150.0 mL of 0.23 M HF with 220.0 mL of 0.31 M NaF
Calculate the pH of the solution that results from each of the following mixtures.
also, I'm so confused how you get the pKa..... can someone explain that part
pKa of HF=3.17
[HF]=(150*10^-3)*0.23=0.0345M
[NaF]=(220*10^-3)*0.31=0.0682M
pH=pKa+log[NaF]/[HF]=3.17+log(0.0682/0.0345)=3.46
150.0 mL of 0.23 M HF with 220.0 mL of 0.31 M NaF Calculate the pH of the...
what is the pH of the solution that results from 140mL of 0.23 M HF with 230.0 mL of 0.31 M NaF
Calculate the pH of the solution that results from each of the following mixtures. A. 140.0 mL of 0.27 M HF with 220.0 mL of 0.31 M NaF B. 170.0 mL of 0.12 M C2H5NH2 with 275.0 mL of 0.20 M C2H5NH3Cl
1) Calculate the pH of the solution that results from each of the following mixtures. A) 150.0 mL of 0.26 M HF with 225.0 mL of 0.32 M NaF B) 165.0 mL of 0.12 M C2H5NH2 with 275.0 mL of 0.22 M C2H5NH3Cl 2) A) As a technician in a large pharmaceutical research firm, you need to produce 100. mLof a potassium dihydrogen phosphate buffer solution of pH = 6.91. The pKa of H2PO4− is 7.21. You have the following...
Estimating pH 1. If you combine 40.0 mL of a 0.80 M HF solution with 60.0 mL of a 0.60 M NaF solution, which of the following is correct? HF pKa = 3.17. a) pH will be > 3.17 b) pH will be < 3.17 c) pH will equal 3.17 2. If 1.50 mL of 1.0 M HNO3 is added to a solution containing 40.0 mL of 0.80 M HF and 60.0 mL of 0.60 M NaF, what will happen...
Use the Henderson–Hasselbalch equation to calculate the pH of each solution: Part B a solution that contains 0.775% C5H5N by mass and 0.950% C5H5NHCl by mass. ( Express your answer using two decimal places.) Part C a solution that is 12.0 g of HF and 22.5 g of NaF in 125 mL of solution (Express your answer using two decimal places.) - Calculate the pH of the solution that results from each of the following mixtures. Part A4 150.0 mL...
29. E 2.- b. 125.0 mL of 0.10 M NH; WILT JUUM 16. Calculate the pH of the solution that results from each mixture. a. 150.0 mL of 0.25 M HF with 225.0 mL of 0.30 M NaF b. 175.0 mL of 0.10 M C H NH, with 275.0 mL of 0.20 M CH,NH4Cl 17. Calculate the ratio of NaF to HF required to create a buffer with pH = 4.00. IT YILC concentration
Calculate the pH at 25°C of 220.0 mL of a buffer solution that is 0.350 M NH4Cl and 0.350 M NH3 before and after the addition of 2.40 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75)
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
. (5 pts) The pKa of HF is 3.17. a) Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF. b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCI?
A 360.0 −mL buffer solution is 0.150 M in HF and 0.150 M in NaF. a) What mass of NaOH can this buffer neutralize before the pH rises above 4.00? = 1.6 b)If the same volume of the buffer were 0.370 M in HF and 0.370 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?