05 mol of HAC to enough v ater to make a total volume of 500 ml. Ka-1.8 x 10-5
Find the pH of a solution prepared from 1.0 L of a 0.15 M solution of Ba(OH)2 and excess Zn(OH)2(s). The Ksp of Zn(OH)2 is 3×10−15 and the Kf of Zn(OH)2−4 is 2×1015.
A buffer is prepared by adding 0.15 mol of lactic acid, CH3CHOHCOOH, and 0.20 mol of sodium lactate, Na+CH3CHOHCOO - , to sufficient water to make 1.0 L of buffer solution. The Ka of lactic acid is 1.4 x 10 - 4. Calculate the pH of the buffer.
A 25-mL solution of 0.25 M HF (Ka =7.1 x 10-4) is titrated with a 0.15 M solution of NaOH. Determine the pH of the solution at the equivalence point. Select one: a. 5.94 b. 10.8 c. 8.90 d. 8.60 e. 8.06
A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of the final solution? The Ka of hydrofluoric acid is 6.8 x 10-4.