What is the pH of the mixture made by adding 75.0 mL of 0.15 M NaF, 100.0 mL of 0.12M HF and 75.0 mL of 0.10 M KOH?
What is the pH of the mixture made by adding 75.0 mL of 0.15 M NaF,...
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.
4. What is the pH of a 100.0 mL buffer solution containing 0.15 M NaHCO3 and 0.15 M Na2CO3? 5. What is the pH after adding 15.0 mL of 0.10 M NaOH to the solution in question 4?
8. What is the pH of a solution made by mixing 29.00 mL of 0.15 M acetic acid with 39.00 mL of 0.15 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 x 10-5 for CH3CO2H.
7. What is the pH of a solution made by mixing 29.00 mL of 0.15 M acetic acid with 29.00 mL of 0.15 M KOH? Assume that the volumes of the solutions are additive. Ka= 1.8 x 10-5 for CH3CO2H oka-loa 8x10
27. Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCI(aq) to 150.0 mL of water at 25.0°C A) 0.70 B) 1.00 C) 1.18 D) 1.30 E) 13.0 Ans: D 28. A mixture is made by adding 50.0 mL of 0.20 M NaOH(aq) to 50.0 mL of water. At 25.0°C, what is its pH? A) 1.00 B) 4.55 C) 7.00 D) 13.0 E) 13.3
What is the pH of a solution made by adding 10.0 mL of 0.10 M HCl to 25.0 mL of 0.10 M NH3? Kb of NH3 is 1.8 X 10-5.
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.040 M HCI. Ka of HF = 7.24 x 10-4. A 3.32 B.3.54 C.3.14 D.2.74 E 2.96
A 55.0 mL sample of 0.24 M HNO3 is titrated with 0.15 M C6H5NH2. Determine the pH at these points: a. At the beginning (before base is added) b. After adding 50.0 mL of C6H5NH2 c. After adding 75.0 mL of C6H5NH2 d. After adding 100.0 mL of C6H5NH2
1.) 160.0 mL of 0.24 M HF with 225.0 mL of 0.30 M NaF find pH 2.) 180.0 mL of 0.11 M C2H5NH2 with 275.0 mL of 0.21 M C2H5NH3Cl find pH 3.) Calculate the ratio of NaF to HF required to create a buffer with pH = 3.80. find [NaF][HF] = - My answer was 2.45 and it said it was wrong
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?