please help! will rate all. Calculate the pH of a solution prepared by mixing 2.50 L...

Question

Question

please help! will rate all.
Calculate the pH of a solution prepared by mixing 2.50 L of 2.35 M HF with 4.50 L of 1.56 M NaF

Answer 1

Answer #1

To find the pH of solution Given that 2.50L of 2.35M HF with 4.50L of 1.56M NaF Using the Henderson - Hasselbalch equation pH

Answer 2

Similar Homework Help Questions

1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M...

1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5 Calculate the pH of this solution of after the addition of 0.003 L of 0.200 M HCL 2. Consider a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5...
A buffer is prepared by mixing 75.0 mL of 0.40 M aqueous HF and 25.0 mL...

A buffer is prepared by mixing 75.0 mL of 0.40 M aqueous HF and 25.0 mL of 0.80 M aqueous NaF. At 25oC, Ka = 3.5 x 10-4 for HF. SHOW WORK (a). (4 points) Calculate the pH of the buffer. (b). (4 points) Your instructor accidentally dropped the bottle containing the buffer in part (a) in a bucket of water, that initially contained 4.00 L of water. What is the pH of the resulting solution?
HELP! Exam tomorrow!! Calculate the pH of a solution that is 2.00 M HF, 1.00 M...

HELP! Exam tomorrow!! Calculate the pH of a solution that is 2.00 M HF, 1.00 M NaOH, and 0.500M NaF n 1.00 L of the solution. Ka for HF = 7.2 x 10-4) HF(aq) + OH-(aq)-->F-(aq) + H2O(l) Correct answer is 3.32 really need help with the set up!! How many moles of solid NaF would have to be added to 1.0 L of 1.90 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume...

Calculate the pH of a buffer solution prepared by dissolving 1.79 mol of HF and 2.26...

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!
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and...

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
Calculate the pH of the solution prepared by mixing 20.00 mL of .217 M potassium monohydrogen pho...

calculate the pH of the solution prepared by mixing 20.00 mL of .217 M potassium monohydrogen phosphate with 35.00 mL of 0.1788 M trisodium phosphate. *please write out the net ionic formula, and all formulas and work* Thank you!

23) What is the pH of a solution prepared by mixing:

23) What is the pH of a solution prepared by mixing: 0.20 moles of acetic acid 0.40 moles of sodium acetate 0.10 moles of sodium hydroxide in 1.0 L of solution a) 4.74 b) 4.14 5.34 d) 13.00 e) None of the above 24) Barbituric acid (Ka = 9.8 X 10-5) is titrated with 0.200 M NaOH. What is the initial pH of 20.0 mL of 0.100 barbituric acida) 2.50 b) 4.01 c) 8.35 d) 7.00 e) None of the above 25) What is the pH in...
A solution is prepared by mixing 300.0 mL of 0.500M NaF to 100.0 mL of 0.200...

A solution is prepared by mixing 300.0 mL of 0.500M NaF to 100.0 mL of 0.200 M HF. Calculate the pH of the solution. Report your answer to two decimal places. Next page If the neutral ligand, L, in the following complex is a weak field ligand, identify the d-orbital electron configuration for the transition metal complex [RuL612+ Select one: cross out O O cross out o at 3 a. none of the choices b. t2g4eg? C. tzgega d. tzge94...
What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl...

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [Ka(HF) = 7.1 10–4] Group of answer choices 1.63 2.82 2.01 0.81

Calculate the pH of a solution that is prepared by dissolving 0.740 mol of hypochlorous acid...

Calculate the pH of a solution that is prepared by dissolving 0.740 mol of hypochlorous acid (HCIO, Ka = 3.00x10-8) and 0.254 mol of hydrofluoric acid (HF, K, = 6.60*10-4) in water and diluting to 4.50 L. Also, calculate the equilibrium concentrations of HCIO, CIO-, HF, and F. Do not make an approximation unless the initial acid concentration is greater than 1000 ~ Kg. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCIO]...