A)
Calculate the pH of 0.100L of a buffer solution that is 0.30 MM in HF and 0.45 MM in NaF.
Express your answer using three significant figures.
B)
Calculate pH of the solution on addition of the following.
0.004 mol of HNO3
Express your answer using three significant figures.
C)
Calculate pH of the solution on addition of the following.
0.002 mol of KOH
Express your answer using three significant figures.
A) Calculate the pH of 0.100L of a buffer solution that is 0.30 MM in HF...
a. Calculate the pH of 0.100 L of a buffer solution that is 0.29M in HF (Ka = 3.5 x 10-4 ) and 0.55M in NaF. - What is the pH after adding 0.004mol of HNO3 to the buffer described in Part A -What is the pH after adding 0.002mol of KOH to the buffer described in Part A?
Calculate the mole ratio of NaF to HF required to create a buffer with pH=4.10. Ka(HF)=6.3×10−4 Express your answer using two significant figures. [NaF][HF] = ??
1)Use the Henderson–Hasselbalch equation to calculate the pH of: a solution that is 13.5 g of HF and 25.0 g of NaF in 125 mL of solution Express your answer using two decimal places. 2) A volume of 20.0 mL of a 0.380 M HNO3 solution is titrated with 0.850 M KOH. Calculate the volume of KOH required to reach the equivalence point. Express your answer to three significant figures and include the appropriate units.
Part A Calculate the pH of 0.250 L of a 0.36 M formic acid-0.30 M sodium formate buffer. Express your answer using three significant figures. ΑΣΦ pH = > Submit Request Answer Part B After the addition of 0.0050 mol of NaOH. Assume that the volume remains constant Express your answer using three significant figures. VALO o ? pH = Submit Request Answer Part C After the addition of 0.0050 mol of HCl. Assume that the volume remains constant. Express...
A.) Calculate the pH of 0.100 L of a buffer solution that is 0.29M in HF (Ka = 3.5 x 10-4 ) and 0.55M in NaF. B.) What is the pH after adding 0.004mol of HNO3 to the buffer described in Part A? C.) What is the pH after adding 0.002mol of KOH to the buffer described in Part A?
1. Calculate the pH of a buffer: a) consisting of 0.600M HF and 0.750M NaF b) after the addition of 0.560g KOH (a strong base) to 1.00L of the buffer solution in part (a).
37. You have 500.0 mL of a buffer solution that is 0.30 M HF and 0.50 M KF. Ka for HF is 7.1 x 10-4 a) Calculate the pH of the buffer. b) Calculate the pH of the buffer after adding 0.020 moles of HCI. c) Calculate the pH of the buffer after adding 0.030 moles KOH. - -Loel.
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!
Using a 0.30 M phosphate buffer with a pH of 8.0, you add 0.70 mL of 0.55 M HCl to 52 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.30 M phosphate buffer with a pH of 8.0, you add 0.70 mL of 0.55 M NaOH to 52 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant...
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.72 mL of 0.54 M HCl to 60. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.72 mL of 0.54 M NaOH to 60. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)